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1. If the reaction below is initially at equilibrium, and then each of the following changes are made, predict which direction the reaction rate will be fastest until equilibrium is once again established: forward, reverse, or no change. H2(g) + Cl2(g) 2 HCl(g) a. the concentration of H₂ is increased forward b. the concentration of HCl is decreased forward c. the concentration of Cl₂ is decreased reverse

1. If the reaction below is initially at equilibrium, and then each of the following changes are made, predict which direction the reaction rate will be fastest until equilibrium is once again established: forward, reverse, or no change. H2(g) + Cl2(g) 2 HCl(g) a. the concentration of H₂ is increased forward b. the concentration of HCl is decreased forward c. the concentration of Cl₂ is decreased reverse

Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter16: Acids And Bases
Section: Chapter Questions
Problem 65AP: . The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in...
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Can you help me to explain step by step with number 1 part A, number 1 part B, and number 1 part C? Can you explain it to me?

Change Made to a Reaction that was at Equilibrium: Increase the concentration of a reactant. Increase the concentration of a product. Decrease the concentration of a reactant. Decrease the concentration of a product. Response: Rate of the forward reaction becomes greater than the rate of the reverse reaction until equilibrium is reestablished. Rate of the reverse reaction becomes greater than the rate of the forward reaction until equilibrium is reestablished. Rate of the forward reaction becomes less than the rate of the reverse reaction until equilibrium is reestablished. Rate of the reverse reaction becomes less than the rate of the forward reaction until equilibrium is reestablished.
Transcribed Image Text:Change Made to a Reaction that was at Equilibrium: Increase the concentration of a reactant. Increase the concentration of a product. Decrease the concentration of a reactant. Decrease the concentration of a product. Response: Rate of the forward reaction becomes greater than the rate of the reverse reaction until equilibrium is reestablished. Rate of the reverse reaction becomes greater than the rate of the forward reaction until equilibrium is reestablished. Rate of the forward reaction becomes less than the rate of the reverse reaction until equilibrium is reestablished. Rate of the reverse reaction becomes less than the rate of the forward reaction until equilibrium is reestablished.
● Definition of equilibrium • Keq: law of mass action ● Le Chatelier's Principle Topics: ● ● ● Properties of acids & bases Brønstead-Lowry Acids & Bases definition Kw & calculating [H3O+], [OH-], pH 1. If the reaction below is initially at equilibrium, and then each of the following changes are made, predict which direction the reaction rate will be fastest until equilibrium is once again established: forward, reverse, or no change. H2(g) + Cl2(g) 2 HCl(g) a. the concentration of H₂ is increased forward b. the concentration of HCl is decreased forward c. the concentration of Cl₂ is decreased versc 2. If the reaction below is initially at equilibrium, and then more NH4* is added, predict which direction the reaction rate will be fastest until equilibrium is once again established: forward, reverse, or no change. Forward If more Hu is added If more wHyt addel, forwa rol NH4* (aq) + H₂O (1) NH3 (aq) + Hut reactant reaction fast until equilibrium reestablished -1 [30+ (aq) 3. Define (a) reversible reaction and (b) equilibrium. A) Reversible reaction is produce original reactant, one where the products of the reaction can themselves react to B.) Equilibrium: Amount of reactant reach a balance istay there, 4. For the reaction below: reverse reaction take place exactly same rate in both direction Reaction takes place in both direction but over all effect forward's 2 NO2 (g) + O2 (g) 2 NO3 (g) a. Write the law of mass action (the equilibrium expression for Keq) Keq = [03] кед [c]c[d] Products Aja (B]b reactants [0₂] [NO₂]² b. If gas concentrations are as follows, 2.10 M NO2, 1.75 M O2, and 1.00 M NO3, calculate Keq 1.00m] 0.130x102 (1.00m) 0.1295 Keq= (2.10m) ³x (675m) 0.130m² (4.41m x1.75m) 0.130 c. Based on the Keq value that you calculated in part b, are the reactants or products predominant (predominant means that there is a greater amount present)? Keq is a less than 1, then equilibrium will shift to reverse direction.
Transcribed Image Text:● Definition of equilibrium • Keq: law of mass action ● Le Chatelier's Principle Topics: ● ● ● Properties of acids & bases Brønstead-Lowry Acids & Bases definition Kw & calculating [H3O+], [OH-], pH 1. If the reaction below is initially at equilibrium, and then each of the following changes are made, predict which direction the reaction rate will be fastest until equilibrium is once again established: forward, reverse, or no change. H2(g) + Cl2(g) 2 HCl(g) a. the concentration of H₂ is increased forward b. the concentration of HCl is decreased forward c. the concentration of Cl₂ is decreased versc 2. If the reaction below is initially at equilibrium, and then more NH4* is added, predict which direction the reaction rate will be fastest until equilibrium is once again established: forward, reverse, or no change. Forward If more Hu is added If more wHyt addel, forwa rol NH4* (aq) + H₂O (1) NH3 (aq) + Hut reactant reaction fast until equilibrium reestablished -1 [30+ (aq) 3. Define (a) reversible reaction and (b) equilibrium. A) Reversible reaction is produce original reactant, one where the products of the reaction can themselves react to B.) Equilibrium: Amount of reactant reach a balance istay there, 4. For the reaction below: reverse reaction take place exactly same rate in both direction Reaction takes place in both direction but over all effect forward's 2 NO2 (g) + O2 (g) 2 NO3 (g) a. Write the law of mass action (the equilibrium expression for Keq) Keq = [03] кед [c]c[d] Products Aja (B]b reactants [0₂] [NO₂]² b. If gas concentrations are as follows, 2.10 M NO2, 1.75 M O2, and 1.00 M NO3, calculate Keq 1.00m] 0.130x102 (1.00m) 0.1295 Keq= (2.10m) ³x (675m) 0.130m² (4.41m x1.75m) 0.130 c. Based on the Keq value that you calculated in part b, are the reactants or products predominant (predominant means that there is a greater amount present)? Keq is a less than 1, then equilibrium will shift to reverse direction.
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