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Question: For the equilibrium \(2.37 \times 10^{- 3}\) ⇌ \(\lbrack N_{2}\rbrack = 2M,\lbrack H_{2}\rbrack = 3M...

For the equilibrium 2.37×10−32.37 \times 10^{- 3} ⇌ [N2]=2M,[H2]=3MNH3\lbrack N_{2}\rbrack = 2M,\lbrack H_{2}\rbrack = 3MNH_{3} the increase in temperature would.

A

Favour the formation of 0.60moll−10.60moll^{- 1}

B

Favour the decomposition of I2I_{2}

C

Not alter the equilibrium

D

Stop the reaction

Answer

Favour the decomposition of I2I_{2}

Explanation

Solution

The reaction is endothermic in reverse direction and hence increase in temperature will favour reverse reaction.