2. Consider the chemical kinetics data set given below for the following reaction at 300K: 1 N20 → N + 2⁰₂ Create two different plots of this data to determine if the reaction follows first or second order kinetics and determine the rate constant. (mol t (seconds) [N₂0] 0.0 5.0 10.0 15.0 20.0 0.1020 0.0165 0.0089 0.0062 0.0048

2. Consider the chemical kinetics data set given below for the following reaction at 300K: 1 N20 → N + 2⁰₂ Create two different plots of this data to determine if the reaction follows first or second order kinetics and determine the rate constant. (mol t (seconds) [N₂0] 0.0 5.0 10.0 15.0 20.0 0.1020 0.0165 0.0089 0.0062 0.0048

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

please add three grapgs, one graph of the order and anotheer two graphs that prove the order
Initial rate data at a certain temperature is given in the table for the following reaction. [NOCI], (M) Initial rate of formation of Cl, (M/s) 2 NOCI(g) → 2 NO(g) + Cl, (g) 0.600 1.30 x 10-5 0.750 2.03 x 10-5 0.900 2.92 x 10-5 Determine the value and units of the rate constant, k. Units: k :
The reaction A → C was performed and the concentration vs. time data below collected. time, s 0 1 2 3 4 5 6 7 8 [A], mol/L 0.9541 0.5884 0.3629 0.2238 0.1380 0.08512 0.05250 0.03238 0.01997 Complete the rate law for the reaction by filling in the values for the rate constant and reaction order. Rate = k[A]x rate constant (without units) =
The National Institute of Science and Technology (NIST) kinetics database lists the rate constant, ? k , of a particular gaseous reaction at 9.89 x 10^-10 cm^3 M-1 S-1 298 k. Convert the rate constant to units of M-1* S-1 M −1 ⋅s −1
A certain reaction is second order in N, and first order in H,. Use this information to complete the table below. Round each of your answers to 3 significant digits. [N] H,] initial rate of reaction x10 0.929 M 1.05 M 95.0 M/s olo 0.436 M 1.05 M |M/s Ar 0.165 M 5.93 М ||M/s
A certain reaction is second order in N, and first order in H,. Use this information to complete the table below. Round each of your answers to 3 significant digits. initial rate of reaction x10 0.537 M 0.350 M 21.0 M/s 0.169 M 0.350 M || M/s 0.261 M 0.721 M M/s
The rate law for the reaction: NH4+ + NO₂ N₂ + 2H₂O is rate =k[NH4+][NO₂] It is found that the rate constant for this reaction is 3.05x10-4 M-1s-1. Calculate the rate of the reaction, including units, if [NH4*] is 0.265M and [NO₂] is 0.0803M. Attach File Browse Local Files
A particular reactant decomposes with a half‑life of 117 s117 s when its initial concentration is 0.376 M.0.376 M. The same reactant decomposes with a half‑life of 221 s221 s when its initial concentration is 0.199 M.0.199 M. Determine the reaction order. 2 1 0 What is the value and units of the rate constant for this reaction? ?=k= Units
The decomposition of hydrogen peroxide was studied at a particular temperature. The following data were obtained, where Time (s) [H,O,] (mol/L) 1.00 120 0.91 300 0.78 600 0.59 1200 0.37 1800 0.22 2400 0.13 3000 0.082 3600 0.050 Determine the reaction order and the value of the rate constant.