college chemistry

calculate the equilibrium constant for the following reaction at 298k given that DeltaGrxn=2.8kj/mol N2O4-2NO2

I thought to get K you use the expression K=e^(-deltaG/(RT)) but I cant get the same answer my professor put down which is 3.1

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asked by Jeremy
  1. I get his answer. Did you use J, or kJ in the exponent? kJ is not a standard unit, try 2800J/mol

  2. PCl5(g) eqarrow PCl3(g) + Cl2(g)
    The reaction above has an equilibrium constant of 0.800 at 340°C, and deltaH°rxn = 87.9 kJ/mol under standard conditions. Under which conditions will this reaction produce the most PCl3(g)?

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