A chemist fills a reaction vessel with 7.92 atm nitrogen (N2) gas, 2.02 atm hydrogen (H2) gas, and 2.11 atm ammonia (NH3) gas at a temperature of 25.0°C

Under these conditions, calculate the reaction free energy ΔG for the following chemical reaction

N2(8) +3H2 2NH3 (g)

Use the thermodynamic information in the ALEKS Data tab. Round your answer to the nearest kilojoule.

The Gibbs free energy of the given reaction is -40 kJ

Explanation:

The given chemical equation follows:

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

We are given:

Putting values in above equation, we get:

The equation used to Gibbs free energy of the reaction follows:

where,

= free energy of the reaction

= standard Gibbs free energy = -32.9 kJ/mol = -32900 J/mol  (Conversion factor: 1 kJ = 1000 J)

R = Gas constant = 8.314J/K mol

T = Temperature =

= Ratio of concentration of products and reactants at any time =

Putting values in above equation, we get:

Hence, the Gibbs free energy of the given reaction is -40 kJ