Match the Term with the definition 1. Equilibrium position 2. Chemical equilibrium 3. Reaction quotient 4. Law of mass action 5. Equilibrium constant C a. used to determine if a reaction has reached equilibrium b. depends on the initial concentrations of the substances in a reaction c. states that every reaction proceeds to an equilibrium state with a specific Keq d. the point at which the reaction appears to "stop" e. the ratio of product concentration to reactant concentration at equilibrium 6. For the reaction N2 (g) + O2(g) 2 NO(g) that is run at 25 °C, Kc = 1.2 × 10-30. Use this information to calculate the equilibrium co for the reaction 2 NO(g) N2 (g) + O2(g) a. 8.3 x 1029 b. 1.2 x 10-30 C. 1.7 x 1030 d. 1.1 x 10-15 e. 6.0 × 10-31 7. Write the equilibrium expression for the formation of nitrosyl bromide. a. [NO] 2 [Br]/[NOBr] 2 b. [NOBr]2/[NO] 2 c. [NOBr] 2/[NO] 2 [Br2] d. [NO] 2[Br2] / [NOBr] 2 e. [NOBr] 2/[NO]² 2NO(g) + Br2 (g) 2NOBr(g)

Match the Term with the definition 1. Equilibrium position 2. Chemical equilibrium 3. Reaction quotient 4. Law of mass action 5. Equilibrium constant C a. used to determine if a reaction has reached equilibrium b. depends on the initial concentrations of the substances in a reaction c. states that every reaction proceeds to an equilibrium state with a specific Keq d. the point at which the reaction appears to "stop" e. the ratio of product concentration to reactant concentration at equilibrium 6. For the reaction N2 (g) + O2(g) 2 NO(g) that is run at 25 °C, Kc = 1.2 × 10-30. Use this information to calculate the equilibrium co for the reaction 2 NO(g) N2 (g) + O2(g) a. 8.3 x 1029 b. 1.2 x 10-30 C. 1.7 x 1030 d. 1.1 x 10-15 e. 6.0 × 10-31 7. Write the equilibrium expression for the formation of nitrosyl bromide. a. [NO] 2 [Br]/[NOBr] 2 b. [NOBr]2/[NO] 2 c. [NOBr] 2/[NO] 2 [Br2] d. [NO] 2[Br2] / [NOBr] 2 e. [NOBr] 2/[NO]² 2NO(g) + Br2 (g) 2NOBr(g)

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 1RQ: Characterize a system at chemical equilibrium with respect to each of the following a. the rates of...

See similar textbooks

Similar questions

. The equilibrium constant for the reaction 2NOCl(g)2NO(g)+Cl2(g)has the value 9.2106at a particular temperature. The system is analyzed at equilibrium, and it is found that the concentrations of NOCl(g) and NO(g) are 0.44 M and 1.5103M. respectively. What is the concentration of Cl2(g) in the equilibrium system under these conditions?
A reaction is represented by this equation: A(aq)+2B2C(aq) Kc=1103 (a) Write the mathematical expression for the equilibrium constant. (b) Using concentrations M, make up two sets of concentrations that describe a mixture of A, B, and C at equilibrium.
Colorless hydrogen gas (H2) and red-brown colored bromine gas (Br2) reacts to form colorless HBr gas. Describe how the concentrations of H2, Br2, and HBr would change increase or decrease as equilibrium was established in a sealed container that initially contained only H2 and Br2. What observation would indicate that equilibrium had been established?
Characterize a system at chemical equilibrium with respect to each of the following a. the rates of the forward and reverse reactions b. the overall composition of the reaction mixture For a general reaction3A(g)+B(g)2C(g), if one starts an experiment with only reactants present, show what the plot of concentrations of A, B, and C versus time would look like. Also sketch the plot illustrating the rate of the forward reaction and rate of the reverse reaction versus time.
. For a given reaction at a given temperature, the special ratio of products to reactants defined by the equilibrium constant is always equal to the same number. Explain why this is true, no matter what initial concentrations of reactants (or products) may have been taken in setting up an experiment.
Which of the diagrams for Questions 107 and 108 best represents an equilibrium mixture with an equilibrium constant of (a) 0.44? (b) 4.0? (c) 36?
Explain that equilibrium is dynamic, and that at equilibrium the forward and backward reaction rates are equal.
The following series of diagrams represent the reaction XY followed over a period of time. The X molecules are red and the Y molecules are green. At the end of the time period depicted, has the reaction system reached equilibrium? Justify your answer with a one-sentence explanation.