The gas phase reaction shown is endothermic a written. Which, change(s) will increase the quantity of ${CH}_{3} CH = {CH}_{2}$ at equilibrium?
(P) Increasing the

(Q) Increasing the pressure
$H_{3} C - CH = {CH}_{2} ⇌$

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P only

Q only

Both P and Q

Neither P nor Q

answer is D.

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Detailed Solution

The gas phase reaction shown is endothermic a written. Both Does't will increase the quantity of ${CH}_{3} CH = {CH}_{2}$ at equilibrium?

$∵ Δ H > 0 .$ As $T ↑\Rightarrow Forward reaction$

$Δ n_{g} = 0$ So, $P ↑\Rightarrow No effect$

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