SHOW ALL WORK ONA SEPARATE SHEET. PUT A BOX AROUND EACH ANSWER. UPLOAD YOUR FILE TO THIS QUESTION. The following initial rate data apply to the reaction below. A + 2B – C+ 2D Exp # [A] (M) [B] (M) Initial Rate (M/s) 1 0.24 0.020 3.3 x 103 2 0.72 0.020 9.9 x 10 3 0.24 0.040 3.3 x 10 3 1. Write the rate expression in terms of disappearance of reactants and appearance of products. 2. If the rate of disappearance of B = 0.16 M/min at a particular moment, what is the rate of

SHOW ALL WORK ONA SEPARATE SHEET. PUT A BOX AROUND EACH ANSWER. UPLOAD YOUR FILE TO THIS QUESTION. The following initial rate data apply to the reaction below. A + 2B – C+ 2D Exp # [A] (M) [B] (M) Initial Rate (M/s) 1 0.24 0.020 3.3 x 103 2 0.72 0.020 9.9 x 10 3 0.24 0.040 3.3 x 10 3 1. Write the rate expression in terms of disappearance of reactants and appearance of products. 2. If the rate of disappearance of B = 0.16 M/min at a particular moment, what is the rate of

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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6. Given the reaction: CH3(CO)CH3 (M) | B(M) 0.010 0.010 CH3(CO)CH3 + I2 + H* → CH3(CO)CH2I + HI H* (M) Rate (M/s) 0.010 3.0 x 10-4 0.010 6.0 x 10-4 0.020 6.0 x 104 0.020 2.4 x 10-3 0.040 4.8 x 10-3 0.010 6.0 x 104 0.010 0.020 0.010 0.040 0.040 0.020 0.020 0.040 0.020 0.040 a. Determine the reaction order for each reactant. b. Solve for the rate constant, k, and the appropriate units. c. Write the rate law for the reaction, including a value for k. d. Solve for the rate of the reaction if there are 1.25 M of CH3(CO)CH3, 2.25 M of I2, and 3.25 M H*.
Using the data in the table, calculate the rate constant of this reaction. k= A + B C + D Trial [A] (M) 1 2 3 Units 0.380 0.380 0.608 [B] (M) 0.300 0.690 0.300 Rate (M/s) 0.0116 0.0614 0.0186
Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A + 2B-C+D k= esc @ NO 2 # 3 с Ad 4 % Trial [A] (M) [B] (M) Rate (M/s) 1 0.250 0.200 2 0.250 0.400 3 0.500 0.200 5 Units G Search or type URL MacBook Pro A 6 & 7 0.0168 0.0168 0.0672
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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+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? 3.
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Smail ||| YouTube O KINETICS AND EQUILIBRIUM Using an integrated rate law for a first-order reaction At a certain temperature the rate of this reaction is first order in NH4OH with a rate constant of 0.0108 s NH,OH(aq). } → NH, (aq) +H,O(aq) Translate M Suppose a vessel contains NH4OH at a concentration of 1.24 M. Calculate the concentration of NH OH in the vessel 63.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. Explanation 82°F Mostly cloudy Check 0/5 Q Search © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | 1
The balanced equation for a given reaction is 4 X + 3 Y → P. The following data regarding initial reaction rates were collected in the lab. What is the rate law for the reaction? Trial [X] (M) [Y] (M) Rate (M/s) 1 0.020 0.060 3.40 x 10–3 2 0.020 0.120 2.72 x 10–2 3 0.080 0.060 1.36 x 10–2
Using the data in the table, calculate the rate constant of this reaction. k= A+B → C + D Trial [A] (M) [B] (M) 1 0.290 0.380 2 0.290 1.03 3 0.464 0.380 Units Rate (M/s) 0.0163 0.119 0.0261
Please show your work (THIS IS NOT A GRADED ASSIGNMENT)
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.