A asked in Science & MathematicsChemistry · 5 months ago

Given that ΔG°f for NH3 = -16.67 kJ/mol, calculate the equilibrium constant for the following reaction at 298 K.?

Full question: Given that ΔG°f for NH3 = -16.67 kJ/mol, calculate the equilibrium constant for the following reaction at 298 K: N2(g) + 3 H2(g) <-> 2 NH3(g)

Please describe your answers clearly and include steps. 

Update:

Once you find K, what do you do? I need the equilibrium constant for the reaction. 

1 Answer

Relevance
  • 5 months ago

    ΔG° = - RT ln K

    -1.667X10^4 J/mol = - 8.314 J/mol K (298 K) ln K

    K = 836

Still have questions? Get answers by asking now.