1. In a reaction involving the iodination of acetone, the following volumes were used to make up the reaction mixture. 1.0 mL 4.0 M acetone + 1.0 mL 1.0 M HCl + 1.0 mL 0.0050 M 12+ 2.0 mL H₂O a. Calculate the initial (diluted) concentration of acetone in the reaction mixture. Moles=4.0.001 -0.004 moles ImL ЧМ moles 0.001 (1+1+112) mL 4= 0.004 mol 0.005 Titre =0.8 [acetonelini = 0.8M b. Calculate the initial (diluted) concentration of the hydrogen ion, H*, in the reaction mixture. 1.0.001 = 0-001 mole 0.005 Titre =0.2M = 5mL 0.001 mol [H]ini = 0.2M c. Calculate the initial (diluted) concentration of iodine, I2, in the reaction mixture. Iml 0.005M/2 0.005 0.001 = 5×10-6 5x10 moles 0.005 litre rate= = 0.001M [12]ini = 0.001 M 2. Using the reaction mixture in Problem 1, a student found that it took 300 seconds for the color of the 12 to disappear. a. What was the rate of the reaction? rate= b. Given the rate from Part a and the initial concentrations of acetone, H+ ion, and 1₂ in the reaction mixture, write Equation 3 as it would apply to the mixture. c. What are the unknowns that remain in the equation in Part b?

for the reactants: ester and enolate ion. • Assume all esters to be ethyl esters. . Do not include counter-ions, e.g., Nat, It, in your answer. • Draw the enolate ion in its carbanion form. • Draw one structure per sketcher. Add additional sketchers using the drop-down menu in the bottom right corner. • Separate multiple reactants using the + sign from the drop-down menu. ? O-Sn [F

For these next two mechanism questions, do each step above the arrows one at a time. i.e. don't try and do them all at once OH 1. NaH (1 eq.) 2. 0⁰ 3. NaOH H₂O

just 2 please