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Question
The reaction, C2H6(g)⇌C2H4(g)+H2(g) is at equilibrium in a closed vessel at 1000 K. The enthalpy change (ΔH) for the reaction is 137.0 kJ.mol−1. Which one of the following actions would shift the equilibrium to the right?
The reaction, C2H6(g)⇌C2H4(g)+H2(g) is at equilibrium in a closed vessel at 1000 K. The enthalpy change (ΔH) for the reaction is 137.0 kJ.mol−1. Which one of the following actions would shift the equilibrium to the right?
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Solution
The correct option is B Increasing the volume of the closed reaction vessel
On decreasing the volume of reaction, a reaction will move in backward direction due to lesser number of moles.
On decreasing the temperature of reaction, the reaction will move in backward direction as the reaction is endothermic reaction.
Adding an inert gas does not result in a shift as there is no change in concentration.
Increasing the volume of reaction will shift the equilibrium in forward direction due to the higher number of moles or due to decrease in concentration.
On decreasing the volume of reaction, a reaction will move in backward direction due to lesser number of moles.
On decreasing the temperature of reaction, the reaction will move in backward direction as the reaction is endothermic reaction.
Adding an inert gas does not result in a shift as there is no change in concentration.
Increasing the volume of reaction will shift the equilibrium in forward direction due to the higher number of moles or due to decrease in concentration.
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