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...
For the following reaction: CS2(g) + 3O2(g) → CO2(g) + 2SO2(g) Compound ΔH°f (kJ mol-1) S° (J mol-1 K-1) CS2 (g) 116.70 237.80 O2 (g) 0.00 205.70 CO2 (g) -393.51 213.74 SO2 (g) -296.84 248.20 Calculate ΔG°rx (in kJ) at 794.8 K for this reaction. Report your answer to two decimal places in standard notation (i.e. 123.45 kJ). Assume ΔH°f and S° do not vary as a function of temperature.
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Calculate ΔG° at 298.0 K for this reaction given that ΔH°rxn = –12.0 kJ and ΔS°rxn = –147 J/K
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