Question

Consider the following equilibrium mixture in a closed system: H2O(g) + CO(g) ⇌ H2(g) + CO2(g). Explain what would happen to the equilibrium upon the addition of carbon monoxide gas?

Answer 1

Answer: The equilibrium will shift to the right direction i.e towards products.

Step-by-step explanation:

Any change in the equilibrium is studied on the basis of Le-Chatelier's principle. This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

For the given equation:

`H_2O(g)+CO(g)\leftrightharpoons H_2(g)+CO_2(g)`

Add more
`CO` gas

If the concentration of
`CO` that is the reactant is increased, so according to the Le-Chatlier's principle, the equilibrium will shift in the direction where decrease of concentration of
`CO` takes place. Therefore, the equilibrium will shift in the right direction i.e. towards the products.