The four equations below represent different equilibrium systems - VCE - SSCE Chemistry - Question 24 - 2018 - Paper 1
Question 24
The four equations below represent different equilibrium systems.
Equation 1
$2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$
$\Delta H = -180 kJ \, mol^{-1}$
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Worked Solution & Example Answer:The four equations below represent different equilibrium systems - VCE - SSCE Chemistry - Question 24 - 2018 - Paper 1
Step 1
Equation 1
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Answer
In this exothermic reaction, lowering the temperature shifts the equilibrium to the right, increasing SO₃ yield. Increasing pressure also shifts the reaction right due to more moles of products.
Step 2
Equation 2
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Answer
This is an exothermic reaction as well. Lowering the temperature shifts it right, increasing CO₂ and H₂ yield. However, the effect of pressure increase is less clear due to equal number of moles on both sides.
Step 3
Equation 3
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Answer
In this endothermic reaction, lowering temperature shifts the equilibrium to the left, decreasing PCl₃ and Cl₂ yield. An increase in pressure shifts the equilibrium to the side with fewer moles, which does not apply here.
Step 4
Equation 4
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Answer
This endothermic reaction will shift to the left with a temperature decrease, hence decreasing yield of CH₄ and H₂O. Moreover, increasing pressure will favor products, but overall yields would decrease.
