17.) Calculate the change in the Gibbs energy if one mole of a perfect gas is allowed to expandisothermally and reversibly at 60°C from a volume of 3.5 L to 8.0 L.A. -2.29 kJB. +2.29 kJC. +9.32 kJD. -9.32 kJ18.) Determine the change in the Gibbs energy for the reaction at 298 K. The Enthalpy of formationfor CO2 (g) was -393.51 kJ/mol. The entropies for C (s), 02 (g) and CO2 (g) are 5.740, 205.138,213.74 J/K molC (s) + 02 (g) → CO2A. -1246 kJ/molB. +1245 kJ/molC. -459.36 kJ/molD. -394.4 kJ/mol

Since you have asked multiple question, we will solve the first question for you. If you want any…

17.) Calculate the change in the Gibbs energy if one mole of a perfect gas is allowed to expand isothermally and reversibly at 60°C from a volume of 3.5 L to 8.0 L. A. -2.29 kJ B. +2.29 kJ C. +9.32 kJ D. -9.32 kJ

17.) Calculate the change in the Gibbs energy if one mole of a perfect gas is allowed to expand isothermally and reversibly at 60°C from a volume of 3.5 L to 8.0 L. A. -2.29 kJ B. +2.29 kJ C. +9.32 kJ D. -9.32 kJ

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 89QRT: Determine the standard Gibbs free energy change, rG, for the reactions of liquid methanol, of CO(g),...

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Question

17.) Calculate the change in the Gibbs energy if one mole of a perfect gas is allowed to expand
isothermally and reversibly at 60°C from a volume of 3.5 L to 8.0 L.
A. -2.29 kJ
B. +2.29 kJ
C. +9.32 kJ
D. -9.32 kJ
18.) Determine the change in the Gibbs energy for the reaction at 298 K. The Enthalpy of formation
for CO2 (g) was -393.51 kJ/mol. The entropies for C (s), 02 (g) and CO2 (g) are 5.740, 205.138,
213.74 J/K mol
C (s) + 02 (g) → CO2
A. -1246 kJ/mol
B. +1245 kJ/mol
C. -459.36 kJ/mol
D. -394.4 kJ/mol

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