For the gas phase reaction, $C_{2} H_{4} ⇌ C_{2} H_{6} (Δ H = - 32.7 k c a l)$ carried out in a vessel the equilibrium concentration of $C_{2} H_{4}$ can be increased by-

Increasing the temperature.

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Decreasing the pressure.

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Removing some

H_{2}

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Adding some

C_{2} H_{6}

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Solution

The correct options are
A Increasing the temperature.
B Decreasing the pressure.
C Removing some $H_{2}$
D Adding some $C_{2} H_{6}$
The negative value of enthalpy change indicates that the forward reaction is exothermic.
When the temperature is increased, the reaction will proceed in the backward direction so that less heat is liberated which will nullify the effect of increased temperature.
The backward reaction proceeds with decrease in the number of moles from 1 to 2.
Hence, when the pressure is decreased, the reverse reaction is favored so that the number of moles and pressure increases .
When some hydrogen is removed or ethane is added, the equilibrium will shift to left. Thus in all these cases, the concentration of ethylene can be increased.

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