Equilibrium constant, $K_{C}$ for the reaction at $500 K$ is $0.061$ . $N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g)$ . At a particular time, the analysis shows that composition of the reaction mixture is $3.0 m o l L^{- 1}$ $N_{2},$ $2.0 m o l L^{- 1} H_{2}$ and $0.5 m o l L^{- 1} N H_{3}$ . Is the reaction at equilibrium and if not in which direction does the reaction tend to proceed to reach equilibrium?

At equilibrium

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Not at equilibrium, backward shift

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Not at equilibrium, forward shift

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Can not be predicted

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Solution

The correct option is C Not at equilibrium, forward shift
The equilibrium reaction is shown below:
$N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g)$
The concentrations of nitrogen, hydrogen and ammonia are 3M, 2M and 0.5M respectively.
The expression for the reaction quotient is $Q = \frac{[N H_{3}]^{2}}{[N_{2}] [H_{2}]} = \frac{0.5 \times 0.5}{3 \times 2^{3}} = \frac{1}{3 \times 8} = 0.0104$ .
The value of the reaction quotient is smaller than the value of the equilibrium constant.

Hence, the reaction will progress in the forward direction so that the equilibrium is achieved. The reaction is not at equilibrium.

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Similar questions

Equilibrium constant, $K_{c}$ for the reaction.

$N_{2} (g) + 3 H_{2} (g \leftrightarrow 2 N H_{3} (g)$ at 500 K is 0.061.
At a particular time, the analysis shows that composition of the reaction mixture is 3.0 mol $L^{- 1} N_{2}, 2.0 m o l L^{- 1} H_{2}$ and 0.5 mol $L^{- 1} N H_{3}$ , Is the reaction at equilibrium? If not in which direction does the reaction tend to proceed to reach equilibrium?

Q. Equilibrium constant,

K_{C}

for the reaction

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

500 K

0.061

At a particular time, the analysis shows that composition of the reaction mixture is

3.0 m o l L^{- 1} N_{2}, 2.0 m o l L^{- 1} H_{2}

and

0.5 m o l L^{- 1} N H_{3} .

Is the reaction at equilibirium and if not in which direction does the reaction tend to proceed to reach equilibrium?

Equilibrium constant, K_c for the reaction

at 500 K is 0.061.

At a particular time, the analysis shows that composition of the reaction mixture is 3.0 mol L^–1 N₂, 2.0 mol L^–1 H₂ and 0.5 mol L^–1 NH₃. Is the reaction at equilibrium? If not in which direction does the reaction tend to proceed to reach equilibrium?

Q. Equilibrium constant,