If the ΔH°rx and ΔS°rx for a gas phase
chemical reaction are 419.53 kJ and -178.85 J/K respectively,
determine ΔG°rx (in kJ) at 103.11 °C. Report your answer
to two decimal places (i.e. 123.45 kJ). Assume that
ΔH°rx and ΔS°rx do not vary with
temperature.
Apply:
G = H - TS
G = (419.53*1000) - (103.11+273)*(-178.85) = 486797.2735 J/mol
G = 48.68 kJ/mol
If the ΔH°rx and ΔS°rx for a gas phase chemical reaction are 419.53 kJ and -178.85...
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