Consider the following reaction:   X + Y + Z ? Products   Reaction # [X] [Y] [Z] Initial Rate (mol/L s) 1 0.800 0.600 1.120 1.428 x 10-3 2 0.200 1.000 0.400   0.91 x 10-5 3 0.200 0.400 0.400   0.91 x 10-5 4 0.800 0.600 1.500   1.28 x 10-3 5 0.200 0.600 1.1200   7.14 x 10-4 a)Determine the rate law b)What is the order of the reaction ? c)Solve for the rate constant.

Final Reactant Concentrations and Reaction Rates   [I-] [BrO3-] [H+] Reaction Time Rate of Reaction 2.8 x 10-5/time Expt. # M M M sec. M/sec 1 0.00166 0.0066 0.0166 258   2 0.0033 0.0666 0.0166 135   3 0.00166 0.0133 0.0166 132   4 0.00166 0.0066 0.033 78   FIND THE RATE?

Final Reactant Concentrations and Reaction Rates   [I-] [BrO3-] [H+] Reaction Time Rate of Reaction 2.8 x 10-5/time Expt. # M M M sec. M/sec 1 0.00166 0.0066 0.0166 258 3.876 x 10^-6 2 0.0033 0.0666 0.0166 135 7.40 x 10^-6 3 0.00166 0.0133 0.0166 132 7.576 x 10^-6 4 0.00166 0.0066 0.033 78 1.282 x 10^-5   Using the general rate law equation below and your orders determined, calculate the rate constant for each experiment and then the average. Rate= k[I-]m[BrO3-]n[H+]p     k______________       k________________ k________________              k ____________   Average value of k __________________ Units of k__________________   Rewrite the final rate law including values for m, n, p and the average value of k and units:   _________________________________

The following initial rate data was collected for the reaction: Experi ment 1 2 HI (g) + C₂H5l (g) --> C₂H6 (g) + 1₂ (g) 3 [HI] 0.015 M 0.030 M 0.030 M [C₂H51] 0.900 M 0.900 M 0.450 M Initial Rate 4.01 x 10 5 M/S 8.04 x 10 5 M/s 3.99 x 10 5 M/S