Trial [H2O2] M [1'] M [H'] M Rate (M/s) -6 0.00050 0.00050 0.00050 1.15 x 10*6 2.30 x 106 2.30 x 106 1.15 x 106 0.010 0.020 0.010 0.010 0.010 0.010 0.020 0.010 0.00100 Write the rate law for the reaction. O a. Rate = k[H2O2]²[I¯ ][H¯ ] O b. Rate = k[H2O2][I* ] O c. Rate = k[H2O2][I* ][H¯ ] O d. Rate = k[H¿O2]²[I* ] O e. Rate = k[H202][I* ]?[H¯ ] 1234
Trial [H2O2] M [1'] M [H'] M Rate (M/s) -6 0.00050 0.00050 0.00050 1.15 x 10*6 2.30 x 106 2.30 x 106 1.15 x 106 0.010 0.020 0.010 0.010 0.010 0.010 0.020 0.010 0.00100 Write the rate law for the reaction. O a. Rate = k[H2O2]²[I¯ ][H¯ ] O b. Rate = k[H2O2][I* ] O c. Rate = k[H2O2][I* ][H¯ ] O d. Rate = k[H¿O2]²[I* ] O e. Rate = k[H202][I* ]?[H¯ ] 1234
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 13.75QE
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