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

what's the

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.