Which of these reactions are you going to measure the rate of in this experiment?Question 1Answer2I–(aq) + H2O2(aq) + 2H+(aq) → I2(aq) + 2H2O(l)I2(aq) + 2S2O32–(aq) → 2I–(aq) + S4O62–(aq)

H2O2(aq) + 2I-(aq) + 2H3O+(aq) → I2(aq) + 4H2O(l) (Reaction 1) I2(aq) + 2S2O32-(aq) → S4O62-(aq) + 2I-(aq) (Reaction 2) I2(aq) + I-(aq) + Starch(aq) → (I3- -Starch)complex (aq) (Reaction 3) Now consider the moment when the blue colour change is about to occur (i.e. when there is no more thiosulfate remaining in solution).Based on the initial experiment and initial concentrations of reagents, calculate the concentrations of the reagents present in the flask at the moment just before the blue colour change begins (ignore the starch, and the S4O62- which is formed as the other by-product in this reaction).Does Reaction (1) continue beyond this point? Multiple choice 2 Question 10a. yesb. no Based on what you have calculated, which reagent in Reaction (1) is the limiting reagent?Multiple choice 3 Question 10a. H+b. H2O2c. I-d. S2O32-

A student performed an initial rate study to determine the rate law for the reaction:S 2 O 82- (aq) + 3I -(aq) ® 2 SO 42- (aq) + I 3-(aq)The results of the study are given in the table below:Experiment [S 2 O 82- (aq)] o(mol L-1 )[I- (aq)] o(mol L-1 )Initial rate(mol L-1 s -1 )1 0.200 0.100 8.35 x 10-32 0.100 0.050 1.05 x 10-33 0.200 0.050 4.25 x 10-34 0.300 0.150 ?i. (1 mark)Determine the order with respect to S 2 O 82-. Justify your answer.ii. (1 mark)Determine the order with respect to I- . Justify your answer.iii. (1 mark)Write the rate law for the overall reaction.iv. (1 mark)What is the overall order of the reaction?v. (1 mark)Calculate the value for the rate constant k of the reaction from the data given forexperiment 1.vi. (2 marks)Given your value for k and your determined rate law, calculate the initial rate forreaction number 4.k1k-1k3vk2v

Consider the results from Experiments 1, 2 and 3 in Question 9. Compare the rate (1/ Dt) for Experiment 1 with the rates in Experiments 2 and 3 where the concentration of [I-] and [S2O82-] are halved. Is the following statement true or false?Rate is proportional to [I-aq]2

Which of the following will complete the double replacement reaction below?Mg(OH)2(s) + 2HNO3(aq) →

If the reaction studied in this experiment was first order with respect to the concentration of H2O2, what would happen to the rate of the reaction if the concentration of H2O2 was doubled?Question 3Select one:The rate would not change. The rate would be doubled. The rate would be tripled.The rate would increase by a factor of 4.The rate would increase by a factor of 8.