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All questions of Chemical Equilibrium for Chemistry Exam
Can you explain the answer of this question below:Under the equilibrium condition for the reaction, 
the total pressure is 12 atm. The value of Kp is:
- A:
16
- B:
0.5
- C:
2
- D:
32
The answer is a.
Under the equilibrium condition for the reaction, the total pressure is 12 atm. The value of Kp is:
16
0.5
2
32
|
Aditya Deshmukh answered |
If 50% of CO2 reacts: C(s) + CO2(g) --> 2CO(g) P(total) = 12 atm If half the CO2 reacted then CO2 is x/2 and CO is x, and Pt = 12. Then x/2 + x = 12 1.5x = 12 x = 8 P(CO2) = 4 atm P(CO) = 8 atm The initial pressure of CO2 is 8 atm. When half of it reacts then 4 atm is left and the pressure of CO is twice as great, which is 8 atm. Kp = P(CO)^2 / P(CO2) Kp = 8^2 / 4 Kp = 16
Among the following, the equilibrium which is not affected by an increase in pressure is:- a)2SO3 (g) ⇔ 2SO2 (g) + O2 (g)
- b)H2 (g) + I2 (s) ⇔ 2HI (g)
- c)C(s) + H2O (g) ⇔ CO (g) + H2 (g)
- d)3Fe(s) + 4H2O (g) ⇔ Fe3O4 (s) + 4H2 (g)
Correct answer is option 'D'. Can you explain this answer?
Among the following, the equilibrium which is not affected by an increase in pressure is:
a)
2SO3 (g) ⇔ 2SO2 (g) + O2 (g)
b)
H2 (g) + I2 (s) ⇔ 2HI (g)
c)
C(s) + H2O (g) ⇔ CO (g) + H2 (g)
d)
3Fe(s) + 4H2O (g) ⇔ Fe3O4 (s) + 4H2 (g)
|
Vedika Singh answered |
As several moles of gaseous species are equal on both sides. Hence, for option (D), equilibrium is not affected by an increase in pressure.
the equilibrium constant Kp changes with:
Passage IIThe complex ion of Fe2+ with the chelating agent dipyridyl (abbreviated dipy) has been studied kinetically in both the forward and backward directions. For the complexion reaction,
the rate of the formation of the complex at 298 K is given by rate = (1. 45 x 1013 L3mol -3s-1) [Fe 2+] [dipy]3 and for the reverse reaction , the rate of disapperance of the complex is
Q. What is equilibrium constant for the equilibrium ? 
- a)8.4138x 10-18
- b)2.3770x 1017
- c)1.1885x 1017
- d)5.9426x 106
Correct answer is option 'C'. Can you explain this answer?
Passage II
The complex ion of Fe2+ with the chelating agent dipyridyl (abbreviated dipy) has been studied kinetically in both the forward and backward directions. For the complexion reaction,
the rate of the formation of the complex at 298 K is given by rate = (1. 45 x 1013 L3mol -3s-1) [Fe 2+] [dipy]3 and for the reverse reaction , the rate of disapperance of the complex is
Q. What is equilibrium constant for the equilibrium ?
a)
8.4138x 10-18
b)
2.3770x 1017
c)
1.1885x 1017
d)
5.9426x 106
|
Suresh Iyer answered |
The correct answer is Option C.
Fe2+ + 3 dipy -----> Fe(dipy)32+
Rf = Kf [Fe2+] [dipy]3
Rb = Kb [Fe(dipy)32+]
Keq = Kb [Fe(dipy)32+] / Kf [Fe2+] [dipy]3
Rf = Rb
Keq = Kf / Kb
= 1. 45 x 1013 / 1.24 x 10-4
= 1.885 x 1017
Fe2+ + 3 dipy -----> Fe(dipy)32+
Rf = Kf [Fe2+] [dipy]3
Rb = Kb [Fe(dipy)32+]
Keq = Kb [Fe(dipy)32+] / Kf [Fe2+] [dipy]3
Rf = Rb
Keq = Kf / Kb
= 1. 45 x 1013 / 1.24 x 10-4
= 1.885 x 1017
For the following gaseous phase equilibrium,
Kp is found to be equal to Kx (Kx is equilibrium constant when concentration are taken in terms of mole fraction. This is attained when pressure is - a)1 atm
- b)0.5 atm
- c)2 atm
- d)4 atm
Correct answer is option 'A'. Can you explain this answer?
For the following gaseous phase equilibrium,
Kp is found to be equal to Kx (Kx is equilibrium constant when concentration are taken in terms of mole fraction. This is attained when pressure is
Kp is found to be equal to Kx (Kx is equilibrium constant when concentration are taken in terms of mole fraction. This is attained when pressure is
a)
1 atm
b)
0.5 atm
c)
2 atm
d)
4 atm
|
Preeti Iyer answered |
The correct answer is Option A.
Kp = Equilibrium constant in terms of partial pressure
Kc = Equilibrium constant in terms of concentration
Kx = Equilibrium constant in terms of mole fraction
Kp = KcRTΔn ---(1)
Kp = K * (Pt)Δn ---(2)
a) 1 atm
Given PCl5 (g) ---> PCl3 (g) + Cl2 (g)
Δn = 2 – 1
Given Kp = Kx
From (2)
Kp = Kx when PT = 1
Kp = Equilibrium constant in terms of partial pressure
Kc = Equilibrium constant in terms of concentration
Kx = Equilibrium constant in terms of mole fraction
Kp = KcRTΔn ---(1)
Kp = K * (Pt)Δn ---(2)
a) 1 atm
Given PCl5 (g) ---> PCl3 (g) + Cl2 (g)
Δn = 2 – 1
Given Kp = Kx
From (2)
Kp = Kx when PT = 1
Q. What is [PCI5] eq?- a)4.09 x 10-4 mol L-1
- b)2.444 x 103 mol L-1
- c)4.09 x 10-6 mol L-1
- d)2.444 x 105 mol L-1
Correct answer is option 'A'. Can you explain this answer?
Q. What is [PCI5] eq?
a)
4.09 x 10-4 mol L-1
b)
2.444 x 103 mol L-1
c)
4.09 x 10-6 mol L-1
d)
2.444 x 105 mol L-1
|
Riya Banerjee answered |
The correct answer is Option A.
PPCl3 = [PCl3]RT
PCl2 = [Cl2]RT
PPCl3 = [PCl3]RT
PCl2 = [Cl2]RT
Ag+(aq)+NH3(aq) 
[Ag(NH3)(aq)]+ ; K, = 3.5x 10-3
[Ag(NH3)]+ (aq)+NH3(aq) [Ag(NH3)2]2+(aq); K2 = 1.7x 10-3
Formation constant of [Ag(NH3)2]+(aq) is- a)2.06
- b)5.2 x 10-3
- c)5.95 x 10-6
- d)None of these
Correct answer is option 'C'. Can you explain this answer?
