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 58.0°C. Assume that ΔG o f is temperature-independent.

The equilibrium constant for this reaction is

Explanation:

The equation used to calculate standard Gibbs free change is of a reaction is:

For the given chemical reaction:

The equation for the standard Gibbs free change of the above reaction is:

We are given:

Putting values in above equation, we get:

To calculate the equilibrium constant (at 58°C) for given value of Gibbs free energy, we use the relation:

where,

= Standard Gibbs free energy = -38.2 kJ/mol = -38200 J/mol  (Conversion factor: 1 kJ = 1000 J )

R = Gas constant = 8.314 J/K mol

T = temperature =

= equilibrium constant at 58°C = ?

Putting values in above equation, we get:

Hence, the equilibrium constant for this reaction is

i dont know

explanation:

c. heat could easily travel through the molecules in the air and escape/enter the flask. removing the air slows down the heat transfer.