Problem: Consider the reaction that occurs during the Haber process: N2(g) + 3 H2(g) → 2 NH3(g)The equilibrium constant is 3.9 x 105 at 300 K and 1.2 x 10–1 at 500 K. Calculate ΔH˚rxn and ΔS˚rxn Delta S_{ m rxn}^circ for this reaction.

FREE Expert Solution

Step 1. Calculate ΔG˚rxn:

G°rxn = -RTlnKG°rxn = -(8.314 Jmol·K)(300 K)[ln(3.9×105)]G°rxn =-32,110.086 Jmol

G°rxn =-32,110.086 Jmol(1 kJ103J)

ΔG˚rxn =  -32.11 kJ/mol


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Problem Details

Consider the reaction that occurs during the Haber process: N2(g) + 3 H2(g) → 2 NH3(g)

The equilibrium constant is 3.9 x 105 at 300 K and 1.2 x 10–1 at 500 K. Calculate ΔH˚rxn and ΔS˚rxn for this reaction.

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