Ag+(aq)+NH3(aq) [Ag(NH3)(aq)]+ ; K, = 3.5x 10-3
[Ag(NH3)]+ (aq)+NH3(aq)[Ag(NH3)2]2+(aq); K2 = 1.7x 10-3
Formation constant of [Ag(NH3)2]+(aq) is
[Ag(NH3)(aq)]+ ; K, = 3.5x 10-3[Ag(NH3)]+ (aq)+NH3(aq)
[Ag(NH3)2]2+(aq); K2 = 1.7x 10-3Formation constant of [Ag(NH3)2]+(aq) is
a)
2.06
b)
5.2 x 10-3
c)
5.95 x 10-6
d)
None of these
|
Krishna Iyer answered |
The correct answer is Option C.
To get the formation constant add both reactions-
So the resultant K = K1 × K2
= 3.5×1.7×10−3
= 5.95×10−6
To get the formation constant add both reactions-
So the resultant K = K1 × K2
= 3.5×1.7×10−3
= 5.95×10−6
Consider the following gaseous equilibria given below
The equilibrium constant for the reaction, 
in terms of K1, K2 and K3 will be- a)K1K2K3
- b)
- c)
- d)
Correct answer is option 'D'. Can you explain this answer?
Consider the following gaseous equilibria given below
The equilibrium constant for the reaction, in terms of K1, K2 and K3 will be
in terms of K1, K2 and K3 will bea)
K1K2K3
b)
c)
d)
|
Veda Institute answered |
Correct Answer :- d
Explanation : K1 = [NH3]2/[N2] [H2]3
K2 = [NO]2/[N2] [O2]3
K3 = [H2O]/[O2]1/2 [H2]
For the reaction :
K = {[NO]2 [H2O]3}/{[NH3]2 [O2]3/2}
= (K2 K33)/K1
For the reaction H2(g)+I2(g)⇌2HI (g) at 721 K
value of equilibrium constant is 50, when molar concentration of both hydrogen and iodine is 0.5 M at equilibrium value of KpKp under the same conditions will be- a)0.05
- b)50
- c)0.1
- d)25 RT
Correct answer is option 'B'. Can you explain this answer?
For the reaction H2(g)+I2(g)⇌2HI (g) at 721 K
value of equilibrium constant is 50, when molar concentration of both hydrogen and iodine is 0.5 M at equilibrium value of KpKp under the same conditions will be
value of equilibrium constant is 50, when molar concentration of both hydrogen and iodine is 0.5 M at equilibrium value of KpKp under the same conditions will be
a)
0.05
b)
50
c)
0.1
d)
25 RT
|
|
Vikram Kapoor answered |
The equilibrium reaction is H2(g)+I2(g)⇔2HI(g).
The relationship between Kp and Kc is Kp=Kc(RT)Δn.
For the equilibrium reaction, Δn=2−(1+1)=0.
Hence, Kp=Kc=50.
The relationship between Kp and Kc is Kp=Kc(RT)Δn.
For the equilibrium reaction, Δn=2−(1+1)=0.
Hence, Kp=Kc=50.
pH of a saturated solution of Ba(OH)2 is 12. The value of solubility product (Ksp) of Ba(OH)2 is- a)4.0 × 10–6
- b)5.0 × 10–6
- c)3.3 × 10–7
- d)5.0 × 10–7
Correct answer is option 'D'. Can you explain this answer?
pH of a saturated solution of Ba(OH)2 is 12. The value of solubility product (Ksp) of Ba(OH)2 is
a)
4.0 × 10–6
b)
5.0 × 10–6
c)
3.3 × 10–7
d)
5.0 × 10–7
|
Sagarika Patel answered |
pH + pOH = 14
pOH = 14 -12 =2 (given pH =12)
pOH = -log[OH-]
[OH-] = 10-pOH= 10-2....1
Ba(OH)2---> Ba+2+ 2OH-
At equilibrium:Ba+2= x andOH-= 2x
since 2x =10-2as eq. 1
therefore x = 10-2/2 = 0.5 * 10-2
ksp= [Ba+2]*[OH-]2= [0.5* 10-2][10-2]2= 0.5 *10-6=5 *10-7
is a gaseous phase equilibrium reaction taking place at 400 K in a 5 L flask. For this 
Does Le-Chatelier’s principle predict a change of equilibrium concentrations for the following reaction if the gas mixture is compressed:
- a)Yes, backward reaction is favoured
- b)Yes, forward reaction is favoured
- c)No change in equilibrium composition is predicted
- d)No information is obtained about concentration changes
Correct answer is option 'A'. Can you explain this answer?
Does Le-Chatelier’s principle predict a change of equilibrium concentrations for the following reaction if the gas mixture is compressed:
a)
Yes, backward reaction is favoured
b)
Yes, forward reaction is favoured
c)
No change in equilibrium composition is predicted
d)
No information is obtained about concentration changes
|
Asf Institute answered |
N2O4(g)⇌2NO2(g)
One mole of N2O4 gives 2 moles of NO2 gas. The pressure of the gas increases. Upon compressing the gaseous mixture, there is a change in an equilibrium concentration & backward reaction is favoured. This is according to Le Chatlier's Principle
When NaNO3 is heated in a closed vessel, oxygen is liberated and NaNO2 is left behind. At equilibrium.a)Addition of NaNO2 favours reverse reaction.b)Addition of NaNO3 favours forward reaction.c)Increasing temperature favours forward reaction.d)Increasing pressure favours reverse reaction.Correct answer is option 'C,D'. Can you explain this answer?
|
Mrinalini Sen answered |
Since NaNo3 and NaNo2 are in solid state change in concentration doesn't affect the equilibrium.
9.2 grams of N2O4(g) is taken in a closed on litre vessel and heated till the following equilibrium is reached
At equilibrium, 50% N2O4(g) is dissociated. What is the equilibrium constant (in mol litre–1) (molecular weight of N2O4 = 92)- a)0.1
- b)0.4
- c)0.2
- d)2
Correct answer is option 'C'. Can you explain this answer?
9.2 grams of N2O4(g) is taken in a closed on litre vessel and heated till the following equilibrium is reached
At equilibrium, 50% N2O4(g) is dissociated. What is the equilibrium constant (in mol litre–1) (molecular weight of N2O4 = 92)
a)
0.1
b)
0.4
c)
0.2
d)
2
|
Nepal Dey answered |
For the complete oxidation of 100 g of Cyclohexanol to cyclohexanon, the quantity of CrO3 required is (assuming 100% chemical yield) [Atomic wt. of Cr = 52) - a)50 grams
- b)67 grams
- c)133 grams
- d)100 grams.
Correct answer is option 'D'. Can you explain this answer?
For the complete oxidation of 100 g of Cyclohexanol to cyclohexanon, the quantity of CrO3 required is (assuming 100% chemical yield) [Atomic wt. of Cr = 52)
a)
50 grams
b)
67 grams
c)
133 grams
d)
100 grams.
|
|
Vedika Singh answered |
As we know that, Cr = 52,
O3 = 16*3 = 48
CrO3 = 52 = 48
= 100 gm
O3 = 16*3 = 48
CrO3 = 52 = 48
= 100 gm
The concentration of the oxides of nitrogen are monitored in air-pollution reports. At 25°C, the equilibrium constant for the reaction,
is 1.3 x 106 and that for 
is 6.5 x 10-16 (when each species is expressed in terms of partial pressure).
