Question

In: Chemistry

At 400 K, the reaction N2 (g) + 3 H2 (g) → 2 NH3 (g) reaches...

At 400 K, the reaction

N2 (g) + 3 H2 (g) → 2 NH3 (g)

reaches equilibrium when the partial pressures of nitrogen, hydrogen, and ammonia gases are 4.00 atm, 1.00 atm, and 1.05 x 10^−2 atm, respectively.

(a) Compute the value of the equilibrium constant, KP at 400K.
(b) Compute the standard Gibbs free energy of this reaction at 400K. Express the result in kJ/mol.

(c) Would the system be at equilibrium at 400 K if the partial pressures of nitrogen, hydrogen, and ammonia gases were 2.00 atm, 1.00 atm, and 5.00 x 10^−3 atm, respectively? If not, would the reaction proceed toward the product or toward the reactants to reach equilibrium at 400K?

(d) Compute the value of the Gibbs free energy of the reaction at 400 K with the values of the partial pressures given above (question (c)). Express the result in kJ/mol.

(d) Given that the standard enthalpy of the reaction at 400K is H = -94 kJ/mol, estimate the value of the equilibrium constant KP at 450 K assuming that the standard enthalpy of reaction does not vary significantly with temperature in this temperature range.

Expert Solution

queen_honey_blossom answered 2 years ago

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