Explain the equilibrium constant for the reaction

Reference no: EM13327739

The standard free energy change for N2O4(g) ? 2 NO2(g) is 5.4 kJ at 25oC. a) What is the equilibrium constant for this reaction? b) What is ?G if we set up the flask to start with 0.450 atm N2O4 and 0.120 atm NO2? c) Hmm? I definitely didn't start with standard condition pressures in b). The free energy value changed. Can you explain why it changed the way it did (more + or more -) compared to the free energy at standard conditions and standard pressures? (Hint: This is really just a Le Chatelier argument type question.)

Reference no: EM13327739

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