In a reaction involving the iodination of acetone, the following volumes were us

Question

In a reaction involving the iodination of acetone, the following volumes were used to make up the reaction mixture: 10 mL 4.0 M acetone + 10 mL 1.0 M HC1 + 10 mL 0.0050 M I2 + 20 mL H2O How many moles of acetone were in the reaction mixture? Recall that, for a component A, no. moles A = MA times V, where MA is the molarity of A and V is the volume in liters of the solution of A that was used. moles acetone What was the molarity of acetone in the reaction mixture? The volume of the mixture was 50 mL, 0.050 L, and the number of moles of acetone was found in Part (a). Again, MA = no. moles A / Vof soln. in liters M acetone How could you double the molarity of the acetone in the reaction mixture, keeping the total volume at 50 mL and keeping the same concentrations of H+ ion and I2 as in the original mixture? Using the reaction mixture in Problem 1, a student found that it took 230 seconds for the color of the I2 to disappear. What was the rate of the reaction? Hint: First find the initial concentration of I2 in the reaction mixture, (T2)0. Then use Equation 5. rate = Given the rate from Part (a), and the initial concentrations of acetone, H+ ion, and I2 in the reaction mixture, write Equation 3 as it would apply to the mixture. rate = What arc the unknowns that remain in the equation in Part (b)? A second reaction mixture was made up in the following way: 10 mL 4.0 M acetone + 20 mL 1.0 M HC1 + 10 mL 0.0050 M I2 + 10 mL H2O What were the initial concentrations of acetone, H+ ion, and I2 in the reaction mixture? (acetone) M; (H+) M; (I2)0 M It took 120 seconds for the I2 color to disappear from the reaction mixture when it occurred at the same temperature as the reaction in Problem 2. What was the rate of the reaction? Write Equation 3 as it would apply to the second reaction mixture: rate = Divide the equation in Part (b) by the equation in Problem 2b. The resulting equation should have the ratio of the two rates on the left side and a ratio of acetone concentrations raised to the m power on the right. Write the resulting equation and solve for the value of m, the order of the reaction with respect to acetone. (Round off the value of m to the nearest integer.) m = A third reaction mixture was made up in the following way: 10 mL 4.0 M acetone + 20 mL 1.0 M HC1 + 5 mL 0.0050 M T2 + 15 mL H2O If the reaction is zero order in I2, how long would it take for the I2 color to disappear at the temperature of the reaction mixture in Problem 3?

Explanation / Answer

a) 10/1000*4=.04 moles of acetone

b) (.04/50)*1000=.8 M

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