Le-Chatelier's Principle

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JEE Advanced 2015

LEVELJEE Advanced

The % yield of ammonia as a function of time in the reaction $N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g), Δ H < 0$ at $(P, T_{1})$ is given below - If this reaction is conducted at $(P, T_{2})$ , with $T_{2} > T_{1}$ , the % yield of ammonia as a function of time is represented by -

For the reaction, $2 SO_{2} (g) + O_{2} (g) ⟶ 2 SO_{3} (g)$ , $Δ H = - 57.2 kJ mol^{- 1}$ and $K_{c} = 1.7 \times 1 0^{16}$ . Which of the following statement is incorrect?

(A)

The equilibrium constant decreases as the temperature increases

(B)

The addition of inert gas at constant volume will not affect the equilibrium constant

(C)

The equilibrium will shift in forward direction as the pressure increases

(D)

The equilibrium constant is large suggestive of reaction going to completion and so no catalyst is required

JEE Main 2018

LEVELJEE Main

Which of the following lines correctly show the temperature dependence of equilibrium constant, $K$ , for an exothermic reaction?

Consider the following reaction : $N_{2} O_{4} (g) ⇌ 2 N O_{2} (g); Δ H^{\circ} = + 58 kJ$ For each of the following cases (A, B), the direction in which the equilibrium shifts is (A) temperature is decreased. (B) pressure is increased by adding $N_{2}$ at constant $T$ .

(A)

(A) towards product, (B) towards reactant

(B)

(A) towards reactant, (B) no change

(C)

(A) towards reactant, (B) towards product

(D)

(A) towards product, (B) no change

LEVELJEE Main

The exothermic formation of $ClF_{3}$ is represented by the equation $Cl_{2} (g) + 3 F_{2} (g) ⇌ 2 ClF_{3} (g)$ ; $Δ H_{r} = - 329 kJ$ Which of the following will increase the quantity of $ClF_{3}$ in an equilibrium mixture of $Cl_{2}$ , $F_{2}$ and $ClF_{3}$ ?

(A)

Adding

F_{2}

(B)

Increasing the volume of the container

(C)

Removing

Cl_{2}

(D)

Increasing the temperature

LEVELJEE Main

One of the following equilibria is not affected by change in volume of the flask

(A)

P C l_{5} (g) ⇌ P C l_{3} (g) + C l_{2} (g)

(B)

N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g)

(C)

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

(D)

S O_{2} C l_{2} (g) ⇌ S O_{2} (g) + C l_{2} (g)

.math-text-wrapper .katex { font-size: 1.05em !important; } .math-text-wrapper .katex-display { margin: 1rem 0 !important; } For the reaction, 2SO2​(g)+O2​(g)⟶2SO3​(g), ΔH=−57.2 kJ mol−1 and Kc​=1.7×1016. Which of the following statement is incorrect?

.math-text-wrapper .katex { font-size: 1.05em !important; } .math-text-wrapper .katex-display { margin: 1rem 0 !important; } Which of the following lines correctly show the temperature dependence of equilibrium constant, K, for an exothermic reaction?

One of the following equilibria is not affected by change in volume of the flask

For the reaction, $2 SO_{2} (g) + O_{2} (g) ⟶ 2 SO_{3} (g)$ , $Δ H = - 57.2 kJ mol^{- 1}$ and $K_{c} = 1.7 \times 1 0^{16}$ . Which of the following statement is incorrect?

Which of the following lines correctly show the temperature dependence of equilibrium constant, $K$ , for an exothermic reaction?