experiment 1 time 92 s, experiment 2 68 s, experiment 3 106 s

temp is 294 K

Experiment 16. A Kinetic Study of an Iodine Clock Reaction (rev 1/14 Page 8 Name Partner Date Performed DATA & CALCULATIONS: A. Dependence of Reaction Rate on Concentration. Temperature Experiment1 Experiment 2 Experiment 3 [1'), initial (mol/L) [S208?), initial (mol/L) At = elapsed time (s) Reaction Rate (mol L-IS-) Determining the order of the Reaction. (round to nearest half-integer or whole-integer) m = Order of reaction with respect to l' = n = Order of reaction with respect to S,O 2- = Overall order of the reaction Calculating rate constant k (you will need to use the values of m and n above in Rate Law) Experiment1 Experiment 2 Experiment 3 Rate Constantak Average Rate Constant at Room Temp B. Dependence of Reaction Rate on Temperature [l], initial - (S202), initial Experiment 5 Experiment 6 Experiment 4 T - Temperature (K) At=time elapsed (s) Rate (mol L -1) k=Rate Constant 1/T (K) Ink Experiment 16. A Kinetic Study of an Iodine Clock Reaction (rev 1/14) Page 9 Graphical Analysis of Temperature Dependence Data. Attach a graph of Ink vs 1/T. Calculate the slope of your straight line Determine the Activation Energy E, (kJ/mol) = Sample Calculations (For each line of data in the report that was calculated, not recorded directly, be sure to put in a sample calculation that sets up one of the calculations on that row.) Experiment 16. A Kinetic Study of an Iodine Clock Reaction (rev 1/14 Page 8 Name Partner Date Performed DATA & CALCULATIONS: A. Dependence of Reaction Rate on Concentration. Temperature Experiment1 Experiment 2 Experiment 3 [1'), initial (mol/L) [S208?), initial (mol/L) At = elapsed time (s) Reaction Rate (mol L-IS-) Determining the order of the Reaction. (round to nearest half-integer or whole-integer) m = Order of reaction with respect to l' = n = Order of reaction with respect to S,O 2- = Overall order of the reaction Calculating rate constant k (you will need to use the values of m and n above in Rate Law) Experiment1 Experiment 2 Experiment 3 Rate Constantak Average Rate Constant at Room Temp B. Dependence of Reaction Rate on Temperature [l], initial - (S202), initial Experiment 5 Experiment 6 Experiment 4 T - Temperature (K) At=time elapsed (s) Rate (mol L -1) k=Rate Constant 1/T (K) Ink Experiment 16. A Kinetic Study of an Iodine Clock Reaction (rev 1/14) Page 9 Graphical Analysis of Temperature Dependence Data. Attach a graph of Ink vs 1/T. Calculate the slope of your straight line Determine the Activation Energy E, (kJ/mol) = Sample Calculations (For each line of data in the report that was calculated, not recorded directly, be sure to put in a sample calculation that sets up one of the calculations on that row.)