The equation represents an equilibrium. 4NH₃(g) + 5O₂(g) ⇌ 4NO(g) + 6H₂O(g) ΔH = -900 kJ mol⁻¹ What would increase the concentration of NO at equilibrium? 1 a reduction in the reaction temperature 2 the use of a suitable catalyst 3 an increase in the total pressure

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The equation represents an equilibrium - CIE - A-Level Chemistry - Question 34 - 2018 - Paper 1

Question 34

The equation represents an equilibrium. 4NH₃(g) + 5O₂(g) ⇌ 4NO(g) + 6H₂O(g) ΔH = -900 kJ mol⁻¹ What would increase the concentration of NO at equilibrium? 1 a redu... show full transcript

Worked Solution & Example Answer:The equation represents an equilibrium - CIE - A-Level Chemistry - Question 34 - 2018 - Paper 1

Step 1

1 a reduction in the reaction temperature

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A reduction in temperature would shift the equilibrium to the right (toward the products) since the reaction is exothermic (as indicated by ΔH = -900 kJ mol⁻¹). This shift increases the concentration of NO.

Step 2

2 the use of a suitable catalyst

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Answer

The use of a suitable catalyst does not affect the position of equilibrium. It only speeds up the rate at which equilibrium is reached without changing the concentrations of reactants or products.

Step 3

3 an increase in the total pressure

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An increase in total pressure would favor the side of the equilibrium with fewer moles of gas. In this case, the reaction has 9 moles on the reactants side (4NH₃ + 5O₂) and 10 moles on the products side (4NO + 6H₂O). Thus, increasing pressure will shift the equilibrium to the left, decreasing the concentration of NO.

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The equation represents an equilibrium - CIE - A-Level Chemistry - Question 34 - 2018 - Paper 1

Worked Solution & Example Answer:The equation represents an equilibrium - CIE - A-Level Chemistry - Question 34 - 2018 - Paper 1

1 a reduction in the reaction temperature

2 the use of a suitable catalyst

3 an increase in the total pressure

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