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Hello I am really struggling with how to understand how to do this lab. Please help. Consider Experiment #3 to be performed in Part B. The initial concentrations of the reactants S2O82− and I− in the reaction solution must be calculated as the solutions in the burets containing the reactants are diluted during the preparation of the reaction solution. Calculate [I−]initial, [S2O82−]initial in the reaction solution for Experiment #3. (see Table 3 and the sample dilution calculations). (2 pts) Consider each experiment to be performed in Part B. The added S2O32− determines when the expected color change will occur to indicate when to stop timing the reaction. The number of moles of S2O82− that have reacted in the measured time is required to calculate the rate of the reaction. a. Calculate [S2O32−]initial in the reaction mixture. Remember that the [S2O32−] of the solution in the buret is diluted when the reaction solution is prepared (see Table 3 and Equation 15 as an example). (1 pt) b. Calculate Δ[S2O82−]reacted using Equation 13 (see Equation 16 as an example). (1 pt) Consider the reaction of A and B2 shown in Equation 18. Solutions of A and B2 were mixed in various quantities. The data in Table 3 were obtained at a constant reaction temperature. 2 A (aq) + 3 B2 (aq) → 2 AB3 (aq) (Eq. 18) Table 4. Reaction Rate Data for Reaction of A and B2 at Constant Temperature Experiment Initial [A], (M) Initial [B2], (M) Reaction Rate, (M/s) 1 0.0125 0.0130 2.33 x 10-4 2 0.0250 0.0130 9.34 x 10-4 3 0.0250 0.0260 1.87 x 10-3 a. Determine the order with respect to each reactant, A and B2, using the Method of Initial Rates. Justify you answer with a calculation. (See sample calculation section for examples) (2 pts) b. Calculate the value of the rate constant, k, for the reaction of A and B2. Show your work. (See Equation 8 and sample calculation section for examples) (2 pts) c. Write the rate equation for the reaction that includes the calculated value of the rate constant. (see sample calculation section for example) (1 pt)