For the reaction shown below,which change in conditions made to the system at equilibrium will result in a net reaction to the right to form more product? C(s)+ 2 H₂(g)⇌ CH₄(g)ΔH° = -74.8 kJ

Question

Quizplus · Accepted Answer

According to Le Chatelier's principle, when pressure is increased, the equilibrium will shift in the direction that produces fewer moles of gas. In this case, the forward reaction produces one mole of gas while the reverse reaction produces two moles of gas. Increasing the pressure will favor the forward reaction and produce more product. Therefore, increasing the pressure is the best choice to shift the equilibrium to the right and form more product.

For the Reaction Shown Below,which Change in Conditions Made to the System