The reaction, $2 S O_{2} (g) + O_{2} (g) ⇌ 2 {S O}_{3} (g)$ (Exothermic), will shift in forward direction by:

adding

{S O}_{3}

at constant volume

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increasing volume of container

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adding

{S O}_{2}

at constant volume

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adding inert gas at constant volume

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Solution

The correct option is B adding ${S O}_{2}$ at constant volume
The given reaction is : $2 {S O}_{2 (g)} + O_{2 (g)} ⇌ 2 {S O}_{3 (g)}$ (Exothermic) by Le Chatelier's principle, addition of ${S O}_{2}$ at constant volume will favour the forward reaction.

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Similar questions

Q. Consider the following equilibrium system;

2 S O_{2 (g)} + O_{2 (g)} ⇌ 2 S O_{3 (g)}

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The reaction, 2SO2(g)+O2(g)⇌2SO3(g) (Exothermic), will shift in forward direction by:

The correct option is B adding SO2 at constant volumeThe given reaction is : 2SO2(g)+O2(g)⇌2SO3(g) (Exothermic) by Le Chatelier's principle, addition of SO2 at constant volume will favour the forward reaction.

The reaction, $2 S O_{2} (g) + O_{2} (g) ⇌ 2 {S O}_{3} (g)$ (Exothermic), will shift in forward direction by:

The correct option is B adding ${S O}_{2}$ at constant volume
The given reaction is : $2 {S O}_{2 (g)} + O_{2 (g)} ⇌ 2 {S O}_{3 (g)}$ (Exothermic) by Le Chatelier's principle, addition of ${S O}_{2}$ at constant volume will favour the forward reaction.