Calcium oxide is used to remove the pollutant SO₂ from smokestack gases by the following exothermic reaction: 2 CaO (s) + 2 SO2 (g) + O2(g) CaSO4 (s) If the system was at equilibrium, what effect would each of the following have on the system. For your answer, indicate whether the reaction shifts to the left, shifts to the right, or no change to reestablish equilibrium. a. The concentration of SO₂ is decreased. b. Additional CaO is added to the system. c. The volume of the container the reaction is placed in decreases. d. The container that contains the reaction is heated in a hot water bath.

Calcium oxide is used to remove the pollutant SO₂ from smokestack gases by the following exothermic reaction: 2 CaO (s) + 2 SO2 (g) + O2(g) CaSO4 (s) If the system was at equilibrium, what effect would each of the following have on the system. For your answer, indicate whether the reaction shifts to the left, shifts to the right, or no change to reestablish equilibrium. a. The concentration of SO₂ is decreased. b. Additional CaO is added to the system. c. The volume of the container the reaction is placed in decreases. d. The container that contains the reaction is heated in a hot water bath.

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...

See similar textbooks

Similar questions

The reaction is at equilibrium at some temperature, T, and the following equilibrium concentrations are measured: [SO2] = 0.90 M, [O2] = 0.35 M, and [SO3] = 1.1 M. Write the equilibrium expression for this reaction. Calculate Keq for the reaction at temperature, T.
Carbon dioxide and water react to form methanol and oxygen, like this: 2 CO,(g)+4 H,O(g)→2 CH;OH(1)+3 O,(g) At a certain temperature, a chemist finds that a 4.6 L reaction vessel containing a mixture of carbon dioxide, water, methanol, and oxygen at equilibrium has the following composition: compound amount CO2 3.94 g H,0 4.50 g CH,OH 3.68 g O2 2.67 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. M K = 0 Lo B Cisc M Explanation Check A Chem 02022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessibility 9 Type here to search (99+ IA ASUS ZenBook Esc F2 F3 F4 F5 F6 F7 F8 %23 %24 21 4. * 6. L. R Y 3)
11
Mercury(II) oxide decomposes to form mercury and oxygen, like this: 2 HgO(s)→2 Hg(1)+O2(g) At a certain temperature, a chemist finds that a 3.3 L reaction vessel containing a mixture of mercury(II) oxide, mercury, and oxygen at equilibrium has the following composition: compound amount HgO 19.5 g Hg 14.6 g O2 0, 17.4 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0 x10
Define equilibrium constant Keq
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2×10-4 at a certain temperature. If a solid sample of NH4SH decomposes, what is the equilibrium concentration of NH3 be?
Consider the following equilibrium reaction:H2(g) + I2(g) ↔ 2HI(g)If the following equilibrium concentrations are observed: [H2] = 4.10 x 10-1M, [I2] = 5.54 x 10-2M, [HI] = 3.50 x 10-2M; what is the equilibrium constant
Write the equilibrium constant expression. Solid carbon and carbon dioxide gas react and form carbon monoxide: C(s) + CO₂(g) = 2CO(g)
Consider the following exothermic reaction at equilibrium: N2 ( g ) + 2H2 ( g ) ⇌ 2NH3 ( g ) Predict how the following changes affect the number of moles of each component of the system after equilibrium is reestablished by completing the table below. Complete the table with the terms increase, decrease, or no change.
Consider the following exothermic reaction at equilibrium: N2 (g) + 2H2 (g) ⇌ 2NH3 (g) Predict how the following changes affect the number of moles of each component of the system after equilibrium is reestablished by completing the table below. Complete the table with the terms increase, decrease, or no change
Nitrosyl bromide decomposes to NO and Br2 in an endothermic process (A,H° = 16.3 kJ/mol-rxn). 2 NOBr(g) ⇒ 2 NO(g) + Br2 (g) Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. a. adding more NOBr(g) shift left shift right O no change b. adding more Br₂(g) shift left shift right O no change c. increasing the volume of the reaction flask shift left shift right O no change d. lowering the temperature shift left shift right O no change
When nitrogen gas reacts with oxygen gas, nitrogen monoxide gas forms: N2(g) + O2(g) ⇋2NO(g) Initially, 0.40 mol of each reactant is placed into a 2.0 L container and equilibrium is established. If Keq=50.1 for the reaction, what are the equilibrium concentrations of all reactants and products? What two conditions are required, if we want to move reaction forward.