For the reaction,
equilibrium constant is- a)
- b)
- c)
- d)
Correct answer is option 'A'. Can you explain this answer?
The concentration of the oxides of nitrogen are monitored in air-pollution reports. At 25°C, the equilibrium constant for the reaction,
is 1.3 x 106 and that for
is 6.5 x 10-16 (when each species is expressed in terms of partial pressure).
For the reaction,
equilibrium constant is
a)
b)
c)
d)
|
Crafty Classes answered |
Given equations are
NO (g) + ½ O2 (g) ⇌ NO2 (g) ----------(i) k1 = 1.3×106
And ½ N2 (g) + ½ O2 (g) ⇌ NO(g) ----------(ii) k2 = 6.5×10-16
To get the reaction, N2(g) + 2O2(g) ⇌ 2NO2(g) ----------(iii) k3
We multiply eqn (i) and eqn (ii) by 2 and adding both reaction, we get eqn (iii)
k3 = k12×k22
= (1.3×106)2×(6.5×10-16)2
= 1.69×1012×42.25×10-32
= 7.14×10-19
NO (g) + ½ O2 (g) ⇌ NO2 (g) ----------(i) k1 = 1.3×106
And ½ N2 (g) + ½ O2 (g) ⇌ NO(g) ----------(ii) k2 = 6.5×10-16
To get the reaction, N2(g) + 2O2(g) ⇌ 2NO2(g) ----------(iii) k3
We multiply eqn (i) and eqn (ii) by 2 and adding both reaction, we get eqn (iii)
k3 = k12×k22
= (1.3×106)2×(6.5×10-16)2
= 1.69×1012×42.25×10-32
= 7.14×10-19
For the reaction, 
if Kp = Kc (RT)X, when the symbols have usual meaning, the value of x is (assuming ideality)[jee Main 2014]- a)-1
- b)-1/2
- c)+1/2
- d)+1
Correct answer is option 'B'. Can you explain this answer?
For the reaction,
if Kp = Kc (RT)X, when the symbols have usual meaning, the value of x is (assuming ideality)
if Kp = Kc (RT)X, when the symbols have usual meaning, the value of x is (assuming ideality)
[jee Main 2014]
a)
-1
b)
-1/2
c)
+1/2
d)
+1
|
Gaurav Kumar answered |
The correct answer is Option B.
SO2(g) + 1/2O2(g) ⇌ SO3(g)
KP = KC(RT)Δn
SO2(g) + 1/2O2(g) ⇌ SO3(g)
KP = KC(RT)Δn
Δn= no. of gaseous moles of product minus no. of gaseous moles of reactant
Δn = 1−1−1/2
∴Δn = −1/2
Δn = 1−1−1/2
∴Δn = −1/2
For the following equilibrium, N2O4 (g) 
2NO2(g)Kp = KC. This is attained when- a)T = 1.0K
- b)T = 12.18 K
- c)T = 27.3 K
- d)T = 273 K
Correct answer is option 'B'. Can you explain this answer?
For the following equilibrium, N2O4 (g) 2NO2(g)
2NO2(g)Kp = KC. This is attained when
a)
T = 1.0K
b)
T = 12.18 K
c)
T = 27.3 K
d)
T = 273 K
|
|
Riya Banerjee answered |
The correct answer is option B
KP=KC(RT)Δn
Δn=1
KP=KC(RT)
RT=1
T=1/R=1/0.0821=12.18
KP=KC(RT)Δn
Δn=1
KP=KC(RT)
RT=1
T=1/R=1/0.0821=12.18
For the reaction:
At a given temperature, the equilibrium amount of CO2(g) can be increased by.- a)Adding a suitable catalyst
- b)Adding an inert gas
- c)Decreasing the volume of the container
- d)Increasing the amount of CO(g)
Correct answer is option 'D'. Can you explain this answer?
For the reaction:
At a given temperature, the equilibrium amount of CO2(g) can be increased by.
a)
Adding a suitable catalyst
b)
Adding an inert gas
c)
Decreasing the volume of the container
d)
Increasing the amount of CO(g)
|
Bhawesh answered |
According to the Le chatlier principle if a constraint (such as a change in pressure, temperature, or concentration of a reactant) is applied to a system in equilibrium, the equilibrium will shift so as to tend to counteract the effect of the constraint. Here if we increase the concentration of CO more CO2 will be formed.
Pure ammonia is placed in a vessel at a temperature where its dissociation constant (α) is appreciable. At equilibrium,
- a)Kp does not change significantly with pressure.
- b)α Does not change with pressure.
- c)Concentration of NH3 does not change with pressure.
- d)Concentration of hydrogen is less than that of nitrogen.
Correct answer is option 'A'. Can you explain this answer?
Pure ammonia is placed in a vessel at a temperature where its dissociation constant (α) is appreciable. At equilibrium,
a)
Kp does not change significantly with pressure.
b)
α Does not change with pressure.
c)
Concentration of NH3 does not change with pressure.
d)
Concentration of hydrogen is less than that of nitrogen.
|
Dheeraj Verma answered |
KP only affected by change in temperature
the equilibrium constant Kp changes with:
At constant temperature, the equilibrium (Kp) for the decomposition reaction
is expressed by 
where, p = pressure,X = extent of decomposition. Which one of the following statement is true:a)Kp Increases with increase of pb)KpIncreases with increase of xc)KpIncreases with decrease of xd)KpRemains constant with change in p and x
Correct answer is option 'D'. Can you explain this answer?
is expressed by where, p = pressure,X = extent of decomposition. Which one of the following statement is true:
|
Aryan Choudhary answered |
Kp is a characteristic constant for a given reaction and changes only with temperature.
A 2 L vessel containing 2g of H2 gas at 27°C is connected to a 2L vessel containing 176 g of CO2 gas at 27°C. Assuming ideal behaviour of H2 and CO2, the partial pressure of H2 at equilibrium is………bar.
Correct answer is '6.25'. Can you explain this answer?
A 2 L vessel containing 2g of H2 gas at 27°C is connected to a 2L vessel containing 176 g of CO2 gas at 27°C. Assuming ideal behaviour of H2 and CO2, the partial pressure of H2 at equilibrium is………bar.
|
Raghav Rane answered |
H2 + CO2 - mixture of non-reacting gases
2g H2 = 1 mol
176g CO2 = 4 mol
Total no. of moles = 5
Total volume = 2+2 = 4L
Temperature = 27+273 = 300K
Total pressure, P=nRT/V=(5*0.083*300/4)= 31.125 bar
According to Dalton's law, p1 = P*(x1)
Mole fraction of H2=1/(1+4)=1/5
Therefore, p(H2)= 31.125*0.2 = 6.225 bar
2g H2 = 1 mol
176g CO2 = 4 mol
Total no. of moles = 5
Total volume = 2+2 = 4L
Temperature = 27+273 = 300K
Total pressure, P=nRT/V=(5*0.083*300/4)= 31.125 bar
According to Dalton's law, p1 = P*(x1)
Mole fraction of H2=1/(1+4)=1/5
Therefore, p(H2)= 31.125*0.2 = 6.225 bar
Select the correct statement (s) about the following equilibrium.
