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conditions? H₂CO3(aq) + 31.7 kJ → H₂O* (aq) + CO2(g) .H₂O* is removed from the system. The volume of the container is halved increasing the pressure in the system. .The temperature is increased. (The reaction is endothermic.) . Carbon dioxide is added to the reaction container. Neon gas is added to the reaction container. at happens to equilibrium when a catalyst is added to tem? lain why increasing pressure shifts equilibrium to the in the reaction below

conditions? H₂CO3(aq) + 31.7 kJ → H₂O* (aq) + CO2(g) .H₂O* is removed from the system. The volume of the container is halved increasing the pressure in the system. .The temperature is increased. (The reaction is endothermic.) . Carbon dioxide is added to the reaction container. Neon gas is added to the reaction container. at happens to equilibrium when a catalyst is added to tem? lain why increasing pressure shifts equilibrium to the in the reaction below

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter18: Thermodynamics And Equilibrium
Section: Chapter Questions
Problem 18.27QP: Hypothetical elements A(g) and B(g) are introduced into a container and allowed to react according...
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1. In which direction will equilibrium shift under each of the following conditions? H₂CO3(aq) + 31.7 kJ ↔ H₂O* + CO2(g) (aq) a. H₂O* is removed from the system. b. The volume of the container is halved increasing the pressure in the system. c. The temperature is increased. (The reaction is endothermic.) d. Carbon dioxide is added to the reaction container. e. Neon gas is added to the reaction container. 2. What happens to equilibrium when a catalyst is added to the system? 3. Explain why increasing pressure shifts equilibrium to the left in the reaction below. 2SO →2SO₂ + O2(g) 3(g) 2(g) 4. Suggest four ways to increase the [NO₂] in the following equilibrium reaction. Indicate if the value of K will be affected by your suggested changes. 2 NO(g) +0₂ 2(g) 2 NO, + 114.6 kJ 2(g)
Transcribed Image Text:1. In which direction will equilibrium shift under each of the following conditions? H₂CO3(aq) + 31.7 kJ ↔ H₂O* + CO2(g) (aq) a. H₂O* is removed from the system. b. The volume of the container is halved increasing the pressure in the system. c. The temperature is increased. (The reaction is endothermic.) d. Carbon dioxide is added to the reaction container. e. Neon gas is added to the reaction container. 2. What happens to equilibrium when a catalyst is added to the system? 3. Explain why increasing pressure shifts equilibrium to the left in the reaction below. 2SO →2SO₂ + O2(g) 3(g) 2(g) 4. Suggest four ways to increase the [NO₂] in the following equilibrium reaction. Indicate if the value of K will be affected by your suggested changes. 2 NO(g) +0₂ 2(g) 2 NO, + 114.6 kJ 2(g)
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