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c. the concentration of the reactants to the rate of the reaction d. the concentration of the products to the concentration of the reactants What is the net reaction equation for the following mechanism? N₂O, (s) NO₂(g) + NO, (g) NO (g) + NO, (g) 2 NO₂(g) a. N₂O, (s) NO₂ (g) + NO, (g) 1 b. N₂O, (s) + NO (g) - 3 NO₂ (g) C. 1 N₂O, (s) + NO (g) 3 NO₂ (g) + NO, (g) d. N₂O, (s) + NO (g) + NO, (g) - 3 NO₂ (g) Consider two reactants, A and B, that produce products C and D. Suppose the equilibrium constant is very large. What does this indicate? a. The production of products is favoured. b. The reaction will not proceed. c. The production of reactants and products is equal. d. The production of reactants is favoured. Sulfuric acid is an important industrial chemical. It is used for fertilizers, detergents, dyes, and medicine. The equilibrium equation for the first step in the contact process is as follows: 2 SO₂(g) + O₂(g) 2 SO, (g), AH=-196 kJ/mol What would you do to increase the production of SO,? a. Raise the temperature considerably to shift the equilibrium to the right. b. Raise the temperature to shift the equilibrium to the right and increase the rate of formation (collision theory). c. Lower the temperature considerably to shift the equilibrium to the right. d. Lower the temperature moderately to shift the equilibrium right while maintaining the rate of formation (collision theory).

c. the concentration of the reactants to the rate of the reaction d. the concentration of the products to the concentration of the reactants What is the net reaction equation for the following mechanism? N₂O, (s) NO₂(g) + NO, (g) NO (g) + NO, (g) 2 NO₂(g) a. N₂O, (s) NO₂ (g) + NO, (g) 1 b. N₂O, (s) + NO (g) - 3 NO₂ (g) C. 1 N₂O, (s) + NO (g) 3 NO₂ (g) + NO, (g) d. N₂O, (s) + NO (g) + NO, (g) - 3 NO₂ (g) Consider two reactants, A and B, that produce products C and D. Suppose the equilibrium constant is very large. What does this indicate? a. The production of products is favoured. b. The reaction will not proceed. c. The production of reactants and products is equal. d. The production of reactants is favoured. Sulfuric acid is an important industrial chemical. It is used for fertilizers, detergents, dyes, and medicine. The equilibrium equation for the first step in the contact process is as follows: 2 SO₂(g) + O₂(g) 2 SO, (g), AH=-196 kJ/mol What would you do to increase the production of SO,? a. Raise the temperature considerably to shift the equilibrium to the right. b. Raise the temperature to shift the equilibrium to the right and increase the rate of formation (collision theory). c. Lower the temperature considerably to shift the equilibrium to the right. d. Lower the temperature moderately to shift the equilibrium right while maintaining the rate of formation (collision theory).

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter12: Kinetics
Section: Chapter Questions
Problem 75E: Experiments were conducted to study the rate of the reaction represented by this equation.[2]...
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18.A chemical reaction rate compares a. the temperature of the reactants to the rate of the reaction b. the surface area of the reactants to the rate of the reaction c. the concentration of the reactants to the rate of the reaction d. the concentration of the products to the concentration of the reactants 19. What is the net reaction equation for the following mechanism? N₂O, (s) NO₂ (g) + NO, (g) - - NO (g) + NO, (g) → 2 NO₂(g) a. N₂O, (s) NO₂ (g) + NO, (g) b. - N₂O₂ (s) + NO (g) → 3 NO₂ (g) C. N₂O₂ (s) + NO (g) 3 NO₂ (g) + NO, (g) d. N₂O, (s) + NO (g) + NO, (g) 3 NO₂ (g) 20. Consider two reactants, A and B, that produce products C and D. Suppose the equilibrium constant is very large. What does this indicate? a. The production of products is favoured. b. The reaction will not proceed. c. The production of reactants and products is equal. d. The production of reactants is favoured. 21.Sulfuric acid is an important industrial chemical. It is used for fertilizers, detergents, dyes, and medicine. The equilibrium equation for the first step in the contact process is as follows: 2 SO₂(g) + O₂(g) → 2 SO, (g), AH=-196 kJ/mol What would you do to increase the production of SO,? a. Raise the temperature considerably to shift the equilibrium to the right. b. Raise the temperature to shift the equilibrium to the right and increase the rate of formation (collision theory). c. Lower the temperature considerably to shift the equilibrium to the right. d. Lower the temperature moderately to shift the equilibrium right while maintaining the rate of formation (collision theory).
Transcribed Image Text:18.A chemical reaction rate compares a. the temperature of the reactants to the rate of the reaction b. the surface area of the reactants to the rate of the reaction c. the concentration of the reactants to the rate of the reaction d. the concentration of the products to the concentration of the reactants 19. What is the net reaction equation for the following mechanism? N₂O, (s) NO₂ (g) + NO, (g) - - NO (g) + NO, (g) → 2 NO₂(g) a. N₂O, (s) NO₂ (g) + NO, (g) b. - N₂O₂ (s) + NO (g) → 3 NO₂ (g) C. N₂O₂ (s) + NO (g) 3 NO₂ (g) + NO, (g) d. N₂O, (s) + NO (g) + NO, (g) 3 NO₂ (g) 20. Consider two reactants, A and B, that produce products C and D. Suppose the equilibrium constant is very large. What does this indicate? a. The production of products is favoured. b. The reaction will not proceed. c. The production of reactants and products is equal. d. The production of reactants is favoured. 21.Sulfuric acid is an important industrial chemical. It is used for fertilizers, detergents, dyes, and medicine. The equilibrium equation for the first step in the contact process is as follows: 2 SO₂(g) + O₂(g) → 2 SO, (g), AH=-196 kJ/mol What would you do to increase the production of SO,? a. Raise the temperature considerably to shift the equilibrium to the right. b. Raise the temperature to shift the equilibrium to the right and increase the rate of formation (collision theory). c. Lower the temperature considerably to shift the equilibrium to the right. d. Lower the temperature moderately to shift the equilibrium right while maintaining the rate of formation (collision theory).
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