Consider the following reversible reaction at equilibrium, \[2{{H}_{2}}{{O}_{(g)}}\] ⇌ \[2{{H}_{2(g)}}+{{O}_{2(g)}}\]; \[\Delta H=241.7\,kJ\] Which one of the following changes in conditions will lead to maximum decomposition of \[{{H}_{2}}{{O}_{(g)}}\] [Kerala PMT 2004]

Increasing temperature at constant pressure

Increasing both temperature and pressure

Decreasing temperature and increasing pressure

Increasing temperature and decreasing pressure

Consider the following reversible reaction at equilibrium, \[2{{H}_{2}

1.	Consider the following reversible reaction at equilibrium, \[2{{H}_{2}}{{O}_{(g)}}\] ⇌ \[2{{H}_{2(g)}}+{{O}_{2(g)}}\]; \[\Delta H=241.7\,kJ\] Which one of the following changes in conditions will lead to maximum decomposition of \[{{H}_{2}}{{O}_{(g)}}\] [Kerala PMT 2004]
A.	Increasing both temperature and pressure
B.	Decreasing temperature and increasing pressure
C.	Increasing temperature and decreasing pressure
D.	Increasing temperature at constant pressure
Answer» D. Increasing temperature at constant pressure

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Consider the following reversible reaction at equilibrium, \[2{{H}_{2}}{{O}_{(g)}}\] ⇌ \[2{{H}_{2(g)}}+{{O}_{2(g)}}\]; \[\Delta H=241.7\,kJ\] Which one of the following changes in conditions will lead to maximum decomposition of \[{{H}_{2}}{{O}_{(g)}}\] [Kerala PMT 2004]

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