Complete the following chart by writing "LEFT", "RIGHT" OR "NONE" for equilibrium shift, and "INCREASES", "DECREASES" or "REMAINS THE SAME" for the concentrations of reactants and products when the indicated stressors are applied to the given system at equilibrium. OSS -AUTON NR « Eo > «SON MA Equilibrium Shift Concentration of SO2 2 SO₂ (8) + 0₂ (8) Concentration of 02 → 2 SO 3 (g) Concentration of SO3

Complete the following chart by writing "LEFT", "RIGHT" OR "NONE" for equilibrium shift, and "INCREASES", "DECREASES" or "REMAINS THE SAME" for the concentrations of reactants and products when the indicated stressors are applied to the given system at equilibrium. OSS -AUTON NR « Eo > «SON MA Equilibrium Shift Concentration of SO2 2 SO₂ (8) + 0₂ (8) Concentration of 02 → 2 SO 3 (g) Concentration of SO3

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The equilibrium constant, Kc, for the following reaction is 2.90×10-2 at 1.15×103K.2SO3(g) 2SO2(g) + O2(g)If an equilibrium mixture of the three gases in a 19.0 L container at 1.15×103K contains 0.291 mol of SO3(g) and 0.381 mol of SO2, the equilibrium concentration of O2 is M.
Nitric acid and nitrogen monoxide react to form nitrogen dioxide and water, like this: 2 HNO,(aq)+NO(9)-3 NO,(g)+H,0(1) At a certain temperature, a chemist finds that a 5.0 L reaction vessel containing a mixture of nitric acid, nitrogen monoxide, nitrogen dioxide, and water at equilibrium has the following composition: compound amount HNO3 22.6 g NO 15.5 g NO2 21.9 g H,0 107.8 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K, = 0 Plecy Terms of Use ©2021 McGraw-Hl Education All Rights Reserved Check Explanation
For the following chemical reaction, CO (g) + H2O (g) <----> CO2 (g) + H2 (g) Kc = 0.0257 If a 2.00L vessel is charged with 0.200 moles of CO, 1.13 moles of H2O, 0.199 moles of CO2, and 0.175 moles of H2, in which direction does the reaction progress to establish equilibrium?
A mixture of 30.0 mol of NO(g) and 18.0 mol of O2(g) is placed in an empty 3.00-liter flask held at a constant temperature. These gases react until the reaction represented below comes to equilibrium. At equilibrium, the vessel contains 26.4 moles of NO2. What is the value of the equilibrium constant at the constant temperature? 2NO(g) + O2(g)  2NO2(g)
For this reaction, the equilibrium constant, Kea, is 6.1 x 10-4 SO3 (g) - O2 (g) + 2SO3 (g) Select the most accurate statement. O the equilibrium favors reactants O the rate of the forwards reaction is very fastfast O at equilibrium, the reaction mixture will contain a lot of both reactants and products O the rate of the forwards reaction is very slow O the equilibrium favors products
Nitric acid and nitrogen monoxide react to form nitrogen dioxide and water, like this: 2 HNO3(aq)+NO(g)→ 3 NO,(g)+H,0(1) At a certain temperature, a chemist finds that a 4.5 L reaction vessel containing a mixture of nitric acid, nitrogen monoxide, nitrogen dioxide, and water at equilibrium has the following composition: compound amount dlo HNO3 14.2 g 18 Ar NO 7.3 g NO, 19.2 g H,O 87.0 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0 x10 ?
The following reaction has an equilibrium constant Kc equal to 3.07 x 10-4 at 24 °C. 2 NOBr (g) ⇋⇋ 2 NO (g) + Br2 (g) If the composition of the mixture has the following concentrations, decide whether the reaction is at equilibrium. If it is not, decide which direction the reaction should go. [NOBr] = 0.0472 M, [NO] = 0.0121 M, [Br2] = 0.0105 M Select one: a. The reaction is at equilibrium. b. The reaction is not at equilibrium and will proceed towards the products to reach equilibrium. c. The reaction is not at equilibrium and will proceed towards the reactants to reach equilibrium.
General Chemistry 4th Edition McQuarrie Rock Gallogly An equilibrium mixture contains 0.500 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00 L container. CO(g) + H₂O(g) = CO₂(g) + H₂(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished? moles of CO₂: University Science Books presented by Macmillan Learning »))) R. mol
Consider the following reaction and its equilibrium constant: 12 (g) + Br2 (g) ÷ 2 IBr (g) Kc = 1.1 × 102 A reaction mixture contains 0.41 M I2, 0.27 M Br2 and 2.2 M IBr. Which of the following statements is TRUE concerning this system? O The equilibrium constant needs to increase. The reaction needs to shift in the direction of the reactants to reach equilibrium. O The system is at equilibrium. O The reaction needs to shift in the direction of the products to reach equilibrium.
(a) At 2000°C, the equilibrium constant for the reaction: N2(g) + O2(g) > 2 NO(g) is 4.1 x 10-4 If the initial concentration are [N2] = 0.2 M and [O2] = 0.1 M, how much of each of the components will be present at equilibrium?
Part A The equilibrium constant, Kc, for the decomposition of COC2 to CO and Cl2 is 0.68. If an equilibrium mixture contains 0.38 M CÓ and 0.55 M Cl2, what is the molar concentration of COCl2 ? COC2 (g) = CO(g) + Cl2 (g) Express your answer to two significant figures and include the appropriate units.