3. Determine the reaction order and reaction rate constant for the decomposition of ozone in water using the data given in the following table, considering zero-, first-, and second-order reactions. Time (min) 0 2 5 9 15 O3 concentration (mg/L) 4.5 3.3 2.1 1.2 0.5

Evaluate the following data to determine whether the reaction is first or second order. Calculate the rate constant and be certain to give its unit. A → Product   A (mmol/L) Time (sec) 1.00 0 0.50 11 0.25 20 0.10 48 0.05 105

Initial rates were measured for the following reaction and are listed in the table. A + 2B ⎯→ products   Expt. Initial Concentrations Initial Rate (mol/L·s) [A] [B] 1 0.115 0.135 2.70 × 10−3  2 0.115 0.270 2.16 × 10−2  3 0.345 0.135 8.10 × 10−3  What is the order of the reaction with respect to A, with respect to B, and overall?

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8. Rates for a certain chemical reaction involving the reactant A were measured as a function of the concentration of A, and these data were plotted in the graph below. What is the order of the reaction with respect to A, and what is the rate constant for the reaction? 0.012 0.010 0.008 0.006· 0.004 0.002 0. 0.2 0.4 0.6 0.8 1 [A](M) A) order with respect to A = 0, k = 0.010 s-l B) órder with respect to A = 1, k = 0.010 s C) order with respect to A = 2, k = 0.00 s- D) order with respect to A = 0, k = 10 s E) order with respect to A = 1, k = 100 s- 11:2 a 2/18 Cop Rate (M/s)

36  The reaction C2H5Cl →C2H4  + HCl is first order in C2H5Cl. The rate constant is 1.60 x 10-6/s. In an investigation of the decomposition of C2H5Cl an initial concentration of 0.165 mol/L was used. What will  the concentration of C2H5Cl be after 125 hours? Select one: a. 0.0803 M b. 0.0703 M c. 0.0603 M d. 0.0503M

B 8. D Trial 1 2 3 4 [A₂] 0.10 0.20 0.30 0.30 [B] 0.50 0.50 0.05 0.10 An experiment was conducted to determine the rate law for the reaction A2(g) + B(9) A₂B(g). The table above shows the data collected. Based on the data in the table. which statement is correct? Initial rate (Ms-¹) 2.5 x 10 5.0 x 10-4 5.0 × 10-5 1.0 x 10-4 Since the rate law can be expressed as ratek[A₂), tripling the concentration of A2 will cause a 9-fold increase in the rate of the reaction. Since the rate law can be expressed as rate k[A₂][B], doubling the concentrations of A₂ and B will quadruple the rate of the reaction. Since the rate law can be expressed as rate k[A] [B], tripling the concentration of A2 while keeping the concentration of B constant will triple the rate of the reaction. Since the rate law can be expressed as rate=k[A₂][B], doubling the concentration of B while keeping the concentration of A₂ constant will double the rate of the reaction.

The reaction between hydrogen and chlorine is as follows: Cl2(g) + H2(g) → 2HCl(g) Experiments show that this reaction is first order with respect to H2 and one-half order with respect to Cl2. What is the rate law?   a. Rate = k [H2]1/2 [Cl2] b. Rate = k [Cl2] [H2]2 c. Rate = k [Cl2]1/2 [H2] d. Rate = k [Cl2]2 [H2]

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1. For an irreversible reaction A products, the graph of 1/[A] as a function of time is linear. What is the reaction order in A? a. Zeroth-order b. First-order c. Second-order d. The order in A cannot be determined based on the information given. 2. A proposed mechanism for the reduction of nitrogen as NO by hydrogen is: Step 1: H₂(g) + 2 NO (g) → N₂O (g) + H₂O (g) Step 2: N₂O (g) + H₂ (g) → N2 (g) + H₂O (g) What is the molecularity of Step 2? a. unimolecular b. bimolecular c. termolecular d. zero molecular (spontaneous) e. More information is needed to answer this question. 3. Which one of the following will change the value of an equilibrium constant? a. changing temperature b. adding other substances that do not react with any of the species involved in the equilibrium c. varying the initial concentrations of reactants d. varying the initial concentrations of products e. changing the volume of the reaction vessel