- a)At constant vapour pressure, number of molecules leaving the liquid equals the number returning to liquid from vapour
- b)This does not represent the static equilibrium
- c)This represents dynamic equilibrium and the rate of the forward and backward reactions become equal
- d)This represents dynamic as well as static equilibrium
Correct answer is option 'A,B,C'. Can you explain this answer?
Select the correct statement (s) about the following equilibrium.
a)
At constant vapour pressure, number of molecules leaving the liquid equals the number returning to liquid from vapour
b)
This does not represent the static equilibrium
c)
This represents dynamic equilibrium and the rate of the forward and backward reactions become equal
d)
This represents dynamic as well as static equilibrium
|
Lavanya Menon answered |
The correct answers are Options A, B and C.
During constant vapor pressure the no of molecules of H2O leaving the surface = the no of H2O molecules coming to the surface from the atmosphere. This process is dynamic as there is continuous movement of molecules.
During constant vapor pressure the no of molecules of H2O leaving the surface = the no of H2O molecules coming to the surface from the atmosphere. This process is dynamic as there is continuous movement of molecules.
Direction (Q. Nos. 1-12) This section contains 12 multiple choice questions. Each question has four choices (a), (b), (c) and (d), out of which ONLY ONE option is correct.
Q.Conversion factor for converting partial pressures (in Kp) to active masses (in Kc) is- a)nRT
- b)1/RT
- c)(RT)2
- d)1/RT2
Correct answer is option 'B'. Can you explain this answer?
Direction (Q. Nos. 1-12) This section contains 12 multiple choice questions. Each question has four choices (a), (b), (c) and (d), out of which ONLY ONE option is correct.
Q.Conversion factor for converting partial pressures (in Kp) to active masses (in Kc) is
a)
nRT
b)
1/RT
c)
(RT)2
d)
1/RT2
|
Hansa Sharma answered |
Kp = kc(RT)∆ng
So to convert kp to kc we have, kc = kp(1/RT)∆ng.
So, the converting factor is 1/RT
So to convert kp to kc we have, kc = kp(1/RT)∆ng.
So, the converting factor is 1/RT
When a reversible reaction 
is followed with time with initial concentration of A being 0.6 mol. L–1, the following graph is obtained:
The equilibrium constant K, for the above reaction is:- a)2 mol L–1
- b)1.2 mol L–1
- c)0.5 mol L–1
- d)0.4 mol L–1
Correct answer is option 'B'. Can you explain this answer?
When a reversible reaction is followed with time with initial concentration of A being 0.6 mol. L–1, the following graph is obtained:
is followed with time with initial concentration of A being 0.6 mol. L–1, the following graph is obtained:The equilibrium constant K, for the above reaction is:
a)
2 mol L–1
b)
1.2 mol L–1
c)
0.5 mol L–1
d)
0.4 mol L–1
|
Jyoti Sharma answered |
Equilibrium arrives at 0.3 mol/l and take stoichiometry of b as 2
For the chemical reaction,
The amount of X3 Y at equilibrium is affected by- a)Temperature and pressure
- b)Temperature only
- c)Pressure only
- d)Temperature, pressure and catalyst
Correct answer is option 'A'. Can you explain this answer?
For the chemical reaction,
The amount of X3 Y at equilibrium is affected by
a)
Temperature and pressure
b)
Temperature only
c)
Pressure only
d)
Temperature, pressure and catalyst
|
Srishti Kulkarni answered |
There are 3 main factors that affect the equilibrium of a reaction:
- Concentration of reactants or products
- Temperature
- Pressure (Affects only gaseous reactions)
Then the formation constant of [Ag(NH3)2]+ is:- a)6.08 × 10–6
- b)6.08 × 106
- c)6.08 × 10–9
- d)None of these.
Correct answer is option 'D'. Can you explain this answer?
Then the formation constant of [Ag(NH3)2]+ is:
a)
6.08 × 10–6
b)
6.08 × 106
c)
6.08 × 10–9
d)
None of these.
|
Shoaib Ali answered |
If u add those equation than k1 and k2 goes in multiply, so u get 5.95 × 10^-6
Direction (Q. Nos. 21) Choice the correct combination of elements and column I and coloumn II are given as option (a), (b), (c) and (d), out of which ONE option is correct.The progress of the reaction 
with time t is shown below.
Match the parameters in Column l with their respective values in Column II.
Codes
- a)a
- b)b
- c)c
- d)d
Correct answer is option 'A'. Can you explain this answer?
Direction (Q. Nos. 21) Choice the correct combination of elements and column I and coloumn II are given as option (a), (b), (c) and (d), out of which ONE option is correct.
The progress of the reaction with time t is shown below.
Match the parameters in Column l with their respective values in Column II.
Codes
with time t is shown below.Match the parameters in Column l with their respective values in Column II.
Codes
a)
a
b)
b
c)
c
d)
d
|
|
Rajesh Gupta answered |
The correct answer is Option A.
Loss in concentration of A in I hour = 
= 0.1
Gain in concentration of B in I hour =
0.2
(i) ∵0.1 mole of A changes to 0.2 mole of B in a given time and thus, n=2
(ii) Equilibrium constant,
= 1.2mollitre−1
(iii) Initial rate of conversion of A = changes in conc. of A during I hour =
= 0.1 mol litre−1hour−1
(iv) ∵ Equilibrium is attained after 5 hr, where [B]=0.6 and [A]=0.3
= 0.1Gain in concentration of B in I hour =
0.2(i) ∵0.1 mole of A changes to 0.2 mole of B in a given time and thus, n=2
(ii) Equilibrium constant,
= 1.2mollitre−1(iii) Initial rate of conversion of A = changes in conc. of A during I hour =
= 0.1 mol litre−1hour−1
(iv) ∵ Equilibrium is attained after 5 hr, where [B]=0.6 and [A]=0.3
For the reaction in equilibrium, A 
B
Thus, K is- a)
- b)
- c)
- d)
Correct answer is option 'B'. Can you explain this answer?
For the reaction in equilibrium, A B
Thus, K is
BThus, K is
a)
b)
c)
d)
|
Sushil Kumar answered |
From the reaction
-d[A]/dt = d[B] /dt
⇒2.3 × 106 [A] = k [B]
as given in question [B] /[A] = 4 × 108
so [A] / [B] = 1/ 4 ×108
⇒ 2.3 × 106 . [A] /[B] = k
⇒ 2.3 × 106 / 4 × 108 = k
Or k = 5.8 × 10-3 /sec¹
-d[A]/dt = d[B] /dt
⇒2.3 × 106 [A] = k [B]
as given in question [B] /[A] = 4 × 108
so [A] / [B] = 1/ 4 ×108
⇒ 2.3 × 106 . [A] /[B] = k
⇒ 2.3 × 106 / 4 × 108 = k
Or k = 5.8 × 10-3 /sec¹
An example of a reversible reaction is:- a)Pb(NO3)2 (aq) + 2NaI (aq) = PbI2(s) + 2NaNO3(aq)
- b)AgNO3(aq) + HCl(aq) = AgCl(s) + HNO3(aq)
- c)2Na(s) + 2H2O(l) = 2NaOH(aq) + H2(g)
- d)KNO3(aq) + NaCl(aq) = KCl(aq) + NaNO3(aq)
Correct answer is option 'D'. Can you explain this answer?
