Find the equlilbrium constant at 25 C for the reaction
2NO2(g)---->N2O4(g)
the following data is also at 25 C:
NO2: ^enthalpy of formation: 33.8 kj/mol, ^gibbs free energy of formation: 51.8 kj/mol, entropy of formation is 240.4 J/mol-K
N2O4: ^enthalpy of formation: 9.7 kj/mol, ^gibbs free energy of formation: 98.3 kj/mol, entropy of formation is 304.3 kj/mol
Can I use ^G(standard)=-RTlnK? I'm not sure if K is equliibrium constant or Freedman's constant, and if I use that equation what value do I use for ^G? I know ^G is zero at equlilbrium, but I'm not sure if ^G(standard) is also zero at equlilbrium. Thank you for your help, I really appreciate it.