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For a particular equilibrium mixture, the temperature is lowered and the amount of ClF₃ changes by 0.010 mol - VCE - SSCE Chemistry - Question 10 - 2003 - Paper 1
Question 10
For a particular equilibrium mixture, the temperature is lowered and the amount of ClF₃ changes by 0.010 mol. The changes occurring would be: | | ClF₃ ... show full transcript
Worked Solution & Example Answer:For a particular equilibrium mixture, the temperature is lowered and the amount of ClF₃ changes by 0.010 mol - VCE - SSCE Chemistry - Question 10 - 2003 - Paper 1
Step 1
ClF₃ changes by 0.010 mol
Answer
According to Le Chatelier's principle, lowering the temperature will favor the exothermic direction of the reaction. If the reaction producing ClF₃ is exothermic, we would expect the equilibrium to shift to the right, resulting in the consumption of ClF₃. Therefore, the change in ClF₃ should be a decrease by 0.010 mol.
Step 2
Determine the changes in F₂ and Cl₁
Answer
Based on the stoichiometric coefficients from the balanced chemical equation associated with the equilibrium, we observe that for every mole of ClF₃ that decreases, there will be a proportional increase in F₂ and Cl₁ based on their respective stoichiometric ratios. Thus, ClF₃'s decrease by 0.010 mol leads to F₂ decreasing by 0.015 mol and Cl₁ decreasing by 0.0050 mol.
Step 3