For the reaction represented by A + B +C→D + E, the following data wereobtained:RunA] (mol/L)[B] (mol/L)[C] (mol/L)Initial rate(mol/(Ls)0.00250.00150.00204.50 x 10-49.00 x 10-44.50 x 10-410.00500.00150.002030.00250.00300.00200.00250.00150.00604.05 x 10-3What is the rate law for this reaction?rate = k[A]O rate =- KKAJ?{B][C]rate = k[A][C]²%3Drate = k[A][B][C]? Which of the following scenarios will have the fastest reaction rate?A 0.50 g chunk of magnesium is reacted with 2.0 mol/L hydrochloric acid at21 °C.A 0.50 g piece of magnesium ribbon is reacted with 1.0 mol/L hydrochloric acidat 23 °C.A 0.025 g sample of powdered magnesium is reacted with 2.0 mol/Lhydrochloric acid at 23 °C.A 0.50 g chunk of magnesium is reacted with 2.0 mol/L hydrochloric acid at23 °C.

Since you have posted multiple unrelated questions, we are entitled to answer the first only. 1) The…

For the reaction represented by A + B + C → D + E, the following data were obtained: Run A) (mol/L) [B] (mol/L) [C) (mol/L) |0.0025 |0.0050 |0.0025 |0.0025 0.0020 |0.0020 |0.0020 |0.0060 Initial rate (mol/(Ls) 4.50 x 10-4 9.00 x 10-4 4.50 x 10-4 4.05 x 10-3 |0.0015 1 2 3 |0.0015 0.0030 0.0015 4 What is the rate law for this reaction? rate = k[A] rate = k[A}²{B][C] rate = k[A][C]? rate = k[A][B][C]? %3D

For the reaction represented by A + B + C → D + E, the following data were obtained: Run A) (mol/L) [B] (mol/L) [C) (mol/L) |0.0025 |0.0050 |0.0025 |0.0025 0.0020 |0.0020 |0.0020 |0.0060 Initial rate (mol/(Ls) 4.50 x 10-4 9.00 x 10-4 4.50 x 10-4 4.05 x 10-3 |0.0015 1 2 3 |0.0015 0.0030 0.0015 4 What is the rate law for this reaction? rate = k[A] rate = k[A}²{B][C] rate = k[A][C]? rate = k[A][B][C]? %3D

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.35PAE: 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...

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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.
Can a reaction mechanism ever be proven correct? Can it be proven incorrect?
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.
The reaction H2SeO3(aq) + 6I-(aq) + 4H+(aq) Se(s) + 2I-3(aq) + 3H2O(l) was studied at 0C, and the following data were obtained: [H2SeO3]0 (mol/L) [H+]0 (mol/L) [I]0(mol/L) Initial Rate (mol/L s) 1.0 104 2.0 102 2.0 102 1.66 107 2.0 104 2.0 102 2.0 10-2 3.33 107 3.0 104 2.0 102 2.0 102 4.99 107 1.0 104 4.0 102 2.0 102 6.66 107 1.0 104 1.0 102 2.0 102 0.42 107 1.0 104 2.0 102 4.0 102 13.2 107 1.0 104 1.0 102 4.0 102 3.36 107 These relationships hold only if there is a very small amount of I3 present. What is the rate law and the value of the rate constant? (Assumethatrate=[H2SeO3]t)
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 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 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
Azomethane decomposes into nitrogen and ethane at high temperatures according to the following equation: (CH3)2N2(g)N2(g)+C2H6(g)The rate of the reaction is followed by monitoring the disappearance of the purple color due to iodine. The following data are obtained at a certain temperature. (a) By plotting the data, show that the reaction is first-order. (b) From the graph, determine k. (c) Using k, find the time (in hours) that it takes to decrease the concentration to 0.100 M. (d) Calculate the rate of the reaction when [ (CH3)2N2 ]=0.415M.
Nitrogen monoxide reacts with chlorine to form nitrosyl chloride. NO(g)+12Cl2(g)NOCl(g) The figure shows the increase in nitrosyl chloride concentration under appropriate experimental conditions. The concentration of nitrosyl chloride actually starts at zero, although this fact may be difficult to see in the figure. (a) Write an expression for the rate of reaction in terms of a changing concentration. (b) Calculate the average rate of reaction between 40 and 120 seconds. (c) Calculate the instantaneous rate of reaction after 80 seconds. (d) Calculate the instantaneous rate of consumption of chlorine 60 seconds after the start of the reaction.
The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table were collected. (a) Determine the order of the reaction for each reactant. (b) Write the rate equation for the reaction. (c) Calculate the rate constant for the reaction. (d) Find the rate of appearance of N2 at the instant when [NO] = 0.350 mol/L and [H] = 0.205 mol/L.
Experimental data are listed here for the reaction B: Time (s) IB] (mol/L) 0.00 0.000 10.0 0.326 20.0 0.572 30.0 0.750 40.0 0.890 Prepare a graph from these data, connect the points with a smooth line, and calculate the rate of change of [B] for each 10-s interval from 0.0 to 40.0 s. Does the rate of change decrease from one time interval to the next? Suggest a reason for this result. How is the rate of change of [AJ related to the rate of change of [B] in each time interval? Calculate the rate of change of [AJ for the time interval from 10.0 to 20.0 s. What is the instantaneous rate, A[B]/Ar, when [BI = 0.750 mol/L?
If the reaction:A+BC+D is designated as first order, the rate depends on: a.the concentration of only one reactant. b.the concentration of each reactant. c.no specific concentration. d.the temperature only.