PROBLEM: Choose the member with the higher entropy in each of the following pairs, and justify your choice [assume constant temperature, except in part (e)]: (a) 1 mol of SO₂(g) or 1 mol of SO3(g) (b) 1 mol of CO₂(s) or 1 mol of CO₂(g) (c) 3 mol of O₂(g) or 2 mol of O3(g) (d) 1 mol of KBr(s) or 1 mol of KBr(aq) seawater at 2°C or at 23°C (e) (f) 1 mol of CF4(g) or 1 mol of CCl4(9)
PROBLEM: Choose the member with the higher entropy in each of the following pairs, and justify your choice [assume constant temperature, except in part (e)]: (a) 1 mol of SO₂(g) or 1 mol of SO3(g) (b) 1 mol of CO₂(s) or 1 mol of CO₂(g) (c) 3 mol of O₂(g) or 2 mol of O3(g) (d) 1 mol of KBr(s) or 1 mol of KBr(aq) seawater at 2°C or at 23°C (e) (f) 1 mol of CF4(g) or 1 mol of CCl4(9)
Chemistry
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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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![PROBLEM: Choose the member with the higher entropy in each of the
following pairs, and justify your choice [assume constant
temperature, except in part (e)]:
(a) 1 mol of SO₂(g) or 1 mol of SO3(g)
(b)
1 mol of CO₂ (s) or 1 mol of CO₂(g)
3 mol of O₂(g) or 2 mol of O3(g)
(c)
(d)
1 mol of KBr(s) or 1 mol of KBr(aq)
seawater at 2°C or at 23°C
(e)
(f) 1 mol of CF₂(g) or 1 mol of CCl4 (9)
PROBLEM: A key step in the production of sulfuric acid is the oxidation
of SO₂(g) to SO3(g):
2SO₂(g) + O₂(g) → 2SO3(g)
At 298 K, AG = -141.6 kJ; AH = -198.4 kJ; and AS = -187.9 J/K
(a) Use the data to decide if this reaction is spontaneous at 25°C, and
predict how AG will change with increasing T.
(b) Assuming AH and AS are constant with increasing T, is the
reaction spontaneous at 900.° C?
PROBLEM:
ΔΗ = 58.1 kJ
At 25°C (298 K), the reduction of copper(1) oxide is
nonspontaneous AG = 8.9 kJ). Calculate the temperature
at which the reaction becomes spontaneous.
AS = 0.165 kJ/K](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdb82b1bf-9ecb-4650-bc73-bb0c93237287%2Fb9ae4d8d-6e7c-43ac-a289-b52c16be0ccf%2Fumr9rsd_processed.png&w=3840&q=75)
Transcribed Image Text:PROBLEM: Choose the member with the higher entropy in each of the
following pairs, and justify your choice [assume constant
temperature, except in part (e)]:
(a) 1 mol of SO₂(g) or 1 mol of SO3(g)
(b)
1 mol of CO₂ (s) or 1 mol of CO₂(g)
3 mol of O₂(g) or 2 mol of O3(g)
(c)
(d)
1 mol of KBr(s) or 1 mol of KBr(aq)
seawater at 2°C or at 23°C
(e)
(f) 1 mol of CF₂(g) or 1 mol of CCl4 (9)
PROBLEM: A key step in the production of sulfuric acid is the oxidation
of SO₂(g) to SO3(g):
2SO₂(g) + O₂(g) → 2SO3(g)
At 298 K, AG = -141.6 kJ; AH = -198.4 kJ; and AS = -187.9 J/K
(a) Use the data to decide if this reaction is spontaneous at 25°C, and
predict how AG will change with increasing T.
(b) Assuming AH and AS are constant with increasing T, is the
reaction spontaneous at 900.° C?
PROBLEM:
ΔΗ = 58.1 kJ
At 25°C (298 K), the reduction of copper(1) oxide is
nonspontaneous AG = 8.9 kJ). Calculate the temperature
at which the reaction becomes spontaneous.
AS = 0.165 kJ/K
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