i hope that you can answer both the questions. thank you so much! Time left 1:08:34Consider the following equilibrium reaction:N204 (g) - 2 NO2 (g)N,O,Concentration(mol /L)NO,TimeAt time t1, heat is applied to the system. Which of the following best describes the equilibrium reaction and the change in Kc?O endothermic and K, increasesO endothermic and Ke decreasesO exothermic and Ke increasesO exothermic and Kç decreasesThe following reactions have equilibrium values all measured at 500 K. Arrange them in order of increasing tendency to proceed to completion (least completion to greatest completion).2 NocI - 2 NO + Cl2Kp = 1.7 x 10-2I.II.N204 - 2 NO2Kp = 1.5 x 103III. 2 S03 - 2 sO2 + 02Kp = 1.3 x 10-5IV.2 NO2 - 2 NO + 02Kp = 5.9 x 10-5O IV < III < |< ||Il

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Answered: At time t1, heat is applied to the…

At time t1, heat is applied to the system. Which of the following best describes the equilibrium reaction and the change in Kc?

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 10RQ: The only stress (change) that also changes the value of K is a change in temperature. For an...

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i hope that you can answer both the questions. thank you so much!

Time left 1:08:34
Consider the following equilibrium reaction:
N204 (g) - 2 NO2 (g)
N,O,
Concentration
(mol /L)
NO,
Time
At time t1, heat is applied to the system. Which of the following best describes the equilibrium reaction and the change in Kc?
O endothermic and K, increases
O endothermic and Ke decreases
O exothermic and Ke increases
O exothermic and Kç decreases
The following reactions have equilibrium values all measured at 500 K. Arrange them in order of increasing tendency to proceed to completion (least completion to greatest completion).
2 NocI - 2 NO + Cl2
Kp = 1.7 x 10-2
I.
II.
N204 - 2 NO2
Kp = 1.5 x 103
III. 2 S03 - 2 sO2 + 02
Kp = 1.3 x 10-5
IV.
2 NO2 - 2 NO + 02
Kp = 5.9 x 10-5
O IV < III < |< ||
Il <l< |II < IV
III < IV < I < ||
O II <l< IV < I|

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