Consider the hypothetical reaction A+B+ 2C 2D + 3E where the rate law is A[A] At Rate == = k[A][B]² An experiment is carried out where [A]o = 1.0 × 10-2² M, = [Blo 3.0 M, and [C]o 2.0 M. The reaction is started, and after 6.0 seconds, = the concentration of A is 3.8 × 10-³ M. a. Calculate the value of k for this reaction. L² mol 2S-1 k= b. Calculate the half-life for this experiment. Half-life = S c. Calculate the concentration of A after 19.0 seconds. Concentration = d. Calculate the concentration of C after 19 seconds. Concentration = M M
Consider the hypothetical reaction A+B+ 2C 2D + 3E where the rate law is A[A] At Rate == = k[A][B]² An experiment is carried out where [A]o = 1.0 × 10-2² M, = [Blo 3.0 M, and [C]o 2.0 M. The reaction is started, and after 6.0 seconds, = the concentration of A is 3.8 × 10-³ M. a. Calculate the value of k for this reaction. L² mol 2S-1 k= b. Calculate the half-life for this experiment. Half-life = S c. Calculate the concentration of A after 19.0 seconds. Concentration = d. Calculate the concentration of C after 19 seconds. Concentration = M M
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter13: Chemical Kinetics
Section: Chapter Questions
Problem 13.23QE: Nitrogen monoxide reacts with chlorine to form nitrosyl chloride. NO(g)+12Cl2(g)NOCl(g) The figure...
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