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Consider the following reversible reaction at equilibrium.
$2 H_{2} O_{(g)} ⇌ 2 H_{2 (g)} + O_{2 (g)}; Δ H = 241.7 kJ$
Which one of the following changes in conditions will lead to maximum decomposition of $H_{2} O_{(g)}$

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Increasing both temperature and pressure

Decreasing temperature and increasing pressure

Increasing temperature and decreasing pressure

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 and value of $∆$ n = 3 - 2 = + 1 is positive so

it is forward with decrease in pressure

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