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.

Dashboard Chemical Equilibria

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

View Explanation

Log in for full answers

Similar Questions

Consider the following reaction at equilibrium. What effect will reducing the pressure of the reaction mixture have on the system? Xe(g) + 2 F2(g) XeF4(g)

In a consumer society, many adults channel creativity into buying things

Economic stress and unpredictable times have resulted in a booming industry for self-help products

People born without creativity never can develop it

A product has a selling price of $20, a contribution margin ratio of 40% and fixed cost of $120,000. To make a profit of $30,000. The number of units that must be sold is: Type the number without $ and a comma. Eg: 20000

Which of the following statement regarding cost is correct:

More Practical Tools for Students Powered by AI Study Helper

Homework AI Solver

Stylized AI Paper Writer

Plagiarism Checker Assistant

Citation AI Academic Writing Tool

In-Class Translation Assistant

AI Note Generator

AI Quiz Answers

Past Exam Questions from University Test Bank

Smart Practice Assistant

Adaptive Practice

Making Your Study Simpler