Which of the following changes will always shift this equilibrium reaction to the right?
2H₂(g) ⇌ H₂(g) + I₂(g)
ΔH = -52 kJ
(A) Adding a catalyst
(B) Increasing the pressure
(C) Increasing the temperature
(D) Adding more of the reactant - HSC - SSCE Chemistry - Question 7 - 2008 - Paper 1
Question 7
Which of the following changes will always shift this equilibrium reaction to the right?
2H₂(g) ⇌ H₂(g) + I₂(g)
ΔH = -52 kJ
(A) Adding a catalyst
(B) Increasing t... show full transcript
Worked Solution & Example Answer:Which of the following changes will always shift this equilibrium reaction to the right?
2H₂(g) ⇌ H₂(g) + I₂(g)
ΔH = -52 kJ
(A) Adding a catalyst
(B) Increasing the pressure
(C) Increasing the temperature
(D) Adding more of the reactant - HSC - SSCE Chemistry - Question 7 - 2008 - Paper 1
Step 1
Adding a catalyst
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Answer
Adding a catalyst does not affect the position of the equilibrium; it only speeds up the rate at which equilibrium is reached.
Step 2
Increasing the pressure
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Answer
Increasing the pressure affects reactions with gaseous substances. However, since the number of moles of gaseous reactants (2) is the same as the number of moles of gaseous products (2), this change does not shift the equilibrium.
Step 3
Increasing the temperature
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Answer
For exothermic reactions (which this is, as indicated by ΔH being negative), increasing the temperature will shift the equilibrium to the left, not to the right.
Step 4
Adding more of the reactant
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Answer
According to Le Chatelier's principle, adding more of a reactant will shift the equilibrium to the right, producing more products in response to the increased concentration of the reactant.
