Find the following answers to questions 1-3 from the information in the picture provided please. 1. Initial concentration of iodine in reaction (mM)2. Initial concentration of hydrogen peroxide in reaction (mM)3. Initial rate (mM/s) CS IODINE CLOCK REACTION|Lab DataConcentrationConcentration of iodide solution (mm)Concentration of thiosulfate solution (mm)Concentration of hydrogen peroxide solution (mm)Temperature of iodide solution (°C)Volume of iodide solution (1) used (mL)Volume of thiosulfate solution (S203²-) used (ml)Volume of DI water used (mL)Volume of hydrogen peroxide solution (H₂O₂) used (mL)Time (s)ObservationsInitial concentration of iodide in reaction (mm)Initial concentration of thiosulfate in reaction (mm)Initial concentration of hydrogen peroxide in reaction (mm)Initial Rate (mm/s)TemperatureTrial 173.931.5145.525.010.01.02.57.528.9Liquid turned darkblue at 28.9seconds1.57.0Trial 273.931.5145.5Trial 373.931.5145.5- XU

The objective of the question is to calculateThe initial concentration of .The initial concentration of .The initial rate of the reaction.The chemical reaction involves iodide (), hydrogen ions (), hydrogen peroxide (), thiosulfate () and produces iodine (), water (), and tetrathionate ().The appearance of a deep blue color upon the addition of starch indicates the presence of .Calculate the total volume in reaction:The total volume in the reaction is the sum of the volumes of the iodide solution, thiosulfate solution, water, and hydrogen peroxide solution:Calculate the initial concentration of :Calculate the initial concentration of :Calculate the initial concentration of :Calculating the final concentration:The final concentration of hydrogen peroxide () is , indicating that it has been fully consumed in the reaction.Calculating the initial rate:This indicates the rate of consumption of hydrogen peroxide at the beginning of the reaction.From the above answer, it is evident that-