Use the initial rates method with the given data to determine the rate law for the hypothetical reaction shown below. mol A+B C Trial [A]() [B](ml) A/A] (mol) At 1 0.015 0.015 2.068875 × 10-9 -9 2 0.015 0.018 2.97918 10 3 0.018 0.015 2.48265 10° -9 • Write the rate law in the form of rate = k[A] [B]", specifying the value of the rate constant (k) and the reaction orders (m and n). • Include two significant figures in the rate constant. • Do not include units for the rate constant. Provide your answer below: rate

11.102 Suppose that you are studying a reaction and need to determine its rate law. Explain what you would need to measure in order to accomplish this in a single experiment, and how you could use graphical methods to get from the experimental data to a complete rate law.

Explain how a species might be part of a rate law but not part of a balanced chemical reaction.

The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.

Explain what is meant by the average rate of a reaction.

Consider the following hypothetical data collected in two studies of the reaction 2A+2BC+2D Time(s) Experiment 1 [A] (mol/L) Experiment 2 [A] (mol/L) 0 1.0 102 1.0 102 10. 8.4 103 5.0 103 20. 7.1 103 2.5 103 30. ? 1.3 103 40. 5.0 103 6.3 104 In Experiment 1, [B]0 = 10.0 M. In Experiment 2, [B]0 = 20.0 M. Rate=[A]t a. Use the concentration versus time data to determine the rate law for the reaction. b. Solve for the value of the rate constant (k) for the reaction. Include units. c. Calculate the concentration of A in Experiment 1 at t =30.s

11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been obtained: [NOJ [HJ Rate = A(N2]/At (mol L~1) (mol L_1) (mol L-1 s_1) 5.0 X 10’1 0.32 0.012 1.0 X 10~’ 0.32 0.048 1.0 X 10"2 0.64 0.096 Derive a rate law for the reaction and determine the value of the rate constant.

Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.

Consider the hypothetical reaction A+B+2C2D+3E In a study of this reaction three experiments were run at the same temperature. The rate is defined as [B]/t. Experiment 1: [A]0 = 2.0 M [B]0 = 1.0 103 M [C]0 = 1.0 M [B] (mol/L) Time(s) 2.7 104 1.0 105 1.6 104 2.0 105 1.1 104 3.0 105 8.5 105 4.0 105 6.9 105 5.0 105 5.8 105 6.0 105 Experiment 2: [A]0 = 1.0 102M [B]0 = 3.0 M [C]0 = 1.0 M [A] (mol/L) Time(s) 8.9 103 1.0 7.1 103 3.0 5.5 103 5.0 3.8 103 8.0 2.9 103 10.0 2.0 103 13.0 Experiment 3: [A]0 = 10.0 M [B]0 = 5.0 M [C]0 = 5.0 101M [C] (mol/L) Time(s) 0.43 1.0 102 0.36 2.0 102 0.29 3.0 102 0.22 4.0 102 0.15 5.0 102 0.08 6.0 102 Write the rate law for this reaction, and calculate the value of the rate constant.

The rate law for a reaction can be determined only from experiment and not from the balanced equation. Two experimental procedures were outlined in Chapter 12. What are these two procedures? Explain how each method is used to determine rate laws.