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Test: Chemical Equilibrium- 2

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

Description

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:

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)

Solution:

QUESTION: 2

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.

Solution:

QUESTION: 3

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

Solution:

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:

A.
Dissolution of AB is exothermic
B.
Dissolution of AB is endothermic
C.
Solubility of AB increases with temperature
D.
Nothing can be predicted.

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:

A.
1.0
B.
2.0
C.
3.0
D.
4.0

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)

A.
50 grams
B.
67 grams
C.
133 grams
D.
100 grams.

Solution:

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:

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

Solution:

QUESTION: 8

In a chemical reaction,

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

A.
1/2
B.
9
C.
1
D.
36

Solution:

QUESTION: 9

If the equilibrium constants for the reactions 1 and 2

Are K₁ and K₂, the equilibrium constant for the reaction

A.
K₁ + K₂
B.
K₁ – K₂
C.
K₁K₂
D.
K₁/K₂

Solution:

QUESTION: 10

Consider the reaction, at equilibrium,

The equilibrium can be shifted towards the forward direction by:

A.
Increasing the amount of carbon in the system
B.
Decreasing the volume of the system
C.
Decreasing the pressure of the system
D.
Increasing the temperature of system

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:

A.
2 mol L^–1
B.
1.2 mol L^–1
C.
0.5 mol L^–1
D.
0.4 mol L^–1

Solution:

QUESTION: 12

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

Solution:

QUESTION: 13

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

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 KpKp under the same conditions will be

A.
0.05
B.
50
C.
0.1
D.
25 RT

Solution:

*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