Demonstrate that the change in a state function for a process is independent of the path by calculating the change in Gibbs free energy for two processes that change the state of 1 mol of a monoatomic ideal gas from (298 K, 1 atm) to (600 K, 1000 atm):

Process A: heat the gas at 1 atm from 298 K to 600 K, then compress it at 600 K from 1 atm to 1000 atm to arrive at the final state (600 K, 1000 atm)

Process B: compress the gas from 1 atm to 1000 atm at 298 K, then heat the gas at 1000 atm from 298 K to 600 K to arrive at the final state (600 K, 1000 atm)

Show that the same result is obtained by applying the definitional relation: deltaG=deltaH - delta (T*S). Note that delta(T*S) does not equal T*deltaS.

Answer rating: 100% (QA)

Solution ProCess A P I atm P2 latm 3 looo dm 24 3K Gook T3 600 K M2 H m cp r 1 41 cu R ... View the full answer