Calculate the free-energy change of the following reaction at 502°C and standard pressure. Values in the table are at standard pressure and25°C.1st attemptSee Periodic TableSee HintCH,(g) +30,(g) –→ 200,(g) + 2H,0(g)AH6,(kJ/mol)S J/mol KAGf, kJ/molC2H4(g)52.3219.568.1O2ls)205.00.CO2(g)-393.5213.6-394.4H20(g)-241.8188.7-228.6kUmol eduPart 2Calculate AG°rxn:AG° rxn=kJPart 3Which phrase best describes this reaction under standard conditions?Choose one:Exothermic and spontaneousEndothermic and spontaneousExothermic and nonspontaneousEndothermic and nonspontaneous

The standard enthalpy change and the entropy change of the reaction are given by: ∆H° = ∑∆H°f…

Calculate AG°nxn: AG°rxn= kJ Part 3 Which phrase best describes this reaction under standard conditions? Choose one: Exothermic and spontaneous Endothermic and spontaneous Exothermic and nonspontaneous Endothermic and nonspontaneous

Calculate AG°nxn: AG°rxn= kJ Part 3 Which phrase best describes this reaction under standard conditions? Choose one: Exothermic and spontaneous Endothermic and spontaneous Exothermic and nonspontaneous Endothermic and nonspontaneous

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

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Calculate the free-energy change of the following reaction at 502°C and standard pressure. Values in the table are at standard pressure and
25°C.
1st attempt
See Periodic Table
See Hint
CH,(g) +30,(g) –→ 200,(g) + 2H,0(g)
AH6,(kJ/mol)
S J/mol K
AGf, kJ/mol
C2H4(g)
52.3
219.5
68.1
O2ls)
205.0
0.
CO2(g)
-393.5
213.6
-394.4
H20(g)
-241.8
188.7
-228.6
kUmol

edu
Part 2
Calculate AG°rxn:
AG° rxn=
kJ
Part 3
Which phrase best describes this reaction under standard conditions?
Choose one:
Exothermic and spontaneous
Endothermic and spontaneous
Exothermic and nonspontaneous
Endothermic and nonspontaneous

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