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

Answer

C

Explanation

`DeltaH` is positive so reaction move forward by increase in temperature & value of `Deltan = 3 - 2 =-1` is positive so it forward with decrease in pressure.