The following reaction has attained equilibrium
`CO(g)+2H_(2)(g)hArrCH_(3)OH(g)`. `DeltaH^(@)=-92.0KJmol^(-1)`
What will happen if
(i) Volume of the reaction vessel is suddenly reduced to half?
(ii) the partial pressure of hydrogen is suddenly doubled?
(iii) an inert gas is added to the system at constant volume.

Explanation

To solve the question regarding the equilibrium reaction \( \text{CO(g)} + 2\text{H}_2(g) \rightleftharpoons \text{CH}_3\text{OH}(g) \) with \( \Delta H^(@) = -92.0 \, \text{kJ/mol} \), we will analyze the effects of three different changes on the system.

### Step-by-Step Solution:

#### (i) Volume of the reaction vessel is suddenly reduced to half.

1. **Understanding the Effect of Volume Change**:
- When the volume of the reaction vessel is halved, the concentration of all gaseous species will double because concentration is inversely proportional to volume (i.e., \( C = \frac{n}{V} \)).
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