An example of a reversible reaction is:
a)
Pb(NO3)2 (aq) + 2NaI (aq) = PbI2(s) + 2NaNO3(aq)
b)
AgNO3(aq) + HCl(aq) = AgCl(s) + HNO3(aq)
c)
2Na(s) + 2H2O(l) = 2NaOH(aq) + H2(g)
d)
KNO3(aq) + NaCl(aq) = KCl(aq) + NaNO3(aq)
|
Avinash Mehta answered |
Weak acids and bases may undergo reversible reactions. For example, carbonic acid and water react this way:
H2CO3 (l) + H2O(l) ⇌ HCO−3 (aq) + H3O+(aq)
Another example of a reversible reaction is:
N2O4 ⇆ 2 NO2
Two chemical reactions occur simultaneously:
N2O4 → 2 NO2
2 NO2 → N2O4
Reversible reactions do not necessarily occur at the same rate in both directions, but they do lead to an equilibrium condition. If dynamic equilibrium occurs, the product of one reaction is forming at the same rate as it is used up for the reverse reaction. Equilibrium constants are calculated or provided to help determine how much reactant and product is formed.
The equilibrium of a reversible reaction depends on the initial concentrations of the reactants and products and the equilibrium constant, K.
The units of KP and KC are equal.- a)true
- b)flase
Correct answer is option 'B'. Can you explain this answer?
The units of KP and KC are equal.
a)
true
b)
flase
|
|
Vivek Khatri answered |
The units of KP are (atm)Δng and the units of KC are (mol/L)Δng. Where Δng = moles of products – moles of reactants which are in the gaseous state only. As the units of KP and KC are not equal the above statement is considered to be false.
For the reaction:
the equilibrium constant at 2000 K and 1.0 bar is 5.25. When the pressure is increased by 8-fold, the equilibrium constant: - a)Increases by a factor of 1.86
- b)Decreases by a factor of 1.86
- c)Remains same
- d)Increases by factor of 8
Correct answer is option 'C'. Can you explain this answer?
For the reaction: the equilibrium constant at 2000 K and 1.0 bar is 5.25. When the pressure is increased by 8-fold, the equilibrium constant:
the equilibrium constant at 2000 K and 1.0 bar is 5.25. When the pressure is increased by 8-fold, the equilibrium constant: a)
Increases by a factor of 1.86
b)
Decreases by a factor of 1.86
c)
Remains same
d)
Increases by factor of 8
|
Monika Yadav answered |
Correct answer is 'c' .
because Keq is only affected by temperature and stoichiometry of reaction. not affected by other factors.
because Keq is only affected by temperature and stoichiometry of reaction. not affected by other factors.
Consider the following equilibrium in a closed container
At a fixed temperature, the volume of the reaction container is halved. For this change, which of the following statements hold true regarding the equilibrium constant (Kp) and degree of dissociation (α)?- a)Neither nor change
- b)Both and change
- c)change but does not change
- d)does not change but change
Correct answer is option 'D'. Can you explain this answer?
Consider the following equilibrium in a closed container
At a fixed temperature, the volume of the reaction container is halved. For this change, which of the following statements hold true regarding the equilibrium constant (Kp) and degree of dissociation (α)?
a)
Neither nor change
b)
Both and change
c)
change but does not change
d)
does not change but change
|
Ramandeep Singh answered |
Basically kp depends on temperature only change in volume doesn't influence it.however degree of dissociation depends upon volume ...so it will change on changing volume.so the answer is ....when the volume of reaction container is halved,equilibrium constant doesn't change but degree of dissociation change.....
Br2(l) ⇌ Br2(g) is in ________- a)homogeneous equilibrium
- b)not in both Homogeneous and heterogeneous equilibrium
- c)cannot say
- d)may or may not be in Homogeneous equilibrium
Correct answer is option 'B'. Can you explain this answer?
Br2(l) ⇌ Br2(g) is in ________
a)
homogeneous equilibrium
b)
not in both Homogeneous and heterogeneous equilibrium
c)
cannot say
d)
may or may not be in Homogeneous equilibrium
|
|
Vandana Gupta answered |
Explanation:
Homogeneous and Heterogeneous Equilibrium:
- In a chemical reaction, equilibrium is a state in which the forward and reverse reactions occur at equal rates.
- A homogeneous equilibrium refers to a reaction in which all the reactants and products are in the same phase (either all gases, all liquids, or all solids).
- A heterogeneous equilibrium refers to a reaction in which the reactants and products are in different phases (such as a gas and a solid, or a liquid and a solid).
The given reaction:
- The given reaction is Br2(l) ⇌ Br2(g).
- Here, the reactant (Br2) is a liquid and the product (Br2) is a gas.
- Since the reactant and product are in different phases (liquid and gas), the reaction is in a heterogeneous equilibrium.
Answer:
- The correct answer is option 'B' - the reaction is not in both homogeneous and heterogeneous equilibrium.
- As explained above, the reaction is in a heterogeneous equilibrium due to the different phases of the reactant and product.
- It is important to note that a reaction can only be in either a homogeneous or a heterogeneous equilibrium, not both at the same time.
Summary:
- The given reaction Br2(l) ⇌ Br2(g) is in a heterogeneous equilibrium because the reactant and product are in different phases. Therefore, the correct answer is option 'B'.
Homogeneous and Heterogeneous Equilibrium:
- In a chemical reaction, equilibrium is a state in which the forward and reverse reactions occur at equal rates.
- A homogeneous equilibrium refers to a reaction in which all the reactants and products are in the same phase (either all gases, all liquids, or all solids).
- A heterogeneous equilibrium refers to a reaction in which the reactants and products are in different phases (such as a gas and a solid, or a liquid and a solid).
The given reaction:
- The given reaction is Br2(l) ⇌ Br2(g).
- Here, the reactant (Br2) is a liquid and the product (Br2) is a gas.
- Since the reactant and product are in different phases (liquid and gas), the reaction is in a heterogeneous equilibrium.
Answer:
- The correct answer is option 'B' - the reaction is not in both homogeneous and heterogeneous equilibrium.
- As explained above, the reaction is in a heterogeneous equilibrium due to the different phases of the reactant and product.
- It is important to note that a reaction can only be in either a homogeneous or a heterogeneous equilibrium, not both at the same time.
Summary:
- The given reaction Br2(l) ⇌ Br2(g) is in a heterogeneous equilibrium because the reactant and product are in different phases. Therefore, the correct answer is option 'B'.
At constant temperature, the pressure is directly proportional to the concentration of the gas.- a)true
- b)false
Correct answer is option 'A'. Can you explain this answer?
At constant temperature, the pressure is directly proportional to the concentration of the gas.
a)
true
b)
false
|
|
Vivek Khatri answered |
We have P = CRT e where p is pressure, R is a universal constant and T is the temperature, we derive the equation from the ideal gas equation PV=nRT. So from P = CRT, we can say that at a constant temperature the pressure is directly proportional to the concentration of the gas.
Which is correct statement if N2 is added at equilibrium condition?
