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...

See similar textbooks

Similar questions

8
Time (s) [D] (M) 2D + E → D₂E 0 5.00 100 4.35 second-order in The reaction above is reactant D and has the concentration versus time data given at 300 K. What is the rate constant for the reaction? k = [?] x 10? M-1.5-1 coefficient (green) exponent (yellow) Enter
Consider the reaction A + 2B = C whose rate at 25°C was measured using three different sets of initial concentrations as listed in the following table: Trial [A] [B] (M) (M) 1 0.30 0.030 3.2x10-3 2 0.30 0.060 6.5×10-3 3 0.60 0.030 1.3x10-2 Rate (M/s) Part B Calculate the initial rate for the formation of C at 25 °C, if [A] = 0.50 M and [B] = 0.075 M. Express your answer to two significant figures and include the appropriate units. ► View Available Hint(s) μA initial rate=0.0225 Submit Previous Answers m S ?
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.
15. The data in the table below were obtained for the reaction: (Show your work!!) 2c1o, 20H > cio, + CIo + H,O Initial Rate (M/s) Experiment Number [CO.)(M) (OH ](M) 0.060 0.030 0.0248 0.020 0.030 0.00276 0.020 0.090 0.00828 a) What is the order of the reaction with respect to CIO,? b) What is the order of the reaction with respect to OH? c) What is the overall order of the reaction?
Need help 6 Use sig figs