Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
Section: Chapter Questions
Problem 58PS: Use standard enthalpies of formation in Appendix L to calculate enthalpy changes for the following:...
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Question 4!
![3.
Use Hess'S law to Calculate 2AGʻrxn USIIig the TUIlUWIng iniormation.
NO(g) + O(g) → NO2(g)
2 03(g) → 3 O2(g)
O2(g) → 2 0(g)
NO(g) + O3(g) → NO2(g) + O2(g)
AG°rxn
AG°rxn = +489.6 kJ
AG°rxn = +463.4 kJ
AG°rxn = -199.5 kJ
a. +753.5 kJ
b. +277.0 kJ
c. -676.0 kJ
d. -1152.5 kJ
e. -225.7 kJ
4. Calculate AGrxn at 298 K under the conditions shown below for the following reaction.
3 Oz(g) → 2 03(g)
P(O2) = 0.41 atm, P(O3) = 5.2 atm
AGO = +326 kJ
%3D
a. +341 kJ
b. +17.8 kJ
c. +332 kJ
d. -47.4 kJ
e. -109 kJ
5. Which of the following is NOT true for AGrxn?
a. If AG°rxn > 0, the reaction is spontaneous in the forward direction.
b. If Q = 1, then DGrxn = AG°rxn.
c. If AG°rxn < 0, the reaction is spontaneous in the forward direction.
d. If AG°rxn > 0, the reaction is spontaneous in the reverse direction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff0e66cf8-8203-445a-adec-0881fdf188fe%2Fa53ae66d-708e-4c98-bc4f-3bfaf0d1b5f9%2Fwfnl26o_processed.jpeg&w=3840&q=75)
Transcribed Image Text:3.
Use Hess'S law to Calculate 2AGʻrxn USIIig the TUIlUWIng iniormation.
NO(g) + O(g) → NO2(g)
2 03(g) → 3 O2(g)
O2(g) → 2 0(g)
NO(g) + O3(g) → NO2(g) + O2(g)
AG°rxn
AG°rxn = +489.6 kJ
AG°rxn = +463.4 kJ
AG°rxn = -199.5 kJ
a. +753.5 kJ
b. +277.0 kJ
c. -676.0 kJ
d. -1152.5 kJ
e. -225.7 kJ
4. Calculate AGrxn at 298 K under the conditions shown below for the following reaction.
3 Oz(g) → 2 03(g)
P(O2) = 0.41 atm, P(O3) = 5.2 atm
AGO = +326 kJ
%3D
a. +341 kJ
b. +17.8 kJ
c. +332 kJ
d. -47.4 kJ
e. -109 kJ
5. Which of the following is NOT true for AGrxn?
a. If AG°rxn > 0, the reaction is spontaneous in the forward direction.
b. If Q = 1, then DGrxn = AG°rxn.
c. If AG°rxn < 0, the reaction is spontaneous in the forward direction.
d. If AG°rxn > 0, the reaction is spontaneous in the reverse direction.
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