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1. For the reaction A + B → C + D, ΔH° = +40 kJ and ΔS° = +50 J/K.  Therefore, the reaction under standard conditions is:   ΔΔG = ΔΔH- TΔΔS Group of answer choices A. spontaneous at temperatures less than 10 K. B. spontaneous at all temperatures. C. spontaneous at temperatures greater than 800 K. D. spontaneous only at temperatures between 10 K and 800 K. E. nonspontaneous at all temperatures.

1. For the reaction A + B → C + D, ΔH° = +40 kJ and ΔS° = +50 J/K.  Therefore, the reaction under standard conditions is:   ΔΔG = ΔΔH- TΔΔS Group of answer choices A. spontaneous at temperatures less than 10 K. B. spontaneous at all temperatures. C. spontaneous at temperatures greater than 800 K. D. spontaneous only at temperatures between 10 K and 800 K. E. nonspontaneous at all temperatures.

Chemistry
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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1.

For the reaction A + B → C + D, ΔH° = +40 kJ and ΔS° = +50 J/K. 

Therefore, the reaction under standard conditions is:

 

ΔΔG = ΔΔH- TΔΔS

Group of answer choices
A. spontaneous at temperatures less than 10 K.
B. spontaneous at all temperatures.
C. spontaneous at temperatures greater than 800 K.
D. spontaneous only at temperatures between 10 K and 800 K.
E. nonspontaneous at all temperatures.
 
2.

Calculate  ΔG° in kJ for the reaction  A2B(g) + ½B2 (g) ↔ A2B2 (g)

given the following data:

A2(g) + B2(g)  ↔↔ A2B2  (g)              K= 2.3 × 106 at 583. K
2A2(g) + B2(g) ↔↔ 2A2B(g)      K= 1.8× 1037 at 583. K

ΔΔG° = ─RTlnK, R = 8.314 J/K

Group of answer choices
A. 137
B. 1350
C. 1323
D. 13
E. 2724
 
3.
For a solution equimolar in HCN and NaCN, which statement is false?
Group of answer choices
A. The [H+] is larger than it would be if only the HCN was in solution.
B. Addition of more NaCN will shift the acid dissociation equilibrium of HCN to the left.
C. The [H+] is equal to the Ka.
D. This is an example of the common ion effect.
E. Addition of NaOH will increase [CN–] and decrease [HCN].
 
 
 
 
 
 
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