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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: Timeless Thinker on May 01, 2020, 09:58:41 PM

Title: Solving for delta G using Gibbs free energy
Post by: Timeless Thinker on May 01, 2020, 09:58:41 PM

Ammonia is synthesized from nitrogen and hydrogen via the reaction:

N₂(g) + 3 H₂(g) → 2 NH₃(g)

ΔG° at 298 K for this reaction is −33.3 kJ/mol. What is the value of ΔG at 298 K for a reaction mixture that consists of 1.9 atm N2, 1.6 atm H2, and 0.65 atm NH3 in kJ/mol?

I used the formula DeltaG = ΔG° -RTln(K

K=(.65)2/(1.9x1.63) = .0543

-((8.314)(298)(ln.0543))/1000 = 7.218 kJ

Delta G = -33.3kJ -7.218kJ

Delta G = -40.518

Is this Correct?