The following equilibrium was established in a container - HSC - SSCE Chemistry - Question 7 - 2024 - Paper 1
Question 7
The following equilibrium was established in a container.
$$2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$$
$\Delta H = -198 \text{ kJ mol}^{-1}$
Which of the fol... show full transcript
Worked Solution & Example Answer:The following equilibrium was established in a container - HSC - SSCE Chemistry - Question 7 - 2024 - Paper 1
Step 1
A. Increasing the volume.
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Answer
Increasing the volume shifts the equilibrium to the side with more gas molecules according to Le Chatelier's principle. Since the equilibrium has 3 moles of gas on the left (2 from SO2 and 1 from O2) and only 2 moles on the right, this would decrease the yield of SO3.
Step 2
B. Increasing the temperature.
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Answer
Since the reaction is exothermic (with a negative enthalpy change), increasing the temperature would shift the equilibrium to the left, favoring the formation of reactants and hence decreasing the yield of SO3.
Step 3
C. Removing the product as it is formed.
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By continuously removing SO3 as it is produced, the equilibrium would shift to the right to counteract this change, thereby increasing the yield of SO3.
Step 4
D. Keeping temperature and volume constant.
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Answer
Maintaining conditions constant means that no shift in equilibrium occurs, so the yield of SO3 would remain unchanged.
