Consider the following reaction at equilibrium. What effect will reducing the volume have on the system?

Question

Consider the following reaction at equilibrium. What effect will reducing the volume have on the system?

BlackTom AI · Accepted Answer

When a system at equilibrium is subjected to a volume decrease, the pressure rises and the system tends to counteract this change by shifting toward fewer gas moles.
In this reaction, count the gaseous species on each side: Left: C3H8(g) and O2(g) contribute 1 + 5 = 6 moles of gas. Right: CO2(g) contributes 3 moles of gas, while H2O(l) is a liquid and does not contribute to the gas-phase mole count. Thus, right side has 3 moles of gas.
Because the right side has fewer gas moles (3) than the left (6), the system will shift toward the products (the right) to reduce the total number of gas molecules and thereby lessen the pressure increase caused by the volume reduction.
This aligns with Le Chatelier’s principle: a decrease in volume (increase in pressure) favors the side with fewer gas moles. Temperature and enthalpy considerations are not directly invoked here, since the driving factor is the change in pressure/volume, not heat exchange.
Therefore, the direction of shift is toward the right, i.e., in the direction of the products.

Consider the following reaction at equilibrium. What effect will reducing the volume have on the system? 单项选择题

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