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An industrial fuel, 'water gas', which consists of a mixture of $H_{2}$ and CO can be made by passing team over red-hot carbon. The reaction is :
$C (s) + H_{2} O (g) ⇌ CO (g) + H_{2} (g), ΔH = + 131 kJ$
The yield of CO and $H_{2}$ at equilibrium would be shifted to the product side by :

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adding hot carbon without increasing temperature

raising the temperature

raising the relative pressure of the steam

reducing the volume of the system

answer is A, C.

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Detailed Solution

Raising the relative pressure of the steam and temperature cause the shifting the reaction in the right side.

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