Determine the rate law for the generic reaction, A + B → products, using the initial rates data provided in this table:PA (bar)Order for B:0.100.100.150.25(a) Report the order of the reaction for each component:Order for A:PB (bar)0.100.150.200.40rate (bar/sec)0.01800.02700.05400.1800 Continued from the previous problem(b) Report the value of the rate constant (pressure in bar, time in sec).

Answered: Image /qna-images/answer/1c06cf33-d16a-46b3-a716-e2f711cb2b71.jpg

Determine the rate law for the generic reaction, A + B → products, using the initial rates data provided in this table: PA (bar) Order for A: 0.10 Order for B: 0.10 0.15 (a) Report the order of the reaction for each component: 0.25 PB (bar) 0.10 0.15 0.20 0.40 rate (bar/sec) 0.0180 0.0270 0.0540 0.1800

Determine the rate law for the generic reaction, A + B → products, using the initial rates data provided in this table: PA (bar) Order for A: 0.10 Order for B: 0.10 0.15 (a) Report the order of the reaction for each component: 0.25 PB (bar) 0.10 0.15 0.20 0.40 rate (bar/sec) 0.0180 0.0270 0.0540 0.1800

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

At elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen: 2N205(8)→ 4NO2 (g) + O2(g) When the rate of formation of O2 is 3.6 x 10-3 M/s, the rate of decomposition of N2O5 is. M/s. A) 0.00090 OB) 1.4 x 10-2 1.8 × 10-3 OD) 3.6 × 10-3 E) 4.4 x 10-4
١
Given the following hypothetical chemical reaction and initial rate experiment data determine the order for all reactants. Next write the rate law. Finally determine the rate constant (k)
6)Write the overall rate law for the following reaction: include the units for the rate constant A + B > C Exp [A] [B] rate 1 0.273 0.763 2.83 M/s 0.273 1.526 2.83 M/s 3. 0.819 0.763 25.47 M/s
Given the following data, determine the rate constant, k (do not use units), of the reaction: A(g) + 2 B(g) → C(g) + 2 D(g) Experiment [A] (torr) [B] (torr) Rate (torr/s) 1 500 300 2.68 2 500 100 0.298 3 250 300 0.67
Given the initial rate data for the reaction below, determine the rate law for this reaction. 4A + 7B ⟶ 4C + 6D [A], M [B], M Δ[C]/Δt (initial), M/s 0.050 0.050 1.04 0.150 0.050 3.12 0.050 0.250 26.0 a ) None of the other answer options are correct. b) rate = 8320 M-2 s-1 [A]2 [B]1 c) rate = 6.66 x 107 M-5 s-1 [A]5 [B]1 d) rate = 2.13 x 1014 M-10 s-1 [A]4 [B]7 e) rate = 8320 M-2 s-1 [A]1 [B]2 Please explain your reasoning and show your work.
A scientist evaluated reaction rates for the reaction A + B --> C using differing initial concentrations of A and B and collected the following data: [A] [B] Rate 0.492 0.430 2.339 0.492 0.860 4.678 0.984 0.430 9.356 0.984 0.860 18.712 a) What is the rate order for reactant B in the rate law for this reaction?
The following reaction shows the decomposition of H2O2. 1 H,02 (aq) → H20 (1) +02 (9) Write down an expression for the rate of the reaction in terms of the reactant H2O2. The initial concentration of H202 is 0.2546 M and the initial rate of the reaction is 9.32 x 104 M/s. find the concentration of H202 after 35.0 s.
Consider the following reaction: 1. 2 N,O5 (g) → 4 NO, (g) + O, (g) The initial concentration of N2O5 was 0.48 mol/L, and 25 minutes after initiating the reaction, all of the N,Os has been consumed. (a) Calculate the average rate of the reaction over this 25-minute time interval. (b) Is it correct to assume that the rate law is Rate = k[N,O5]² based on the balanced chemical equation? Briefly explain your answer.
4. Although the depletion of stratospheric ozone threatens life on Earth today, its accumulation was one of the crucial processes that allowed life to develop in prehistoric times: ( WRITE YOUR ANSWERS IN YOUR SOLUTIONS PAGE) 302(g) → 203 (g) (a) Express the reaction rate in terms of [02] and [03]. (b) At a given instant, the reaction rate in terms of [02] is 2.17.10-5 mol/L-s. What is it in terms of [03]?
Given the experimental information in the following table below: Why are the rates calculated not equal? A → products Time (minutes) [A] (M) 0.00 0.1563 1.00 0.1469 2.00 0.1431
Suppose you are studying the kinetics of the reaction between nitrogen monoxide and hydrogen gas. You perform the reaction multiple times with different starting concentrations and measure the initial rate for each, resulting in this table. Experiment [NO] (M) [H2] (M) Initial Rate (M/s) 1 0.0050 0.0020 1.25 x 10–5 2 0.010 0.0020 5.00 x 10–5 3 0.0050 0.0040 2.50 x 10–5 Based on the data, choose the correct exponents to complete the rate law. rate=k[NO]x[H2]y x=? y=?