Enter your answer in the provided box. In the Mond process for the purification of nickel, carbon monoxide is reacted with heated nickel to produce Ni (CO) 4, which is a gas and can therefore be separated from solid impurities: Ni (s) + 4CO (g) ⇌ Ni (CO) 4 (g) Given that the standard free energies of formation of CO (g) and Ni (CO) 4 (g) are - 137.3 and - 587.4 kJ/mol, respectively, calculate the equilibrium constant of the reaction at 70.0°C. Assume that ΔG o f is temperature-independent.

The equilibrium constant is 6.6 * 10^5

Explanation:

Step 1: Data given

The standard free energies of formation of CO (g) = - 137.3 kJ/mol

The standard free energies of formation of Ni (CO) 4 (g) = - 587.4 kJ/mol,

Temperature = 70.0 °C

Step 2: The balanced equation

Ni (s) + 4CO (g) ⇌ Ni (CO) 4 (g)

For 1 mol Ni we need 4 moles CO to produce 1 mol Ni (CO) 4

Step 3: Calculate Gibbs free energy

Gibbs free energy = standard free energy of formation of products - standard free energy of formation of reactants

Gibbs free energy = standard free energy of formation (Ni (CO) 4) - standard free energy of formation (Ni (s)) + 4Gf (CO))

Gibbs free energy = - 587.4 - (4*-137.3)

Gibbs free energy = - 587. 4 + 549.2

Gibbs free energy = - 38.2 kJ/mol

Step 4: Calculate the equilibrium cosntant K

Δ G ∘ = - RT ln K

-38.2 kJ/mol = - 8.314 * 343 * ln K

ln K = 13.4

K = e^13.4

K = 6.6 * 10^5

The equilibrium constant is 6.6 * 10^5

656055.062

Explanation:

dа ta:

- gas constant, R = 8.3144 J / (mol*K)

- temperature, T = 70 °C or 70+273 = 343 K

The standard free energy of reaction is:

ΔG = G of formation of Ni (CO) 4 (g) - 4 * G of formation of CO (g) - G of formation of Ni (s)

ΔG = - 587.4 - 4 * (-137.3) - 0 = - 38.2 kJ/mol or - 38200 J/mol

The relationship between the standard free energy of reaction (ΔG) and the the equilibrium constant (Kp) is:

ΔG = - R*T*ln (Kp)

-38200 / (-8.3144*343) = ln (Kp)

e^13.394 = Kp

656055.062 = Kp