\begin{tabular}{|l|l|l|l|l|l|l|l|} \hline mixture & water & HIO3 & H2SO3 & Time(s)expl & 1/time(s-1)exped & Time(s)calc. & Time(s-1)calc. \\ \hline a & 3.00ml & 5.00ml & 2.00ml & 103.59 & & \\ \hline b & 2.00ml & 5.00ml & 3.00ml & 33.83 & & \\ \hline c & 1.00ml & 5.00ml & 4.00ml & 22.59 & & \\ \hline d & 0 & 5.00ml & 5.00ml & Trial117.12rrial217.31 & Trial 1 & & \\ \hline e & 3.00ml & 2.00ml & 5.00ml & 35.03 & & \\ \hline f & 2.00ml & 3.00ml & 5.00ml & 20.53 & & \\ \hline g & 1.00ml & 4.00ml & 5.00ml & 26.31 & & \\ \hline \end{tabular} 1. Use the experimental times to calculate the value of 1/ time and fill in the appropriate column in the table. 2. Average the two best times required for mixture d and calculate the value of the rate constant, k. (See handout "Simplified Rate Law Calculations"). Show your work. 3. Using the rate constant calculated in number 2 and the law of mass action (see handout "Simplified Rate Law Calculations") calculate time in seconds for each of the mixtures, a through g. Show the calculation for mixture d and for one other mixture in the space below. You and your lab partner must use different mixtures for the second sample caiculation. 4. On a separate sheet of paper, complete the calculations outlined in the procedure for the determination of the order of the reaction with respect to the non-first order component. Do this only for the non-first order reactant, not for both reactants. Problem Use the value of the rate constant calculated in number 2 above and the law of mass action, calculate the reaction time for a mixture of 22.50mL water, 15.50mL sulfurous acid, and 19.00 mL. iodic acid. Show your work