- a)The equilibrium will shift to forward direction because according to IInd law of thermodynamics the entropy must increases in the direction of spontaneous reaction.
- b)The condition for equilibrium is G(N2)+3G(H2)=2G (NH3) where, G is Gibbs free energy per mole of the gaseous species measured at that partial pressure. The condition of equilibrium is unaffected by the use of catalyst, which increases the rate of both the forward and backward reactions to the same extent.
- c)The catalyst will increases the rate of forward reaction by α and that of backward reaction by β
- d)Catalyst will not alter the rate of either of the reaction.
Correct answer is option 'B'. Can you explain this answer?
Which is correct statement if N2 is added at equilibrium condition?
a)
The equilibrium will shift to forward direction because according to IInd law of thermodynamics the entropy must increases in the direction of spontaneous reaction.
b)
The condition for equilibrium is G(N2)+3G(H2)=2G (NH3) where, G is Gibbs free energy per mole of the gaseous species measured at that partial pressure. The condition of equilibrium is unaffected by the use of catalyst, which increases the rate of both the forward and backward reactions to the same extent.
c)
The catalyst will increases the rate of forward reaction by α and that of backward reaction by β
d)
Catalyst will not alter the rate of either of the reaction.
|
|
Anisha Pillai answered |
Increasing the collision frequency and lowering the activation energy, but will not affect the position of equilibrium.
d)The equilibrium will shift to the left because the addition of N2 will increase the concentration of reactants and decrease the concentration of products, favoring the reverse reaction.
d)The equilibrium will shift to the left because the addition of N2 will increase the concentration of reactants and decrease the concentration of products, favoring the reverse reaction.
WHat is the expression of KC of the chemical equation Ag2O(s) + 2HNO3(aq) ⇌ 2AgNO3(aq) +H2O(l)?- a)[AgNO3(aq)]2/[HNO3(aq)]2
- b)[AgNO3(aq)]/[HNO3(aq)]2
- c)[AgNO3(aq)]2/[HNO3(aq)]
- d)[AgNO(aq)]2/[HNO3(aq)]2
Correct answer is option 'A'. Can you explain this answer?
WHat is the expression of KC of the chemical equation Ag2O(s) + 2HNO3(aq) ⇌ 2AgNO3(aq) +H2O(l)?
a)
[AgNO3(aq)]2/[HNO3(aq)]2
b)
[AgNO3(aq)]/[HNO3(aq)]2
c)
[AgNO3(aq)]2/[HNO3(aq)]
d)
[AgNO(aq)]2/[HNO3(aq)]2
|
|
Anshul Mehra answered |
Explanation:
The expression for the equilibrium constant (Kc) of a chemical equation is obtained by taking the concentration of the products raised to the power of their stoichiometric coefficients and dividing it by the concentration of the reactants raised to the power of their stoichiometric coefficients.
In the given chemical equation:
Ag2O(s) + 2HNO3(aq) → 2AgNO3(aq) + H2O(l)
The stoichiometric coefficients of the products are 2 for AgNO3(aq) and 1 for H2O(l), while the stoichiometric coefficients of the reactants are 2 for Ag2O(s) and 2 for HNO3(aq).
Therefore, the expression for Kc is as follows:
Kc = [AgNO3(aq)]^2 / [HNO3(aq)]^2
Reasoning:
To determine the correct expression for Kc, we need to consider the stoichiometry of the reaction. The stoichiometric coefficients in the balanced equation indicate the ratio of reactants and products in the reaction.
In this case, since 2 moles of AgNO3(aq) are produced for every 2 moles of HNO3(aq) consumed, the concentration of AgNO3(aq) should be squared in the expression for Kc.
Similarly, since 2 moles of AgNO3(aq) are produced for every 2 moles of HNO3(aq) consumed, the concentration of HNO3(aq) should also be squared in the expression for Kc.
Conclusion:
Therefore, the correct expression for Kc is [AgNO3(aq)]^2 / [HNO3(aq)]^2, which is option 'A'. This expression takes into account the stoichiometry of the reaction and correctly represents the equilibrium constant for the given chemical equation.
The expression for the equilibrium constant (Kc) of a chemical equation is obtained by taking the concentration of the products raised to the power of their stoichiometric coefficients and dividing it by the concentration of the reactants raised to the power of their stoichiometric coefficients.
In the given chemical equation:
Ag2O(s) + 2HNO3(aq) → 2AgNO3(aq) + H2O(l)
The stoichiometric coefficients of the products are 2 for AgNO3(aq) and 1 for H2O(l), while the stoichiometric coefficients of the reactants are 2 for Ag2O(s) and 2 for HNO3(aq).
Therefore, the expression for Kc is as follows:
Kc = [AgNO3(aq)]^2 / [HNO3(aq)]^2
Reasoning:
To determine the correct expression for Kc, we need to consider the stoichiometry of the reaction. The stoichiometric coefficients in the balanced equation indicate the ratio of reactants and products in the reaction.
In this case, since 2 moles of AgNO3(aq) are produced for every 2 moles of HNO3(aq) consumed, the concentration of AgNO3(aq) should be squared in the expression for Kc.
Similarly, since 2 moles of AgNO3(aq) are produced for every 2 moles of HNO3(aq) consumed, the concentration of HNO3(aq) should also be squared in the expression for Kc.
Conclusion:
Therefore, the correct expression for Kc is [AgNO3(aq)]^2 / [HNO3(aq)]^2, which is option 'A'. This expression takes into account the stoichiometry of the reaction and correctly represents the equilibrium constant for the given chemical equation.
One mole of N2O4(g) at 300 K is kept in a closed container under one atmosphere. It is heated to 600 K when 20% by mass of N2O4(g) decomposes to NO2(g). The resultant pressure is:- a)1.2 atm
- b)2.4 atm
- c)2.0 atm
- d)1.0 atm
Correct answer is option 'B'. Can you explain this answer?
One mole of N2O4(g) at 300 K is kept in a closed container under one atmosphere. It is heated to 600 K when 20% by mass of N2O4(g) decomposes to NO2(g). The resultant pressure is:
a)
1.2 atm
b)
2.4 atm
c)
2.0 atm
d)
1.0 atm
|
|
Vivek Khatri answered |
N2O4 → 2NO2
moles of unreacted N2O4 = 1 (1 - 0.2) = 0.8
moles of NO2 = 2 * 0.2 = 0.4
- - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - (+)
total moles n2 = 0.8 + 0.4 = 1.2
P1/(T1 n1) = P2/(T2 * n2)
1/(300 * 1) = P2/(600 * 1.2)
P2 = 2.4 atm
moles of unreacted N2O4 = 1 (1 - 0.2) = 0.8
moles of NO2 = 2 * 0.2 = 0.4
- - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - (+)
total moles n2 = 0.8 + 0.4 = 1.2
P1/(T1 n1) = P2/(T2 * n2)
1/(300 * 1) = P2/(600 * 1.2)
P2 = 2.4 atm
If KC of a reaction N2(g) + O2(g) ⇌ 2NO(g) is 2 x 10-3, then what is the KP?- a)4 x 10-3
- b)1 x 10-3
- c)3 x 10-3
- d)2 x 10-3
Correct answer is option 'D'. Can you explain this answer?
