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

constant depends on

Volume of the reaction vessel

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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 D
The temperature

The temperature is the only factor that can affect the value of Equilibrium constant.

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Similar questions

N_{2} (g) + 3 H_{2} (g) ⇌ 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

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

For the reaction

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

N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g); Δ H = - 22 k c a l

E_{a}

70 k c a l

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

k c a l

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