Considering the reaction below at equilibrium, which of the following statements is correct? N2O4 (g) ⇄ 2NO2 (g) Considering the reaction below at equilibrium, which of the following statements is correct? N2O4 (g) ⇄ 2NO2 (g) A. N2O4 can no longer react to form NO2. B. NO2 is being formed more quickly than N2O4. C. The ratio of [NO2]2/[N2O4] is not changing. D. The concentration of N2O4 is equal to the concentration of NO2.

Considering the reaction below at equilibrium, which of the following statements is correct? N2O4 (g) ⇄ 2NO2 (g) Considering the reaction below at equilibrium, which of the following statements is correct? N2O4 (g) ⇄ 2NO2 (g) A. N2O4 can no longer react to form NO2. B. NO2 is being formed more quickly than N2O4. C. The ratio of [NO2]2/[N2O4] is not changing. D. The concentration of N2O4 is equal to the concentration of NO2.

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy

Section18.7: Calculating And Using Standard Free Energies, Δfg˚

Problem 3RC

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The Keq for the equilibrium below is 0.112 at 700.0 °C. SO2 (g) + 1/2 O2 (g) <==> SO3 (g) What is the value of Keq at this temperature for the following reaction? 2SO3 (g) <==> 2SO2 (g) + O2 (g) A) 79.7B) 2.99C) 17.86D) 4.46E) 8.93
The Keq for the equilibrium below is 2.4 × 10-3 at 700 °C.SO2 (g) + ½ O2 (g) ⇌ SO3 (g)What is the value of Keq at this temperature for the following reaction?2 SO3 (g) ⇌ 2 SO2 (g) + O2 (g)
4) For the reaction shown below, at a particular time, the following concentrations are obtained: [N2O4] = 2.00 M, [NO2] = 0.20 M. Is this reaction at equilibrium? If not, which direction will the reaction proceed and what will the concentrations be at equilibrium? N2O4 (g) « 2 NO2 (g)Kc = 0.200
How will adding nitrogen gas affect the following equilibria? N2(g) + 3H2(g) 2NH3(g) ΔH= -92.2 kJ a. Shift Left b. No Change c. Shift Right
The Keq for the equilibrium below is 5.4 × 1013 at 480.0 °C. 2NO (g) + O2 (g) ⇌ 2NO2 (g) What is the value of Keq at this temperature for the following reaction? NO2 (g) ⇌ NO (g) + 1/2O2 (g)
What is the relationship of the equilibrium constants for the following two reactions? (1) 2NO2(g) + N2O4(g); (2) N204(g) + 2NO2(g) A. Keq of reaction (1) is the reciprocal of Key of reaction (2). B. Keq of reaction (2) is the reciprocal of Key of reaction (1) C. Keq of reaction (2) is the reciprocal of Keq of reaction (1) D. Answers A and B are both correct E. There is no relationship between the Keqs of these reactions.
Consider the reaction below, for which K = 4.2 × 10–31 at 27 °C. N2 (g) + O2 (g) ⇌ 2NO (g) What is the value of K for the equilibrium below?4NO (g) ⇌ 2N2 (g) + 2O2 (g) Select one: a. 8.4 × 1031 b. 2.4 × 1030 c. 1.8 × 10–61 d. 8.4 × 10–31 e. 5.7 × 1060
How will a decrease in Pressure affect the following equilibria? N2(g) + 3H2(g) 2NH3(g) ΔH= -92.2 kJ a. Shift Left b. No Change c. Shift Right
For the following reaction, which modification will shift the position of equilibrium to favor more products? 2NO(g) + Cl2(g) ⇌ 2NOCl(g) ∆Hº = –77.1 kJ/mol Group of answer choices 1. increase the pressure at constant temperature 2. add more NOCl at constant temperature 3. increase the temperature at constant pressure 4. remove some NO at constant temperature 5. increase the volume at constant temp
At a given temperature, the equilibrium constant Kc for the reaction below is 3.30×10-3. 2SO2(g)+O2(g)2SO3(g)What is the value of the equilibrium constant for each of the following reactions at that temperature? SO2(g)+12O2(g)SO3(g) 2SO3(g)2SO2(g)+O2(g) SO3(g)SO2(g)+12O2(g)
63 Following a series of experiments, equilibrium constants were obtained for the reactions below: N2(g) + O2(g) ⇌ 2 NO(g) Kc = 1.50 x 10–30 N2(g) + ½ O2(g) ⇌ N2O(g) Kc = 2.40 x 10–18 What is the equilibrium constant for the following reaction? N2O(g) + ½ O2(g) ⇌ 2 NO(g) Group of answer choices 1.60 x 1012 2.40 x 10-18 3.60 x 10-48 1.60 x 10-12 6.25 x 10-13