For which reactions will the position of equilibrium shift due to changing the volume of the container.

Question

BlackTom AI · Accepted Answer

Question restatement: The prompt asks which reactions will have their equilibrium position shift when the container volume is changed.

Option a: 'Only reactions where the number of moles of gas changes.' This is correct. According to Le Chatelier's principle, changing the volume affects the pressure of the system. A shift occurs only if the reaction involves a change in the number of gas moles (Δn_g ≠ 0). If the number of gas moles is unchanged, a volume change affects both sides proportionally and the position of equilibrium remains the same.

Option b: 'Only reactions which have less gaseous products than reactants.' This is misleading. The direction of the shift depends on Δn_g, not simply on whether products are fewer. Reactions with Δn_g > 0 or Δn_g < 0 can shift in different directions; the key is whether moles of gas change, not the relative amount of products vs reactants.

Option c: 'All reactions involving a gas.' This overstates the case. If there are gases but the total number of gas moles is the same on both sides (Δn_g = 0), changing the volume does not shift the equilibrium position.

Option d: 'Only reactions which have more gaseous products than reactants.' This is another mischaracterization. The driving factor is the change in moles of gas between sides (Δn_g), not whether products dominate numerically. Reactions with Δn_g ≠ 0 can shift in either direction depending on whether volume is increased or decreased.

Option e: 'All reactions where the number of moles change.' This is close but phrased broadly. The essential criterion is the change in the number of gas moles (gas-phase Δn_g ≠ 0). If the reaction involves gases but Δn_g = 0, there is no shift even though moles may change in a non-gaseous sense. The emphasis should be specifically on gas moles changing, not just any moles changing.

In summary, the correct interpretation is that equilibrium shifts with volume change only for reactions where the number of gas moles changes (Δn_g ≠ 0). The other options either misstate the dependence on Δn_g, misclassify cases with no net gas-mole change, or overgeneralize to all gas-involving reactions.

For which reactions will the position of equilibrium shift due to changing the volume of the container.单项选择题

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