40-16X 10. A reaction between substances A and B has been found to give the following data: 3A + 2B 2C+D [A] (mol/L) [B] (mol/L) Rate of appearance of C (mol/L-hr) 1.0 X3 3.0 1.0x10-2 0.300x10-6 1.0x10-2 8.10x10-6 2.0x10-2 3.0 3.24 x10-5 1.20 x10-6 7.30x10-5 2.0x10-2 1.0 3.0x10-2 3.0 Using the above data, determine the order of the reaction with respect to A and B, the rate law, and calculate the specific rate constant. Copyright 2018 Pearson Education, Inc.

40-16X 10. A reaction between substances A and B has been found to give the following data: 3A + 2B 2C+D [A] (mol/L) [B] (mol/L) Rate of appearance of C (mol/L-hr) 1.0 X3 3.0 1.0x10-2 0.300x10-6 1.0x10-2 8.10x10-6 2.0x10-2 3.0 3.24 x10-5 1.20 x10-6 7.30x10-5 2.0x10-2 1.0 3.0x10-2 3.0 Using the above data, determine the order of the reaction with respect to A and B, the rate law, and calculate the specific rate constant. Copyright 2018 Pearson Education, Inc.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A reaction between substances A and B has been found to give the following data: [A] (mol/L) 1.0×10-² 1.0×10-² 2.0×10-² 2.0×10-² 3.0×10-² 3A + 2B > 2C+D [B] (mol/L) 1.0 3.0 3.0 1.0 3.0 Rate of appearance of C (mol/L-hr) 0.300×10-6 8.10×10-6 3.24x10-5 1.20×10-6 7.30×10-5 Using the above data, determine the order of the reaction with respect to A and B, the rate law, and calculate the specific rate constant.
Which statement does not accurately describe chemical equilbirum for a reversible chemical reaction A↔B? Assume the forward rate constant is k1 and the reverse rate constant is k-1, and assume both directions are first order). -d[A]/dt = d[B]/dt k1 = k-1 K = [B]eq/[A]eq K = k1/k-1 None of these
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Questions 8-10 refer to the following energy diagram for a reaction proceeds by a three-step mechanism. F D E В E IA G 8. Which transformation represents the rate-determining step for the reaction? a) A → C b) С >Е c) E → G d) A → E e) С -> G f) A → G
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Chem 112 - Lab Report RATES OF REACTIONS 1. Effect of Concentration Reaction time, Min Mg + 1M-hcl 2.5 Mg + 0.8M-hcl 5.5 Mg + 0.6M-hcl 7.0 Mg + 0.4M-hcl 10.5 2. Effect of Temperature and Catalyst A. Reaction at room temperature 11.0 B. Reaction at 40 °c 5.5 C. Reaction at 55 c 2.5 D. Reaction at 70 °c 1.5 E. Reaction with catalyst 0.5 3. Effect of ph Ph of your unadjusted solution? 2.96__[H+] Time 10.5_ Ph of adjusted solution? _1.52_[H*] Time 5.6_ What is the increase in [H+] between ph adjusted and unadjusted solutions? What difference in reaction times did you observe for the above two solutions? Summarize your results by answering the following questions. Recall that a shorter time to react implies a faster reaction rate. (1) What effect does increasing the concentration of a solution (hcl) have upon the rate of Reaction? (step 1)
he reaction 2 ClO2(aq) + 2 OH-(aq) ClO3-(aq) + ClO3-(aq) + H2O(l) was studied at a certain temperature with the following results: Experiment [ClO2(aq)] (M) [OH-(aq)] (M) Rate (M/s) 1 0.0359 0.0359 0.0209 2 0.0359 0.0718 0.0418 3 0.0718 0.0359 0.0837 4 0.0718 0.0718 0.167 (a) What is the rate law for this reaction? Rate = k [ClO2(aq)] [OH-(aq)] Rate = k [ClO2(aq)]2 [OH-(aq)] Rate = k [ClO2(aq)] [OH-(aq)]2 Rate = k [ClO2(aq)]2 [OH-(aq)]2 Rate = k [ClO2(aq)] [OH-(aq)]3 Rate = k [ClO2(aq)]4 [OH-(aq)] (b) What is the value of the rate constant?(c) What is the reaction rate when the concentration of ClO2(aq) is 0.0640 M and that of OH-(aq) is 0.0732 M if the temperature is the same as that used to obtain the data shown above? M/s
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When [F] is decreasing at 0.15mol/Lxs, how fast is [G] increasing? Be sure to use correct number of significant figures.
A+B- -AB Trial (A] (M) (B] (M) Rate (M/s) 1 0.200 0.200 2.00 x 102 0.400 0.200 8.00 x 102 0.200 0.400 4.00 x 102 What is the rate constant for the reaction above? 2.
16. The reaction between A and B is %23 as follows: * A + 2B 2C The rate of reaction with variation of concentration of A and B at the same temperature is shown in Table 2. Table 2 Experiment [A]/mol dm [B/mol dm 2.00 1.50 1.00 0.50 1.00 1.00 1.50 2.00 Rate of reaction Imol dm s 1.20 x 10 9.00 x 10 1.35 x 10 II III IV What is the value of x? 3.00x 10 B..00 x 103 C. 1.20x 102 D. 2.40 x 102 A.3.00X 10-7 B.6.00 x10 C.1-20 X10-3 b- 240 x 10-3 you 20
The following experimental data were obtained for the reaction of NH,+ and NO2- in acidic solution. NH, + (aq) + NO2 (aq) → N2 (g) +2 H2O(€) [NH, ] (mol L) NO, ¯] (mol L1) Rate = A[N2]/At (mol L-s) 0.0096 0.110 3.06 x 10-7 0.0096 0.055 1.53 x 10-7 0.0509 0.220 3.25 x 10-6 0.0259 0.220 1.65 x 10-6 Determine the rate law for this reaction. (Use k for the rate constant.) Rate = Calculate the rate constant. Rate constant =| mol L-1s 1 Try s1 L mol-1 s-1 L² mol-2 Submit Answer 9 item attempts remaining