The free energy of formation of nitric oxide, no, at 1000 k (roughly the temperature in an automobile engine during ignition) is about 78 kj/mol. calculate the equilibrium constant kp for the reaction n2(g) + o2(g) 2no(g) at this temperature.

The value of for the chemical equation is

Explanation:

For the given chemical equation:

To calculate the for given value of Gibbs free energy, we use the relation:

where,

= Gibbs free energy = 78 kJ/mol = 78000 J/mol  (Conversion factor: 1kJ = 1000J)

R = Gas constant =

T = temperature = 1000 K

= equilibrium constant in terms of partial pressure = ?

Putting values in above equation, we get:

Hence, the value of for the chemical equation is

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