The following reaction attains equilibrium at high temperature.
$N_{2} (g) + 2 H_{2} O (g) + h e a t ⇌ 2 N O (g) + 2 H 2 (g)$
The yield of NO is affected by:

increasing the nitrogen concentration

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decreasing the hydrogen concentration

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compressing the reactionmixture

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none of these

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Solution

The correct options are
A increasing the nitrogen concentration
B decreasing the hydrogen concentration
C compressing the reactionmixture
As concentration of reaction (gaseous) are increased at equilibrium, reaction will go in the forward direction. Also above reaction is endothermic therefore increase in temperature will favour it.

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Similar questions

N_{2} (g) + 2 H_{2} O (g) + heat ⇌ 2 N O (g) + 2 H_{2} (g)

N O

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

N O (g)

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

N O (g)

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

4.42 M^{- 2} s^{- 1}

[H_{2}] = 0.015 M

2 N O (g) + 2 H_{2} (g) = N_{2} (g) + 2 H_{2} O (g)

N O

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