NEET Chemistry: Equilibrium PYQs Chapterwise Practice

Q 1 :
Higher yield of NO in

$N_{2 (g)} + O_{2 (g)} ⇌ 2 N O_{(g)}$ can be obtained at [ $Δ H of the reaction = + 180.7$ $kJ$ ${mol}^{- 1}$ ]

(A) higher temperature
(B) lower temperature
(C) higher concentration of $N_{2}$
(D) higher concentration of $O_{2}$

Choose the correct answer from the options given below: [2025]

B, C, D only
A, C, D only
A, D only
B, C only

1

2

3

4

(2)

$N_{2 (g)} + O_{2 (g)} ⇌ 2 {NO}_{(g)}; Δ H = + 180.7 kJ {mol}^{- 1}$

As the given reaction is endothermic, hence, it will go to the product side on increasing temperature. Also, on adding reactants, the reaction goes towards the product side.

Hence, conditions given in A, C, and D increase the production of ${NO}_{(g)}$ .

Q 2 :
For the reaction in equilibrium

$N_{2 (g)} + 3 H_{2 (g)} ⇌ 2 N H_{3 (g)}, Δ H = - Q$

Reaction is favoured in the forward direction by [2024]

use of catalyst
decreasing concentration of $N_{2}$
low pressure, high temperature and high concentration of ammonia
high pressure, low temperature and higher concentration of $H_{2}$

1

2

3

4

(4)

According to Le Chatelier’s principle:
(i) Raising the temperature shifts the equilibrium to the left and decreases the equilibrium concentration of ammonia. In other words, low temperature is favourable for high yield of ammonia, but practically very low temperatures slow down the reaction and thus a catalyst is used.

(ii) If $H_{2}$ is added to the reaction mixture at equilibrium, then the equilibrium of the reaction is disturbed. In order to restore it, the reaction proceeds in a direction wherein $H_{2}$ is consumed, i.e., more of $H_{2}$ and $N_{2}$ react to form $N H_{3}$ and finally the equilibrium shifts in the right (forward) direction.

(iii) As the pressure increases, the equilibrium shifts in the forward direction, a direction in which the number of moles of the gas decreases.

Q 3 :
Which one of the following conditions will favour maximum formation of the product in the reaction $A_{2 (g)} + B_{2 (g)} ⇌ X_{2 (g)}, Δ_{r} H = - X$ $kJ$ ? [2018]

Low temperature and high pressure
Low temperature and low pressure
High temperature and high pressure
High temperature and low pressure

1

2

3

4

(1)

On increasing the pressure and decreasing the temperature, equilibrium will shift in forward direction.

Q 4 :
For the reversible reaction,

$N_{2 (g)} + 3 H_{2 (g)} ⇌ 2 N H_{3 (g)} + h e a t$

The equilibrium shifts in the forward direction [2014]

by increasing the concentration of $N H_{3 (g)}$
by decreasing the pressure
by decreasing the concentrations of $N_{2 (g)}$ and $H_{2 (g)}$
by increasing pressure and decreasing temperature

1

2

3

4

(4)

As the forward reaction is exothermic and leads to lowering of pressure (produces lesser number of gaseous moles) hence, according to Le Chatelier’s principle, at high pressure and low temperature, the given reversible reaction will shift in forward direction to form more product.

Q 5 :
For a given exothermic reaction, $K_{p}$ and $K_{p}'$ are the equilibrium constants at temperatures $T_{1}$ and $T_{2}$ , respectively. Assuming that heat of reaction is constant in temperature range between $T_{1}$ and $T_{2}$ , it is readily observed that [2014]

$K_{p} > K_{p}'$
$K_{p} < K_{p}'$
$K_{p} = K_{p}'$
$K_{p} = \frac{1}{K_{p}'}$

1

2

3

4

(1)

$\log \frac{K'_{p}}{K_{p}} = - \frac{Δ H}{2.303 R} [\frac{1}{T_{2}} - \frac{1}{T_{1}}]$

For exothermic reaction, $Δ H = - ve$ , i.e., heat is evolved. The temperature $T_{2}$ is higher than $T_{1}$ .

Thus, $(\frac{1}{T_{2}} - \frac{1}{T_{1}})$ is negative.

So, $\log K'_{p} - \log K_{p} = - ve$ or $\log K_{p} > \log K'_{p}$

or $K_{p} > K'_{p}$

Topic Question Set

Q 2 :
For the reaction in equilibrium

$N_{2 (g)} + 3 H_{2 (g)} ⇌ 2 N H_{3 (g)}, Δ H = - Q$

Reaction is favoured in the forward direction by [2024]

Q 3 :
Which one of the following conditions will favour maximum formation of the product in the reaction $A_{2 (g)} + B_{2 (g)} ⇌ X_{2 (g)}, Δ_{r} H = - X$ $kJ$ ? [2018]

Q 4 :
For the reversible reaction,

$N_{2 (g)} + 3 H_{2 (g)} ⇌ 2 N H_{3 (g)} + h e a t$

The equilibrium shifts in the forward direction [2014]

Q 5 :
For a given exothermic reaction, $K_{p}$ and $K_{p}'$ are the equilibrium constants at temperatures $T_{1}$ and $T_{2}$ , respectively. Assuming that heat of reaction is constant in temperature range between $T_{1}$ and $T_{2}$ , it is readily observed that [2014]

Want Us to Email you About Special Offers & Updates?

Topic Question Set

Q 1 : Higher yield of NO in N2(g)+O2(g)⇌2NO(g) can be obtained at [ΔH of the reaction =+180.7 kJ mol-1] (A) higher temperature (B) lower temperature (C) higher concentration of N2 (D) higher concentration of O2 Choose the correct answer from the options given below: [2025]

Q 2 : For the reaction in equilibrium N2(g)+3H2(g)⇌2NH3(g), ΔH=-Q Reaction is favoured in the forward direction by [2024]

Q 3 : Which one of the following conditions will favour maximum formation of the product in the reaction A2(g)+B2(g)⇌X2(g), ΔrH=-X kJ ? [2018]

Q 4 : For the reversible reaction, N2(g)+3H2(g)⇌2NH3(g)+heat The equilibrium shifts in the forward direction [2014]

Q 5 : For a given exothermic reaction, Kp and Kp' are the equilibrium constants at temperatures T1 and T2, respectively. Assuming that heat of reaction is constant in temperature range between T1 and T2, it is readily observed that [2014]

Want Us to Email you About Special Offers & Updates?

Q 2 :
For the reaction in equilibrium

$N_{2 (g)} + 3 H_{2 (g)} ⇌ 2 N H_{3 (g)}, Δ H = - Q$

Reaction is favoured in the forward direction by [2024]

Q 3 :
Which one of the following conditions will favour maximum formation of the product in the reaction $A_{2 (g)} + B_{2 (g)} ⇌ X_{2 (g)}, Δ_{r} H = - X$ $kJ$ ? [2018]

Q 4 :
For the reversible reaction,

$N_{2 (g)} + 3 H_{2 (g)} ⇌ 2 N H_{3 (g)} + h e a t$

The equilibrium shifts in the forward direction [2014]

Q 5 :
For a given exothermic reaction, $K_{p}$ and $K_{p}'$ are the equilibrium constants at temperatures $T_{1}$ and $T_{2}$ , respectively. Assuming that heat of reaction is constant in temperature range between $T_{1}$ and $T_{2}$ , it is readily observed that [2014]