Question

Each reaction is allowed to come to equilibrium, and then the volume is changed as indicated. Predict the effect (shift right, shift left, or no effect) of the indicated volume change. c. CaCO3(s) ⇌ CaO(s) + CO2(g) (volume is increased)

Accepted Answer

Identify the reaction type: The given reaction is a decomposition reaction where solid calcium carbonate (CaCO3) decomposes into solid calcium oxide (CaO) and gaseous carbon dioxide (CO2). Determine the effect of volume change on gases: Increasing the volume of the system decreases the pressure. According to Le Chatelier's principle, the system will adjust to counteract this change. Analyze the reaction's response to pressure change: In this reaction, the only gaseous product is CO2. Increasing the volume (and thus decreasing the pressure) will shift the equilibrium towards the side with more moles of gas. Count the moles of gases on each side of the equation: The reactant side has no gaseous moles, and the product side has one mole of CO2 gas. Predict the shift in equilibrium: Since increasing the volume favors the formation of more gas, the equilibrium will shift to the right, promoting the decomposition of CaCO3 to form more CO2.