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The iodine ion reacts with hypochlorite ion (the activeingredient in chlorine bleaches) in the following way: OCl- + I- ----> OI- +Cl-. This rapid reaction gives the following ratedata:[OCl-],M I-,M Rate, L/s1.6 x10-3 1.6x10-3 1.75 x 1047.6 x10-3 1.6x10-3 2.72 x 1041.6 x10-3 9.6x10-3 2.72 x 105
A) write the rate law for this reaction
B) What is the overall order of the reaction
C) What is the numerical value of the rate constant and what are the units?
D) Calculate the rate of this reaction when the initial concentrations of OCl- and I- are 7.6 x10-3 M and 9.6 x 10-3M respectively.
For the reaction, A = B + C, the rate law is k[A]. If it takes 80.0 seconds for 70.0% of a 10.0 gram sample of A to be transformed into products, what is the value of the rate constant.
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