A reaction of the form aA → Products is second order with a rate constant of 0.169 L/(mol ·s). If the initial concentration of A is 0.300 mol/L, how many seconds would it take for the concentration of A to decrease to 6.07 x 10-3 mol/L? Time S %3D
A reaction of the form aA → Products is second order with a rate constant of 0.169 L/(mol ·s). If the initial concentration of A is 0.300 mol/L, how many seconds would it take for the concentration of A to decrease to 6.07 x 10-3 mol/L? Time S %3D
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 5ALQ: Consider the following statements: In general, the rate of a chemical reaction increases a bit at...
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Step 1
Given,
Rate Constant (k) = 0.169 L/(mol .s)
Initial concentration [A]o = 0.300 mol/L
After time 't', [A]= 6.07 ×10-3 mol/L
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