Question 31Consider the following reaction at equilibrium. Which manipulation would shift the equilibrium point towards reactands4 NO₂(g) + O₂(g) = 2 N₂O₂(g)O decrease of the volume of reaction vessel and remove NO₂O decrease of the volume of reaction vessel and add N₂OsO increase of the volume of reaction vessel and remove NO₂O increase of the volume of reaction vessel and add O₂Question 32 Question 30Which of the following equilibrium constants is most consistent with a reaction that has mostly products and very little reactantequilibrium point?OK-7.5 x 10-19OK-6.3 x 10-1OK 1.3 x 10-5OK 2.3 x 10 1K = 9.8 x 10.⁹Question 31

This can be explained on the basis of Le-chateliers Principle which states that any type of stress…

Question 31 Consider the following reaction at equilibrium. Which manipulation would shift the equilibrium point towards mactanta 4 NO₂(g) + O₂(g) 2 N₂O₂(g) decrease of the volume of reaction vessel and remove NO₂ decrease of the volume of reaction vessel and add N₂O₁ O increase of the volume of reaction vessel and remove NO₂ increase of the volume of reaction vessel and add O₂ estion 32

Question 31 Consider the following reaction at equilibrium. Which manipulation would shift the equilibrium point towards mactanta 4 NO₂(g) + O₂(g) 2 N₂O₂(g) decrease of the volume of reaction vessel and remove NO₂ decrease of the volume of reaction vessel and add N₂O₁ O increase of the volume of reaction vessel and remove NO₂ increase of the volume of reaction vessel and add O₂ estion 32

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 20Q

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1’he reaction in Exercise 12.33 was repeated. This time, the reaction began when only NO was injected into the reaction container. 110.200 mol L_l NO was injected, what were the equilibrium concentrations of all species? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) ^2 NO K = 4.1 X 10~4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L"' ofO2, what were the equilibrium concentrations of all species?
Nitrogen dioxide can decompose to nitrogen oxide and oxygen. 2NO2(g)2NO(g)+O2(g) K is 0.87 at a certain temperature. A 5.0-L flask at equilibrium is determined to have a total pressure of 1.25 atm and oxygen to have a partial pressure of 0.515 atm. Calculate PNO and PNO2 at equilibrium.
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