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

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

Quizplus · Accepted Answer

According to Le Chatelier's principle, when the volume is decreased, the equilibrium will shift in the direction that produces fewer moles of gas. In this case, CH4 has only one mole of gas, while C and H2S each have zero moles of gas, so decreasing the volume will shift the equilibrium to the right, favoring the formation of more CH4. Thus, choice C will result in a net reaction to the right to form more product. Adding He or more C will not affect the equilibrium because they are not part of the reaction. Increasing the volume will favor the formation of more gases, but there are no additional moles of gas on either side of the reaction, so it will not affect the equilibrium.

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