A substance A is consumed by a reaction of unknown order. The initial concentration is 2 mM, and concentrations at later times are as shown: Time (min) [A] (mM) 1 1.66 2 1.44 4 1.12 8 0.76 16 0.48 Test whether or not a first-order reaction fits the data.

A substance A is consumed by a reaction of unknown order. The initial concentration is 2 mM, and concentrations at later times are as shown: Time (min) [A] (mM) 1 1.66 2 1.44 4 1.12 8 0.76 16 0.48 Test whether or not a first-order reaction fits the data.

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

A plot of In[A] versus time (in seconds) for a First Order Reaction has the following trendline equation: y = -0.006283x -0.639 Calculate the concentration of the reactant at time=72 seconds. (Report your answer to 3 SF. Include units of M in your answer) Answer:
show detailed work
What is the rate constant for the reaction?
Please help explain this question... Not sure if I am doing this right. I am stuck
19. The initial rate of reaction between Substance A and Substance B was measured at a series of concentrations of each reactant with the following results. Solve for the rate law expression of this reaction. Note: Include all rough notes, show all calculations, follow the rules of significant figures, and box your final answer. ( A + B → AB Trial Number Trial #1 Trial #2 Trial #3 [A] 0.10 M 0.30 M 0.30 M [B] 0.10 M 0.10 M 0.20 M Initial rate 5.0 X 104 1.5 X 103 6.0 X 103 (mol/L·s)
Calculate the rate law from the given data: Run [B] [C] Initial Rate (M/sec) 1 1.5 2.0 0.20 2 1.5 4.0 0.40 3 3.0 2.0 0.80
Based on the data below. Graphically determine the rate law for the reaction, and extract the rate constant and initial concentrations. 2 A -----> B Time [A] 5 11.4730407 10 7.6906092 15 5.15516951 20 3.45561346 25 2.31636698 30 1.55270722 35 1.04081077
For the given data, what is the correct unit for the rate constant, k? Run [B] [C] Initial Rate (M/sec) 1 1.5 2.0 0.20 2 1.5 4.0 0.40 3 3.0 2.0 0.80
For the reaction below, a series of experiments was conducted and the data collected in the table below. a. Determine the rate law and the overall order of the reaction. b. Calculate the rate constant, including appropriate units. c. Determine the initial rate when the initial concentrations of both reactants are 0.12 M. Reaction (might be unbalanced): NO (g) + Cl2 (g) → NOCI (g) Experiment Data: Experiment # Initial [NO] (M) Initial [Cl2] (M) Initial Rate (M/s) 0.13 1.0x10-2 0.20 2 0.26 0.20 4.0x10-2 3 5.0x10-3 0.13 0.10
A certain reaction is second order in N₂ and first order in H₂. Use this information to complete the table below. Be sure each of your answer entries has the correct number of significant digits. 1.58 M 0.540 M 3.89 M 0.382 M 0.382 M 0.155 M Explanation initial rate of reaction Check 0.440 M/s Mis MIS X S tv W MacBook Air © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center C 5 Accessibility
The reaction A→ Products is a first-order reaction with a rate constant of 1.91 x 10-3 min-1. The reaction started with an initial concentration of A equal to 0.0881 M, what is the concentration of A after 131.1 minutes? Do not write unit in answer. Report your answer with four places past the decimal point. Type your answer... Submit