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 hydrogen gas? The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the left which would result in more reactants being produced until equilibrium is achieved. The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the right which would result in more CO2 being produced until equilibrium is achieved. The addition of hydrogen gas would not disrupt the equilibrium, so nothing would happen.

Answer 1

Holg) + colg) H. (g) + CO₂ (g) Let 4 moles of the , & moles of co, a moles of H₂ and 8 moles of ca are present in 1 Livessel at equilibrium. Now, if we add 4 moles of the, a new equilibrium will be achieved as per below. Holg) + Colg) 2 Hz (9) + CO2(g) old equilibrium: 4 4 S : 4moles 4 6 8 T of h 84m odded atu new equilibrium 4th tt 8-n from the above, we can say that to compen- sate the added hydrogen, equilibrium shifts towards the reactant side and there is an increase of almol/L) of reactants at new equilübrium. Hence, option A is the correct answer.