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Test: Chemical Equilibrium - 2


25 Questions MCQ Test Physical Chemistry | Test: Chemical Equilibrium - 2


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This mock test of Test: Chemical Equilibrium - 2 for Chemistry helps you for every Chemistry entrance exam. This contains 25 Multiple Choice Questions for Chemistry Test: Chemical Equilibrium - 2 (mcq) to study with solutions a complete question bank. The solved questions answers in this Test: Chemical Equilibrium - 2 quiz give you a good mix of easy questions and tough questions. Chemistry students definitely take this Test: Chemical Equilibrium - 2 exercise for a better result in the exam. You can find other Test: Chemical Equilibrium - 2 extra questions, long questions & short questions for Chemistry on EduRev as well by searching above.
QUESTION: 1

An example of a reversible reaction is:

Solution:
QUESTION: 2

Then the formation constant of [Ag(NH3)2]+ is:

Solution:
QUESTION: 3

Does Le-Chatelier’s principle predict a change of equilibrium concentrations for the following reaction if the gas mixture is compressed:

Solution:

N2​O4​(g)⇌2NO2​(g)

One mole of N2​O4​ 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

QUESTION: 4

The plot given below shows the relation between (1/T) and log(s), where S is the solubility of an electrolyte AB and T is the temperature in Kelvin. What conclusion can be drawn from the plot:
Solution:
QUESTION: 5

A mixture of 2 mole each of helium and an unknown gas (normal boiling point = 0°C) is kept in a 22.4 L flask. If the flask is cooled to 0.1°C, the resultant pressure (in atm) inside the flask is:           
Solution:
QUESTION: 6

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)           
Solution:

As we know that, Cr = 52, 
O3 = 16*3 = 48
CrO3 = 52 = 48
= 100 gm

QUESTION: 7

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:           
Solution:
QUESTION: 8

In a chemical reaction, 

The total pressure at equilibrium is 6 atm. The value of equilibrium constant is:
Solution:
QUESTION: 9

If the equilibrium constants for the reactions 1 and 2



Are K1 and K2, the equilibrium constant for the reaction
Solution:
QUESTION: 10

Consider the reaction, at equilibrium,

 The equilibrium can be shifted towards the forward direction by:
Solution:
QUESTION: 11

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:
Solution:
QUESTION: 12

If the equilibrium reaction  is heated, it is observed that the concentration of A increases. Then,
Solution:
QUESTION: 13

Consider the reaction:

The unit of the thermodynamic equilibrium constant for the reaction is:
Solution:

An equilibrium constant is defined to be equal to the ratio of the forward and backward reaction rate constants. This particular concentration quotient, , has the dimension of concentration, but the thermodynamic equilibrium constant, K, is always dimensionless.

QUESTION: 14

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 Kp under the same conditions will be
Solution:

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.

*Answer can only contain numeric values
QUESTION: 15

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.

Solution:

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

 

QUESTION: 16

The relationship between the equilibrium constant K1 for the reaction

And the equilibrium constant K2 for the reaction
Solution:
QUESTION: 17

The hydrolysis constant (Kh) of NH4Cl is 5.6×10–10. The concentration of H3O+ in a 0.1 M solution of NH4Cl at equilibrium is:
Solution:
QUESTION: 18

The equilibrium constant Kc for the following reaction at 842°C is 7.90 × 10–3. What is Kp at same temperature:
Solution:
QUESTION: 19

For the equilibrium what is the temperature at which

Solution:
QUESTION: 20

At a certain temperature, the following reactions have the equilibrium constants as shown below:

S(s) + O2(g) <=> SO2(g); Kc1 = 5 X 1052

2S(s) + 3O2(g) <=> 2SO3(g) ; Kc2 = 1029 

What is the equilibrium constant, Kc​ for the reaction at the same temperature?

SO2(g) + O2(g) <=> 2SO3(g)
Solution:

Equilibrium reactions depend upon the reaction equations

The Kc​ for the reaction is calculated as,

By the equation,

By reversing the first equation and doubling the coefficient Kc​

 

(KC,​)−1

Multiply both side of the equation  by K,

2.5×1076

 

 

QUESTION: 21

Consider the following gaseous equilibria given below

The equilibrium constant for the reaction, in terms of K1, K2 and K3 will be
Solution:

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

QUESTION: 22

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)
Solution:
QUESTION: 23

In a chemical reaction: xenon gas is added at constant volume. The equilibrium:
Solution:
QUESTION: 24

The equilibrium constants for the reactions   and   are K1 and K2, respectively. The equilibrium constant for the reaction  is
Solution:
QUESTION: 25

Correct statement on the effect of addition of aq. HCl on the equilibrium is:
Solution:

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