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Consider the following reversible reaction at equilibrium,2H2O(g) ⇌ 2H2(g) + O2(g); ∆H=241.7 kJWhich one of the following changes in conditions will lead to maximum decomposition of H2O(g) ?

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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 is C.

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Detailed Solution

∆H is positive so reaction move forward by increase in temperature & value of ∆n = 3-2=+1 is positive so it forward with decrease in pressure.

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Consider the following reversible reaction at equilibrium,2H2O(g) ⇌ 2H2(g) + O2(g); ∆H=241.7 kJWhich one of the following changes in conditions will lead to maximum decomposition of H2O(g) ?