Constant temperature, the following reaction is at equilibrium in a closed container:
`C(s)+H_(2)O(g)hArr CO(g)+H_(2)(g)`
At constant pressure, if the amount of the solid carbon is reduced to half at equilibrium, then what will be the change in the concentration of CO(g)?

Explanation

At a particular temperature, the concentration of any pure solid is independent of its amount. Thus, keeping the temperature constant, if the amount of solid carbon is reduced to half at equilibrium, then its concentration will remain unchanged. So, the concentration of CO(g) will also remain unaffected.