In the reaction $N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g)$ , the value of the equilibrium constant depends on :

the volume of the reaction vessel

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the total pressure of the system

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the initial concentration of nitrogen and hydrogen

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the temperature

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Solution

The correct option is C the temperature
Arrhenius equation-
$k = A e^{\frac{- E_{a}}{R T}}$
where,
$k =$ rate constant of a chemical reaction
$E_{a} =$ Activation energy.
$R =$ Universal gas constant
$A =$ Pre-exponential factor

From this, we can easily infer that the value of the equilibrium constant depends only on the temperature.

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Similar questions

In the reaction $N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g)$ , the value of the equilibrium

constant depends on

N_{2} (g) + 3 H_{2} (g) \Leftrightarrow 2 N H_{3} (g)

In the reaction $N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g)$ , the value of the equilibrium

constant depends on

1 M, 2 M,

15 M

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

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

K_{p}

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