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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?

Respuesta :

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

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:

[tex]H_2O(g)+CO(g)\leftrightharpoons H_2(g)+CO_2(g)[/tex]

Add more [tex]CO[/tex] gas

If the concentration of [tex]CO[/tex] 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 [tex]CO[/tex] takes place. Therefore, the equilibrium will shift in the right direction i.e. towards the products.

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