Question 5 5 points consider the following chemical

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Unformatted text preview: state that a process is not spontaneous under conditions of constant volume and constant temperature? a) ΔA ≤ 0 b) ΔA < 0 c) ΔA > 0 d) Δ A ≥ 0 e) ΔG ≤ 0 f) ΔG < 0 g) ΔG > 0 h) ΔG ≥ 0 Explain your reasoning. Question 4: (5 points) For an ideal gas, the expression dA – dG can be written as: a) – nRdT b) + Vdp c) + TdS d) + SdT e) + nR dT f) – pdV g) + pdV h) – Vdp i) – TdS j) – SdT Show how you arrive at the chosen result. Question 5: (5 points) Consider the following chemical reaction at 298.15K and 18.2 bars: l2 (s) + H2 (g) à༎ 2HI (g) Using the data in the data section, you calculate the reaction Gibbs free energy change for three moles of iodine and three moles of hydrogen at 298.15K and 18.2 bars to be: a) - 12.0 kJ b) - 7.6 kJ c) - 7.4 kJ d) - 5.8 kJ e) 19.4 kJ f) 20.4 kJ g) 27.8 kJ h) 31.2 kJ Show your calculations! Question 6: (5 points) Consider the following chemical reaction at 1 bar: l2 (s) + H2 (g) à༎ 2HI (g) Using the data in the data section and assuming that the reaction enthalpy change and the reation used to calculate the change in chemical potential!...
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This note was uploaded on 01/26/2014 for the course CHEM 3615 taught by Professor Aresker during the Spring '07 term at Virginia Tech.

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