If KC of a reaction N2(g) + O2(g) ⇌ 2NO(g) is 2 x 10-3, then what is the KP?
a)
4 x 10-3
b)
1 x 10-3
c)
3 x 10-3
d)
2 x 10-3
|
Saanvi Roy answered |
To determine the value of KP, the equation relating KP and KC needs to be used. The equation is:
KP = KC(RT)^(Δn)
Where:
KP is the equilibrium constant in terms of partial pressures
KC is the equilibrium constant in terms of concentrations
R is the ideal gas constant
T is the temperature in Kelvin
Δn is the difference in the number of moles of gas between the products and reactants
In this reaction, the balanced equation is:
N2(g) + O2(g) ⇌ 2NO(g)
The reaction involves 2 moles of gas on the left side (N2 and O2) and 2 moles of gas on the right side (2NO). Therefore, Δn = 2 - 2 = 0.
Given that KC = 2 x 10^-3, we can use the equation to solve for KP:
KP = KC(RT)^Δn
Since Δn = 0, the equation simplifies to:
KP = KC
Substituting the given value of KC, we get:
KP = 2 x 10^-3
Therefore, the correct answer is option 'D', which is 2 x 10^-3.
KP = KC(RT)^(Δn)
Where:
KP is the equilibrium constant in terms of partial pressures
KC is the equilibrium constant in terms of concentrations
R is the ideal gas constant
T is the temperature in Kelvin
Δn is the difference in the number of moles of gas between the products and reactants
In this reaction, the balanced equation is:
N2(g) + O2(g) ⇌ 2NO(g)
The reaction involves 2 moles of gas on the left side (N2 and O2) and 2 moles of gas on the right side (2NO). Therefore, Δn = 2 - 2 = 0.
Given that KC = 2 x 10^-3, we can use the equation to solve for KP:
KP = KC(RT)^Δn
Since Δn = 0, the equation simplifies to:
KP = KC
Substituting the given value of KC, we get:
KP = 2 x 10^-3
Therefore, the correct answer is option 'D', which is 2 x 10^-3.
If the equilibrium reaction 
is heated, it is observed that the concentration of A increases. Then,- a)A must be a gas
- b)Either B or C must be solid
- c)The reaction is exothermic
- d)The reaction is endothermic
Correct answer is option 'C'. Can you explain this answer?
If the equilibrium reaction is heated, it is observed that the concentration of A increases. Then,
is heated, it is observed that the concentration of A increases. Then,a)
A must be a gas
b)
Either B or C must be solid
c)
The reaction is exothermic
d)
The reaction is endothermic
|
|
Ramandeep Singh answered |
Basically when temperature increases,the reactant A utilizes the heat and decomposes into B and C...leading to endothermic reaction( in which heat is utilized)..
However in above case it is given that when temperature increases,concentration of A increase,it means that A is not utilizing the heat to proceed a forward reaction .....
so reaction comes to be exothermic....so correct option is C.
However in above case it is given that when temperature increases,concentration of A increase,it means that A is not utilizing the heat to proceed a forward reaction .....
so reaction comes to be exothermic....so correct option is C.
The equilibrium N2(g) + O2(g) ⇌ 2NO(g), is an example of _____________- a)homogeneous chemical equilibrium
- b)heterogeneous chemical equilibrium
- c)neither homogeneous nor heterogeneous
- d)both homogeneous and heterogeneous
Correct answer is option 'A'. Can you explain this answer?
The equilibrium N2(g) + O2(g) ⇌ 2NO(g), is an example of _____________
a)
homogeneous chemical equilibrium
b)
heterogeneous chemical equilibrium
c)
neither homogeneous nor heterogeneous
d)
both homogeneous and heterogeneous
|
|
Vivek Khatri answered |
In homogeneous equilibrium, the reactants and products are present in the same phase or physical state. Nitrogen, Oxygen, and nitrogen monoxide are present in a gaseous state, so it is homogeneous chemical equilibrium.
CO2(g) + C(s) ⇌ 2CO(g) is an example of _____________- a)homogeneous equilibrium
- b)heterogeneous equilibrium
- c)neither homogeneous nor heterogeneous
- d)both homogeneous and heterogeneous
Correct answer is option 'B'. Can you explain this answer?
CO2(g) + C(s) ⇌ 2CO(g) is an example of _____________
a)
homogeneous equilibrium
b)
heterogeneous equilibrium
c)
neither homogeneous nor heterogeneous
d)
both homogeneous and heterogeneous
|
|
Ameya Reddy answered |
Heterogeneous equilibrium
In a chemical reaction, the reactants and products can be either in the same phase (homogeneous) or in different phases (heterogeneous). The given reaction: CO2(g) + C(s) ⇌ 2CO(g) involves reactants and products in different phases, which makes it an example of a heterogeneous equilibrium.
Explanation:
Definition:
A heterogeneous equilibrium is a type of chemical equilibrium in which the reactants and products of a reaction are present in different phases.
Reactant and Product Phases:
In the given reaction, CO2(g) is a gas, C(s) is a solid, and 2CO(g) is also a gas. The reactants and products are present in different phases: gas and solid. Therefore, the reaction is an example of a heterogeneous equilibrium.
Visual Representation:
CO2(g) + C(s) ⇌ 2CO(g)
Interpretation:
The forward reaction involves the reactant CO2(g) and solid C(s) to produce 2CO(g) as products. The reverse reaction involves the reactant 2CO(g) to produce CO2(g) and C(s) as products.
Phase Change:
In the forward reaction, the reactant CO2(g) is a gas and the reactant C(s) is a solid. During the reaction, the solid carbon (C) combines with the gaseous carbon dioxide (CO2) to form gaseous carbon monoxide (CO). This phase change from solid to gas and gas to solid indicates a heterogeneous equilibrium.
Presence of Different Phases:
The presence of different phases (gas and solid) in the reactants and products of the reaction indicates a heterogeneous equilibrium. This means that the reaction does not occur entirely in one phase, but involves a mixture of phases.
Therefore, the given reaction CO2(g) + C(s) ⇌ 2CO(g) is an example of a heterogeneous equilibrium.
In a chemical reaction, the reactants and products can be either in the same phase (homogeneous) or in different phases (heterogeneous). The given reaction: CO2(g) + C(s) ⇌ 2CO(g) involves reactants and products in different phases, which makes it an example of a heterogeneous equilibrium.
Explanation:
Definition:
A heterogeneous equilibrium is a type of chemical equilibrium in which the reactants and products of a reaction are present in different phases.
Reactant and Product Phases:
In the given reaction, CO2(g) is a gas, C(s) is a solid, and 2CO(g) is also a gas. The reactants and products are present in different phases: gas and solid. Therefore, the reaction is an example of a heterogeneous equilibrium.
Visual Representation:
CO2(g) + C(s) ⇌ 2CO(g)
Interpretation:
The forward reaction involves the reactant CO2(g) and solid C(s) to produce 2CO(g) as products. The reverse reaction involves the reactant 2CO(g) to produce CO2(g) and C(s) as products.
