Nitrogen tetroxide breaks down according to the equation: N2O4 (g) →2NO2 (g) AH = 54KJ / mol Pure N2O4 (g) was added to a 3.00 L container at 127 ° C under a pressure of 5.00 kPa. After the system reached its equilibrium state, the

Chemistry: Principles and Reactions
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Author:William L. Masterton, Cecile N. Hurley
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Chapter8: Thermochemistry
Section: Chapter Questions
Problem 90QAP: Consider a metal ion A2+ and its nitrate salt, In an experiment, 35.00 mL of a 0.217 M solution of...
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Nitrogen tetroxide breaks down according to
the equation:
N204 (g) +2NO2 (g) AH = 54KJ / mol
%3D
Pure N204 (g) was added to a 3.00 L container
at 127 ° C under a pressure of 5.00 kPa. After
the system reached its equilibrium state, the
total pressure in the container was found to
have risen to 8.43 kPa.
Question 1: Calculate the value of KP at 127 oC
for this reaction
Question 2: The volume of the container is
suddenly compressed to 1.00 L at 127 ° OC,
tripling the pressure of all components in the
container from equilibrium in (a). In what
direction would the equilibrium of the reaction
shift? Calculate the new partial pressures of
N204 and NO2, as well as the total pressure in
the container, once equilibrium is re-
established
Transcribed Image Text:Nitrogen tetroxide breaks down according to the equation: N204 (g) +2NO2 (g) AH = 54KJ / mol %3D Pure N204 (g) was added to a 3.00 L container at 127 ° C under a pressure of 5.00 kPa. After the system reached its equilibrium state, the total pressure in the container was found to have risen to 8.43 kPa. Question 1: Calculate the value of KP at 127 oC for this reaction Question 2: The volume of the container is suddenly compressed to 1.00 L at 127 ° OC, tripling the pressure of all components in the container from equilibrium in (a). In what direction would the equilibrium of the reaction shift? Calculate the new partial pressures of N204 and NO2, as well as the total pressure in the container, once equilibrium is re- established
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