Consider the following reversible reactionat equilibrium:
`2H_(2)O(g) hArr 2H_(2)(g)+O_(2)(g), DeltaH=+24.7 kJ`
Which one of the following changes in conditions will lead to maximum decomposition of `H_(2)O(g)`?

Options

A. Increasing both temeprature and pressure
B. Decreasing temperature and increasing pressure
C. Increasing temperature and decreasing pressure
D. Increasing temperature at constant pressure

Answer

C

Explanation

`2H_(2)O(g) hArr 2H_(2)(g)+O_(2)(g) , DeltaH =241.7 kJ`
Here, the forward reaction is endothermic and proceeds with an increase in number of moles of gaseous constituents, therefore, high temperature and low pressure will favour the forward reaction leading to maximum decomposition of `H_(2)O`