A 100% 7:07 PM Wed Feb 5 Unanswered •1 attempt left For reaction 2A + 3B → 2C + D, following data of concentration and rate was obtained Trial Initial [A] Initial [B] Initial Rate (M/sec) 10.015 M 0.200 M 3.67 × 10^-6 20.030 M 0.200 M 7.33 × 10^-6 3 0.015 M 0.400 M 1.47 × 10^-5 The special rate constant k 1.2 x 10^-3 (1/M•sec) 9.2 × 10^-4 (1/M•sec) 1.6 x 10^-3 (1/M-sec) 6.1 × 10^-3 (1/M^2·sec) D 8.2 x 10^-3 (1/M^2•sec) Submit ш

A 100% 7:07 PM Wed Feb 5 Unanswered •1 attempt left For reaction 2A + 3B → 2C + D, following data of concentration and rate was obtained Trial Initial [A] Initial [B] Initial Rate (M/sec) 10.015 M 0.200 M 3.67 × 10^-6 20.030 M 0.200 M 7.33 × 10^-6 3 0.015 M 0.400 M 1.47 × 10^-5 The special rate constant k 1.2 x 10^-3 (1/M•sec) 9.2 × 10^-4 (1/M•sec) 1.6 x 10^-3 (1/M-sec) 6.1 × 10^-3 (1/M^2·sec) D 8.2 x 10^-3 (1/M^2•sec) Submit ш

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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For the following reaction 4 experiments have been run and the data collected is in the following table: 2 MnO, (aq) + 5 H,C,0, (aq) + 6 H* (aq) 2 Mn2+ (aq) + 10 CO2 (g) + 8 H,0 (1) Experimen [MnO,], M [H,C,O,], M [H*], M Rate, M/s t 1 0.2410 0.3470 0.2690 0.1147 2 0.3260 0.6210 0.2270 0.2776 3 0.5630 0.5740 0.7420 0.4431 4 0.2410 0.3470 0.3840 0.1147 0.4140 0.5740 0.5610 0.3258 6. 0.3260 0.4930 0.4910 0.2203
For the reaction A+B+CD+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Trial 1 2 3 4 [Α] (M) 0.30 0.30 0.60 0.60 B (M) 0.30 0.30 0.30 0.60 с IM (M) 0.30 0.90 0.30 0.30 Initial rate (M/s) 9.0x10-5 2.7x10-4 3.6x10 3.6x10+ What is the reaction order with respect to C? Express your answer as an integer. ▸ View Available Hint(s) 1 Submit Previous Answers ✓ Correct The rate tripled when [C] was tripled. This indicates an order of 1 with respect to C because 3 = 3¹. ▾ Part D What is the value of the rate constant for this reaction? When entering compound units, indicate multiplication of units explicitly using a multiplication dot (in the menu). For example, M¹s¹. Express your answer to two significant figures and include the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot or a dash. ▸ View Available Hint(s) k= 3.3x103 M-2.s-¹ Submit Previous Answers All attempts…
5:15 PM Wed Mar 15 Question 18 of 75 What is the rate at which Br(aq) disappears in the reaction below if the rate of disappearance of BrO3(aq) is 0.059 M/s? BrO₂ + 5 Br + 6 H 3 Br₂ + 3H₂O Tap here or pull up for additional resources - 4 7 +/- 2 3 LO 80 M/S 5 9 O LTE 15% Submit 冈。 x 100
A 100% 7:07 PM Wed Feb 5 3 ... Unanswered •1 attempt left Rate law of a reaction is experimentally determined as Rate = k [A]^2 [B] The unit of k is 1/(M^2-sec) 1/(M-sec) sec/M M/sec M^2/sec Submit
The rate of the reaction (A[CI/Ar) was measured in three trials with varying initial concentrations of the reactants. [B] (M) A[CV/AI (M/s) Trial order: 3 order: [A]o (M) 0.600 0.600 rate = k 1.20 0.250 0.500 0.500 What is the order of the reaction with respect to reactant A? 3.05 x 10-6 What is the rate law for this reaction? 1.22 x 10-5 What is the order of the reaction with respect to reactant B? 1.22 x 10-5
The following initial rate data were found for the reaction 2MnO4 +5H₂C2O4 + 6H+ → 2 Mn²+ [-] (M) {H+] (M) 1.00×10-3 1.0 1.00×10-3 1.0 2.00×10-3 1.0 2.00×10-3 2.0 Experiment 1 [MnO4-] (M) 1.00×10-3 2.00×10-3 2.00×10-3 2.00×10-3 The rate law for this reaction is 2 (ر) Rate = k[MnO4]²[H₂C₂O4][H+] Rate = k[MnO4]²[H₂C₂O4]5[H+]6 Rate = k[MnO4]²[H₂C₂O4] Rate = k[MnO4][H₂C₂O4][H+] Rate = k[MnO4]²[H₂C₂O4]² + 10 C Rate (M/s) 2.0×10-4 8.0×10-4 1.6x10-3 1.6×10-3
I’m not sure where I went wrong. Please help with a and b.
Need help 6 Use sig figs
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