Chemical Equilibrium Test

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Chemical Equilibrium Test - 7

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Weekly Quiz Competition

Question 1
1 / -0

For a reaction A → B

The rate of the reaction is

A
1.6 × 10^–4

B
3.2 × 10^–4

C
−1.6 × 10^–4

D
reaction is at equilibrium

Solution

As concentration of product is not changing with time, the reaction is at equilibrium.
Question 2
1 / -0

The equilibrium constant for the reaction, N₂ (g) + O₂(g) ⇌ 2 NO (g) is 4 × 10^-4 at 2000 K. In presence of a catalyst, equilibrium is attained ten times faster. Therefore, the equilibrium constant, in presence of the catalyst, at 2000 K is

A
4 × 10^-3

B
4×10^-4

C
4×10^-5

D
difficult to compute without more data

Solution

A catalyst does not affect the value of Equilibrium constant ( K_eq) it only reduces the time of attainment of equilibrium. In fact, it does not even change the position of equilibrium.
Question 3
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In which of the following cases does the reaction go farthest to completion

A
K = 10³

B
K = 10^–2

C
K = 10

D
K = 1

Solution

Extent of reaction depends upon value of K_eq. Higher the K_eq higher is the extent of reaction.
Question 4
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For a reaction, N₂ + 3H₂ ⇌ 2NH₃ , the value of K_c would depend upon

A
initial concentration of the reactants

B
Pressure

C
temperature

D
all of the above

Solution

The equilibrium constant K_C of a reaction depends only on temperature and nature of reactants.
Question 5
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Which is not correct for an exothermic reaction

A

B

C

D

Solution

For exothermic Reaction ∆H° < 0hence slope > 0
Question 6
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For the given reaction, 2A (s) + B (g) ⇌ C (g) + 2D (s) + E (s) the degree of dissociation of B was found to be 20% at 300 K and 24% at 500 K. The rate of forward reaction

A
increases with increase in pressure and temperature.

B
increases with increase in pressure and decrease in temperature.

C
depends on temperature only and increases with increase in temperature.

D
increases with increasing the concentration of B and increasing the temperature.

Solution

As degree of dissociation, α increases with increase in temperature of reaction, the reaction is endothermic in nature. Therefore, on increase in temperature, Rate of forward reaction increases.

Also, ∆n_g = 0 for the reaction, pressure has no effect on equilibrium.
Question 7
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The gas A₂ in the left flask allowed to react with gas B₂ present in right flask as

A₂(g) + B₂ (g) ⇌ 2AB (g) ; K_c = 4 at 27°C

What is the concentration of AB when equilibrium is established?

A
1.33M

B
2.66M

C
0.66M

D
0.33M

Solution
Question 8
1 / -0

For the gas phase reaction, 2NO(g) ⇌ N₂ (g) + O₂ (g), ∆H = –43.5 kcal, which one of the following is true for N₂(g) + O₂(g) ⇌ 2NO(g)

A
K is independent of T

B
K decreases as T decreases

C
K increases as T decreases

D
K varies with addition of NO

Solution

The given reaction, N₂(g)+ O₂(g) ⇌ 2NO (G) is endothermic. Therefore, according to Le Chatelier’s principle, high temperature favours forward reaction and hence K increases as T increases or K decreases as T decreases.
Question 9
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The reactions, PCl₅ (g) ⇌ PCl₃ (g) + Cl₂ (g) and COCl₂ ⇌ CO (g) + Cl₂ (g) are simultaneously in equilibrium in an equilibrium box at constant volume. A few moles of CO(g) are later introduced into the vessel. After some time, the new equilibrium concentration of

A
PCl₅ will remain unchanged

B
PCl₃ will become less

C
PCl₅ will become less

D
COCl₂will become less

Solution

If some CO is added, the reaction (ii) will move in backward direction, this results in the decrease in concentration of Cl₂ and reaction (i) will move in forward 6 direction, hence concentration of PCl₅ will definitely decrease. Concentration of COCl₂ will increase and so will be the concentration of PCl₃.
Question 10
1 / -0

For the decomposition of PCl₅ g in a closed vessel, the degree of dissociation is 'x' at a total pressure 'P'.

Which among the following relations is correct?

A

B

C

D

Solution