Given the following data, estimate the rate constant of A(g) + B(g) → AB(g) (do not write the units in your answer) Experiment [A] (M) [B] (M) Rate (M/s) 1 0.400 0.200 0.8 0.200 0.200 0.200 0.200 0.100 0.05

Given the following data, estimate the rate constant of A(g) + B(g) → AB(g) (do not write the units in your answer) Experiment [A] (M) [B] (M) Rate (M/s) 1 0.400 0.200 0.8 0.200 0.200 0.200 0.200 0.100 0.05

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

Using the following rate law and the experimental values given in the question figures, calculate k: Rate = k[F2][ClO2] [F2] (M) [ClO2] (M) Initial Rate (M/s) Experiment 1 0.5 0.5 0.300 Experiment 2 0.8 0.8 0.768 Experiment 3 0.5 0.8 0.480
The synthesis of ammonia obeys the following reaction: N2(g) + 3H2(g) → 2 NH3(g) N2(g) concentration measurements were taken at different times and plotted. 1) What is the average reaction rate of NH3(g) between 0 and 3 hours? (Attention, the graph is in "hour" and we want a speed in "mole/L s") 2) What is the instantaneous rate of reaction of NH3(g) at the 1st hour? 3) What is the general speed between 0 and 3 hours?
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
Using the data in the table, determine the rate constant of the reaction and select the appropriate units. k= A + 2BC+D 1.6 Incorrect Trial [A] (M) [B] (M) Rate (M/s) 1 0.350 0.320 2 0.350 0.640 3 0.700 0.320 Units Incorrect 0.0102 0.0102 0.0408 M-2S-1
Given the following rate law of a fictional reaction: [A] Rate = k- [B* (C] By what factor does the rate change if each of the following changes occur? (a) B is doubled [ Select ] (b) A is halved [ Select] (c) A is halved and C is doubled [Select] [ Select > >
Using the data in the table, calculate the rate constant of Trial [A] (M) [B] (M) Rate (M/s) this reaction. 1. 0.400 0.210 0.0120 A +B C+D 2 0.400 0.525 0.0750 3 0.480 0.210 0.0144 Units k =
Using the data in the table, determine the rate constant of the Trial [A] (M) | [B] (M) Rate (M/s) reaction and select the appropriate units. 1 0.220 0.260 0.0189 2 0.220 0.520 0.0189 А + 2B → C+ D 3 0.440 0.260 0.0756 Units 0.0484 k M-'s-1 Incorrect
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
The data shows that the rate depends on the concentration of the reactants. How else can a chemist increase the rate of reaction?
What is the rate constant without units?
Use this data to determine the value of the rate constant. Ex # [A] (M) [B] (M) Rate (M/hr) 1 .240 .120 2.00 2 .120 .120 .500 3 .240 .0600 1.00 Question 4 options: 289 per hour 579 per hour 8.3 per hour 0.0144 per hour 69.4 per hour .00346 per hour 0.060 per hour 0.0173 per hour 17 per hour 0.12 per hour
Ln [A] Post Lab Assignment 1. Nitrosyl chloride, NOCI, decomposes to NO and Cl2. 2NOCI(g) → 2NO(g) + Cl, (g) Determine the rate law, the rate constant, and the overall order for this reaction from the following data: [NOCI] (M) Rate (mol L-1 h-1) 0.10 0.20 0.30 3.2 x 10-9 7.2 x 10-9 2. A 5.0 mL dye solution of 3.45 e-5 M is mixed with 15.0 mL bleach solution of 0.21 M. What are the initial concentrations of [Dye] and [Bleach] for your experiment? 3. The plots of 1/[A] vs time, In([A]) vs. time, and [A] vs. time of a solution of substance A are shown below. What is the reaction order with respect to A? 000 009 007 000 0 20 40 Time (min) Time 09 08 Time