What are the true statements?: A. The rate law for a reaction can be determined from the stoichiometry of the overall reaction. B. Most reaction rates will decrease with time. C. If ln k and 1/T are plotted for a reaction, the activation energy is the negative of the slope divided by R. D. The rate constant for a reaction depends on the concentration of the reactant for a first order reaction. E. The rate of reaction usually decreases if the temperature of the reaction is decreased. F. The products of a reaction are lower in energy than the reactants

A reaction has a rate constant of 0.0117/s at 400.0 K and 0.689/s at 450.0 K.a. Determine the activation barrier for the reaction.b. What is the value of the rate constant at 425 K?

The rate law of the decomposition of silane (SiH4) Rate = k[SiH4]1                It takes 125 seconds for 2.00 M silane to decrease to 0.20 M at 240oC. a. Right the integrated rate law for the decomposition of silane. b. Determine the value and unit of the rate constant.  c. How much time is required for 3.00 M silane to decrease to a concentration of 0.600 M.

Which of the following is true: I. First order reactions proceed at a constant rate II. First order reactions have a constant half-life III. First order reactions have one reactant O a. Il only O b. I, II, and II O c. Il and II O d. I only O e. I and II

Calculate the initial concentration for a zero order reaction with a final concentration of 0.848 M, a rate constant of 0.00966 M/min, at 62.1 minutes. a. 1.45 b. 4.01 c. none of these d. 1.54 e. 1.73

Consider the mechanism shown here: 2 NO N202 N202 + H2 →N20 + H20 (slow step) N20 + H2→N2 + H2O For the overall reaction, what would you predict the order of the kinetics with respect to H2 to be? a. second order Ob. zeroeth order C. I need to do a kinetics experiment to decide. a. first order

5. If 0.020 M KI was used instead of 0.010 M KI, how would this effect: a. the rate of the reaction? b. the value of the rate constant “k"?

At 330 degrees Celsius, the rate constant for the second order decomposition of NO2 is 0.775M ^ - 1 * s ^ - 1 the Initial concentration of NO2 is 0.0500M a. Write the rate law expression for this reaction b. What is the concentration of NO2 after 30.0 minutes? c. How long in minutes will it take the concentration to decrease to 0.0050M? d. What is the half life for this reaction? e. What effect would doubling the NO2 concentration have on the rate of the reaction?

a. What is the overall order of the reaction? b. Write the rate expression. c. Calculate the rate constant, k. d. If the concentration of MnO4-, H2C2O4, & H+ are 0.155 M, 0.293M, and 0.475M respectively, what is the rate of the reaction?

d. There is too little information to assess the change. 8. If a reaction is first order with respect to [A], doubling the concentration of [A] will: a. double the rate of the reaction. b. increase the rate of the reaction fourfold. c. increase the rate of the reaction eightfold. d. not affect the rate of the reaction. 207 9. If a reaction is zero order with respect to [C], tripling the concentration of [C] will: a. triple the rate of the reaction. b. result in a fourfold increase in the rate of the reaction. c. result in a ninefold increase in the rate of the reaction. d. no impact on the rate of the reaction. 10. If a reaction is second order with respect to [B], doubling the concentration of [B] will: a. double the rate of the reaction. b. result in a fourfold increase in the rate of the reaction. c. result in an eightfold increase in the rate of the reaction. d. not affect the rate of the reaction. 11. For a second-order reaction, the plot of 1/[concentration] with respect to time…