15. At a certain temperature K. = 314 for the reaction 2 SO2(g) + 102(g) 2 2 SO3(g). If [O2] = 0.200 and [SO2] = 0.0528 when the system is at equilibrium, what is [SO3]? A. [SO3] = 3.32 В. [SO3] %3D 1.45 C. [SO3] = 0.418 D. [SO3] = 0.747
15. At a certain temperature K. = 314 for the reaction 2 SO2(g) + 102(g) 2 2 SO3(g). If [O2] = 0.200 and [SO2] = 0.0528 when the system is at equilibrium, what is [SO3]? A. [SO3] = 3.32 В. [SO3] %3D 1.45 C. [SO3] = 0.418 D. [SO3] = 0.747
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter8: Thermochemistry
Section: Chapter Questions
Problem 12QAP: The heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q,...
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![Questions 15-21 concern the reaction 2 SO2(8) + 102(g) 2 2 SO3(g), the crucial step in the
production of sulfuric acid. For this reaction AH° = -198 kJ/mol and AS° = -0.187 kJ/mol·K. SO2
(perhaps from the production of copper metal) is mixed with air and heated, resulting in the formation
of SO3. (All concentrations are in Kolks units.)
%3D
15. At a certain temperature Kc = 314 for the reaction 2 SO2(g) + 102(g)22 SO3(g). If [O2] =
0.200 and [SO2] = 0.0528 when the system is at equilibrium, what is [SO3]?
A. [SO3] = 3.32
B. [SO3] = 1.45
C. [SO3] = 0.418
D. [SO3] = 0.747
16. A system is set up in which the concentrations of SO2, O2, and SO3 are all 0.123. The system is
heated to a temperature where K. = 14.7. Which of the following equations can be used to calculate the
concentrations of SO2, O2, and SO3 when 2 SO2(g) + 102(8) 2 SO3(g) reaches equilibrium?
(0.123-2х)2
(0.123+ 2x) (0.123+ x)'
(0.123 – 2x)?
(0.123 – 2x) (0.123– x)!
A. 14.7 =
В. 14.7 %3D
(0.123+ 2x)?
(0.123 – 2x)²(0.123-x)'
(2x)?
(2x) (x)'
С. 14.7 %-
D. 14.7 =](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1c9ec205-c724-4ca2-b5f2-e7d121be95e9%2F9e9163f1-4d19-49c3-a61f-c7994cfa70ed%2Fcv0grdk_processed.png&w=3840&q=75)
Transcribed Image Text:Questions 15-21 concern the reaction 2 SO2(8) + 102(g) 2 2 SO3(g), the crucial step in the
production of sulfuric acid. For this reaction AH° = -198 kJ/mol and AS° = -0.187 kJ/mol·K. SO2
(perhaps from the production of copper metal) is mixed with air and heated, resulting in the formation
of SO3. (All concentrations are in Kolks units.)
%3D
15. At a certain temperature Kc = 314 for the reaction 2 SO2(g) + 102(g)22 SO3(g). If [O2] =
0.200 and [SO2] = 0.0528 when the system is at equilibrium, what is [SO3]?
A. [SO3] = 3.32
B. [SO3] = 1.45
C. [SO3] = 0.418
D. [SO3] = 0.747
16. A system is set up in which the concentrations of SO2, O2, and SO3 are all 0.123. The system is
heated to a temperature where K. = 14.7. Which of the following equations can be used to calculate the
concentrations of SO2, O2, and SO3 when 2 SO2(g) + 102(8) 2 SO3(g) reaches equilibrium?
(0.123-2х)2
(0.123+ 2x) (0.123+ x)'
(0.123 – 2x)?
(0.123 – 2x) (0.123– x)!
A. 14.7 =
В. 14.7 %3D
(0.123+ 2x)?
(0.123 – 2x)²(0.123-x)'
(2x)?
(2x) (x)'
С. 14.7 %-
D. 14.7 =
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