Chemical Principles: The Quest for Insight
7th Edition
ISBN: 9781464183959
Author: Peter Atkins, Loretta Jones, Leroy Laverman
Publisher: W. H. Freeman
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Chapter 5, Problem 5J.10E
(a)
Interpretation Introduction
Interpretation:
The change in partial pressure of
Concept Introduction:
Le-Chatlier’s principle:
If a chemical system at equilibrium experiences a change in concentration, temperature, volume, or partial pressure, then the equilibrium shifts to neutralize the imposed change and a new equilibrium is established.
Example:
Increasing the concentration of reactants shifts the equilibrium to the right side and thus concentration of the water also increases.
(b)
Interpretation Introduction
Interpretation:
The change in partial pressure of
Concept Introduction:
Refer to part (a).
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The reaction
N2O4(g) = 2NO2(3)
has a K, = 0.140 at 25 °C. In a reaction vessel containing the gases in equilibrium at that temperature, the partial pressure of N204
was 0.235 atm.
(a) What was the partial pressure of NO2 in the reaction mixture?
pressure of NO2 = i
atm
(b) What was the total pressure of the mixture of gases?
total pressure = i
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Be sure to answer all parts. Enter your answers in scientific notation.
At a particular temperature, K = 6.9 × 10² for
2NO(g) + 2H₂(g) = N₂(g) + 2H₂O(g)
Calculate Ke for each of the following reactions:
(a) NO(g) + H₂(g) = = N₂(g) + H₂O(g)
2
(b) 2N₂(g) + 4H₂O(g) = 4NO(g) + 4H₂(g)
Kc =
Kc=
× 10
X
x 10
Carbon monoxide and water vapor, each at 200. Torr, were introduced into a container of volume 0.250 L. When the mixture reached equilibrium at 700 degrees Celsius, the partial pressure of CO2(g) was 88 Torr. Calculate the value of K for the equilibrium CO (g) + H2O (g)⇋ CO2(g)+H2(g).
Chapter 5 Solutions
Chemical Principles: The Quest for Insight
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Solutions: Crash Course Chemistry #27; Author: Crash Course;https://www.youtube.com/watch?v=9h2f1Bjr0p4;License: Standard YouTube License, CC-BY