A particular reaction is carried out using equal amounts of CH₄(g) and H₂O(g) - VCE - SSCE Chemistry - Question 1 - 2008 - Paper 1
Question 1
A particular reaction is carried out using equal amounts of CH₄(g) and H₂O(g).
Which one of the following sets of changes in conditions would lead to the greatest i... show full transcript
Worked Solution & Example Answer:A particular reaction is carried out using equal amounts of CH₄(g) and H₂O(g) - VCE - SSCE Chemistry - Question 1 - 2008 - Paper 1
Step 1
Volume of reaction vessel: increased; Temperature: increased
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Answer
Increasing the volume of the reaction vessel decreases the pressure, which favors the side of the reaction with more moles of gas. However, an increase in temperature generally favors endothermic reactions, shifting the equilibrium towards products. This combination would likely lead to an increase in product formation.
Step 2
Volume of reaction vessel: increased; Temperature: decreased
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Answer
Increasing the volume while decreasing the temperature would lower pressure and may shift equilibrium towards reactants, as it favors exothermic shifts. This is not favorable for product formation.
Step 3
Volume of reaction vessel: decreased; Temperature: increased
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Answer
Decreasing the volume increases pressure, which may favor the reaction's side with fewer moles of gas. The higher temperature favors endothermic reactions, potentially increasing product formation, but the pressure effect may counterbalance it.
Step 4
Volume of reaction vessel: decreased; Temperature: decreased
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Answer
Decreasing volume increases pressure, but a lower temperature generally favors exothermic reactions. This change would not significantly favor product formation.
