The effect on equilibrium position of a gas-phase reaction needs to be explained when there is a change in volume of the reaction vessel and whether there are reactions or not that will not shift their equilibria by change in volume needs to be determined. Also, the reason needs to be explained for no shift in equilibrium position for a gas-phase reaction in rigid container to which inert gases are added. Concept introduction: According to LeChatlier's principle, when a dynamic equilibrium is subjected to a change in either concentration or temperature or pressure, then the position of equilibrium will shift in such a direction that it nullifies the change. For example: A + B ⇌ C is a system at equilibrium. If concentration of A is increased by adding some more amount of A at equilibrium, then left side concentration is increasing, so to nullify this change, equilibrium shifts towards right side. Hence, forward reaction or formation of C is favoured in this case.

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Chapter 6, Problem 56E

Interpretation Introduction

Interpretation: The effect on equilibrium position of a gas-phase reaction needs to be explained when there is a change in volume of the reaction vessel and whether there are reactions or not that will not shift their equilibria by change in volume needs to be determined. Also, the reason needs to be explained for no shift in equilibrium position for a gas-phase reaction in rigid container to which inert gases are added.

Concept introduction: According to LeChatlier's principle, when a dynamic equilibrium is subjected to a change in either concentration or temperature or pressure, then the position of equilibrium will shift in such a direction that it nullifies the change.

For example:

A + B ⇌ C is a system at equilibrium.

If concentration of A is increased by adding some more amount of A at equilibrium, then left side concentration is increasing, so to nullify this change, equilibrium shifts towards right side. Hence, forward reaction or formation of C is favoured in this case.

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