14. The data in the table below was collected for the following reaction at 425°C. 2 A(g) + 3 B(g) →3 C(g) +2 D(g) Trial 1 2 3 4 [A] i, M [B]i, M Initial Rate, M/s 0.100 0.050 1.0 × 10-3 0.050 0.050 2.5 × 10-4 0.100 0.100 2.0 × 10-3 0.150 0.100 4.5 x 10-3 a. What is the rate law for this reaction? b. What is the overall order of the reaction? 15. The rate constant for the following reaction is 3.00 x 10-3 M-1 min-1 at 500 K:

14. The data in the table below was collected for the following reaction at 425°C. 2 A(g) + 3 B(g) →3 C(g) +2 D(g) Trial 1 2 3 4 [A] i, M [B]i, M Initial Rate, M/s 0.100 0.050 1.0 × 10-3 0.050 0.050 2.5 × 10-4 0.100 0.100 2.0 × 10-3 0.150 0.100 4.5 x 10-3 a. What is the rate law for this reaction? b. What is the overall order of the reaction? 15. The rate constant for the following reaction is 3.00 x 10-3 M-1 min-1 at 500 K:

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

Consider the reaction: NO2 + 03 → NO3 + 02 [NO,], M [02], M Rate, M/s 6.30 x 10-3 Experiment 1 0.21 0.70 1.89 × 10-2 3.15 x 10-3 2 0.63 0.65 3 0.21 0.35 4 0.42 0.35 6.30 x 10-3 Calculate the rate of [NO3] production at 0.84 M [NO2land 1.4 M [03]. Final answer must be rounded off to 2 decimal places, and shall NOT have any units.
The following data were collected for the reaction between hydrogen and nitric oxide at 700°C. 2 H2(g) + 2 NO(g) - 2 H20(g) + N2(g) Experiment [H2]/M [NO]/M Initial rate/M-s-1 0.012 0.031 4.5x10-6 0.0060 0.031 2.2x10-6 3 0.012 0.0155 1.1x10-6 (a) What is the rate law for the reaction? (Rate expressions take the general form: rate = k. [A]ª . [B]b.) chemPad Help Greek - (b) Calculate the rate constant for the reaction. 4.0 (c) Suggest a plausible reaction mechanism that is consistent with the rate law. (Hint: Assume that the oxygen atom is the intermediate. Omit states-of-matter from your answer.) First step: chemPad Help Greek - Second step: chemPad Help Greek
The following data was collected for the reaction: A + B + C = Products Experiment Initial concentration (mM) Initial Rate (mM.s-1) A B C 1 1.25 1.25 1.25 8.7 2 2.5 1.25 1.25 17.4 3 1.25 3.02 1.25 50.8 4 1.25 3.02 3.75 457 5 3.01 1.00 1.15 ? Write the rate law for the reaction What is the order for the reaction? Use the data to predict the reaction rate for experiment 5
Consider the following general reaction for which gases A and B are mixed in a constant volume container: A(g) + B(g) -> C(g) + D(g) Match what happens to the rate of the reaction under the following changes: (consider each change separately) v all of gas B is removed from the container more gas A is added to the container the temperature of the container is increased there is no change to the reaction rate ya catalyst is added to the container I. the reaction proceeds at a faster rate v gas D is also added to the container the reaction proceeds at a slower rate II. some of gas B is removed from the container Iy the reaction does not proceed at all the volume of the container is increased
Find concentration of each of the ions in: b. a 0.96M solution of H2SO4
What is the rate constant of the reaction?
Consider the reaction: NO2 + 03 → NO3 + 02 [NO,], M [03], M Rate, M/s 6.30 x 10-3 Experiment 1 0.21 0.70 1.89 x 10-2 3.15 x 10-3 0.63 0.65 3 0.21 0.35 4 0.42 0.35 6.30 x 10-3 Calculate the rate of [NO3] production at 0.84 M [NO2]and 1.4 M [03]. Final answer must be rounded off to 2 decimal places, and shall NOT have any units.
The following data were obtained at constant temperature for the reaction: 4A(g) + 4B (g) → 3C(g) Initial [A] Initial [B] mol Experiment mol mol Initial Rate L-min L L 1 0.105 0.215 4.50 2 0.315 0.215 13.5 3 0.105 0.430 18.0 4 0.315 0.430 54.0 Part 1 of 2 Select the single best expression for the rate law for the reaction. Ok [A]³ [B]³ G Ok [A] [B] Ok [A] [B] Ok [A][B]²
Find the rate constant (M-1 s-1) for the reaction
Consider the reaction between nitric oxide and hydrogen 2NO + H2 → N20 + H20 Initial Rate of Disappearance of NO Experiment Initial [NO], M Initial [H2], M (mol/L sec) 1 6.4 x 10-3 2.2 x 10-3 2.0 x 10-5 2 12.8 x 10-3 2.2 x 10-3 8.0 x 10-5 6.4 x 10-3 4.4 x 10-3 4.0 x 10-5 What is the rate law for this reaction? a. Rate = k[NO] b. Rate = k[NO]? c. Rate = k[NO]²[H2] d. Rate = k[No][H2]
Need the following questions answered The reaction of interest: O2 (g) + 2 NO (g) → 2 NO2 (g) Expt. [O2] (M) [NO] (M) Initial Rate (M/s) 1 0.0110 0.0130 0.00321 2 0.0220 0.0130 0.00640 3 0.0110 0.0260 0.01280 4 0.0330 0.0130 0.00960 5 0.0110 0.0390 0.02880 What is the reaction order for oxygen? What is the reaction order for nitrogen monooxide? What is the overall reaction order? What is the rate law for this reaction? What is the specific rate constant (k) for this reaction? Write the rate law for this reaction that includes the numerical value of the specific rate constant: