The table shows the partial pressures in an equilibrium mixture formed by the Haber process.3H2(g) + N2(g) ⇌ 2NH3(g)4partial pressure / kPasubstance7000nitrogen8000hydrogen4000ammoniaWhat is the numerical value of the equilibrium constant, Kp, for this reaction?2.24 × 108D7.14 × 10–5C4.76 × 10–5B4.46 × 10–9A3© UCLES 2023 03_9701_12_1.18 [Turn over
Question
The table shows the partial pressures in an equilibrium mixture formed by the Haber process.3H2(g) + N2(g) ⇌ 2NH3(g)4partial pressure / kPasubstance7000nitrogen8000hydrogen4000ammoniaWhat is the numerical value of the equilibrium constant, Kp, for this reaction?2.24 × 108D7.14 × 10–5C4.76 × 10–5B4.46 × 10–9A3© UCLES 2023 03_9701_12_1.18 [Turn over
Solution
The equilibrium constant, Kp, for a reaction is given by the ratio of the product of the partial pressures of the products to the product of the partial pressures of the reactants, each raised to the power of their stoichiometric coefficients in the balanced chemical equation.
For the Haber process, the balanced chemical equation is:
3H2(g) + N2(g) ⇌ 2NH3(g)
The partial pressures are given as:
P(N2) = 7000 kPa P(H2) = 8000 kPa P(NH3) = 4000 kPa
The equilibrium constant, Kp, is given by:
Kp = [P(NH3)^2] / [P(N2) * (P(H2)^3)]
Substituting the given values:
Kp = [4000^2] / [7000 * (8000^3)]
Kp = 16 x 10^6 / 4.48 x 10^12
Kp = 3.57 x 10^-6
So, the closest answer to this value is 4.76 x 10^-5 (Option C).
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