Phase Change:
In the forward reaction, the reactant CO2(g) is a gas and the reactant C(s) is a solid. During the reaction, the solid carbon (C) combines with the gaseous carbon dioxide (CO2) to form gaseous carbon monoxide (CO). This phase change from solid to gas and gas to solid indicates a heterogeneous equilibrium.
Presence of Different Phases:
The presence of different phases (gas and solid) in the reactants and products of the reaction indicates a heterogeneous equilibrium. This means that the reaction does not occur entirely in one phase, but involves a mixture of phases.
Therefore, the given reaction CO2(g) + C(s) ⇌ 2CO(g) is an example of a heterogeneous equilibrium.
For the following equation, 2HBr(g) ⇌ H2(g) + Br2(g); are both KP and KC are equal?- a)yes
- b)cannot say
- c)no
- d)depends on the temperature
Correct answer is option 'A'. Can you explain this answer?
For the following equation, 2HBr(g) ⇌ H2(g) + Br2(g); are both KP and KC are equal?
a)
yes
b)
cannot say
c)
no
d)
depends on the temperature
|
|
Vivek Khatri answered |
We have here KC = [H2][Br2]/[HBr]2; KP = [pH2][pBr2]/[pHBr]2, where pH2 = [H2]RT, pBr2 = [Br2]RT and [pHBr] = [HBr]RT. So in this case as Δng = 0, where Δng = moles of products – moles of reactants which are in gaseous state only, both KP and KC are equal.
Consider the reaction: 
The unit of the thermodynamic equilibrium constant for the reaction is:- a)mol L–1
- b)L mol–1
- c)mol2L–2
- d)Dimensionless
Correct answer is option 'D'. Can you explain this answer?
Consider the reaction:
The unit of the thermodynamic equilibrium constant for the reaction is:
a)
mol L–1
b)
L mol–1
c)
mol2L–2
d)
Dimensionless
|
Prachi Dwivedi answered |
As equilibrium constant i.e K(eq) is itself the ratio of 2other rate constant i.e K(forward) and K(backward)so it is unit less .
When two reactants, A and B are mixed to give products, C and D, the reaction quotient, (Q) at the initial stages of the reaction:- a)Is zero
- b)Decreases with time
- c)Is independent of time
- d)Increases with time
Correct answer is option 'D'. Can you explain this answer?
When two reactants, A and B are mixed to give products, C and D, the reaction quotient, (Q) at the initial stages of the reaction:
a)
Is zero
b)
Decreases with time
c)
Is independent of time
d)
Increases with time
|
|
Juhi Sen answered |
The reaction quotient (Q) and its relation to reactants and products
The reaction quotient (Q) is a measure of the relative concentrations of reactants and products in a chemical reaction at any given point in time. It is calculated in the same way as the equilibrium constant (K), but it is determined using the concentrations of reactants and products at any moment during the reaction, rather than at equilibrium.
Initial stages of the reaction
In the initial stages of a reaction, before equilibrium is reached, the concentrations of reactants are typically higher compared to the concentrations of products. This is because the reaction has just started, and the products have not had enough time to form in significant amounts. As a result, the value of Q in the initial stages of the reaction is generally smaller than the equilibrium constant, K.
Understanding the options
a) Is zero: This option is incorrect because it implies that no products are formed at the initial stages of the reaction, which is not true. Some products will be present, although in smaller amounts compared to the reactants.
b) Decreases with time: This option is also incorrect because the value of Q does not necessarily decrease with time. It depends on the specific reaction and the rate at which reactants are converted to products.
c) Is independent of time: This option is incorrect because Q changes with time as the reaction progresses. Initially, Q will be smaller than K, but as the reaction proceeds, Q will approach the value of K.
d) Increases with time: This option is the correct answer. As the reaction progresses, reactants are consumed, and products are formed. This leads to an increase in the concentrations of products and a decrease in the concentrations of reactants. Consequently, the value of Q increases with time and approaches the value of K as equilibrium is approached.
Conclusion
In summary, the reaction quotient (Q) at the initial stages of a reaction is smaller than the equilibrium constant (K). As the reaction progresses, Q increases with time and approaches the value of K. The correct answer to the given question is option 'D'.
The reaction quotient (Q) is a measure of the relative concentrations of reactants and products in a chemical reaction at any given point in time. It is calculated in the same way as the equilibrium constant (K), but it is determined using the concentrations of reactants and products at any moment during the reaction, rather than at equilibrium.
Initial stages of the reaction
In the initial stages of a reaction, before equilibrium is reached, the concentrations of reactants are typically higher compared to the concentrations of products. This is because the reaction has just started, and the products have not had enough time to form in significant amounts. As a result, the value of Q in the initial stages of the reaction is generally smaller than the equilibrium constant, K.
Understanding the options
a) Is zero: This option is incorrect because it implies that no products are formed at the initial stages of the reaction, which is not true. Some products will be present, although in smaller amounts compared to the reactants.
b) Decreases with time: This option is also incorrect because the value of Q does not necessarily decrease with time. It depends on the specific reaction and the rate at which reactants are converted to products.
c) Is independent of time: This option is incorrect because Q changes with time as the reaction progresses. Initially, Q will be smaller than K, but as the reaction proceeds, Q will approach the value of K.
d) Increases with time: This option is the correct answer. As the reaction progresses, reactants are consumed, and products are formed. This leads to an increase in the concentrations of products and a decrease in the concentrations of reactants. Consequently, the value of Q increases with time and approaches the value of K as equilibrium is approached.
Conclusion
In summary, the reaction quotient (Q) at the initial stages of a reaction is smaller than the equilibrium constant (K). As the reaction progresses, Q increases with time and approaches the value of K. The correct answer to the given question is option 'D'.
Direction (Q. Nos. 15-18) This section contains a paragraph, wach describing theory, experiments, data etc. three Questions related to paragraph have been given.Each question have only one correct answer among the four given options (a),(b),(c),(d)Passage IAt 573 K, PCI5 dissociates as,
PCI5 (g) ⇔ PCI3(g)+ Cl2 (g), Kp= 11.5 atm
Given, [PCI3]eq, = [Cl2]eq = 0.01 mol L-1
Q.
Kc of this equilibrium is- a)2.444 x 10-3
- b)4.09
- c)4.09 x 102
- d)0.244 mol L-1
Correct answer is option 'D'. Can you explain this answer?
Direction (Q. Nos. 15-18) This section contains a paragraph, wach describing theory, experiments, data etc. three Questions related to paragraph have been given.Each question have only one correct answer among the four given options (a),(b),(c),(d)
Passage I
At 573 K, PCI5 dissociates as,
PCI5 (g) ⇔ PCI3(g)+ Cl2 (g), Kp= 11.5 atm
Given, [PCI3]eq, = [Cl2]eq = 0.01 mol L-1
PCI5 (g) ⇔ PCI3(g)+ Cl2 (g), Kp= 11.5 atm
Given, [PCI3]eq, = [Cl2]eq = 0.01 mol L-1
Q.
Kc of this equilibrium is
Kc of this equilibrium is
a)
2.444 x 10-3
b)
4.09
c)
4.09 x 102
d)
0.244 mol L-1
|
Maheshwar Malik answered |
Method to Solve :
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