Can I please get some help solving questions 3 (c) and question 4? Thank you. Advance Study Assignment: The lodination of Acetone1. In a reaction involving the iodination of acetone, the following volumes were used to make up the reac-tion mixture:mol HCl = 1.010L = .01 mer0502 2.20 Ma. How many moles of acetone were in the reaction mixture? Recall that, for a component A, molesA = MAX V, where MA is the molarity of A and V is the volume in liters of the solution of A thatwas used.molacedone = 4.0M 0.005 L=0.02 mol0.020 moles acetone5 mL 4.0 M acetone + 10 mL 1.0 M HCl + 10 mL 0.0050 M I₂ + 25 mL H₂Ob. 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,moles of AMA= V of soln. in litersC.0.020-40 M0.050 Lc. How could you double the molarity of the acetone in the reaction mixture, keeping the total volumeat 50 mL and keeping the same concentrations of H* ion and I, as in the original mixture?reduce the amount of H₂0 byand5 MLadding 5mL of 4.0 Macetone.110ML 4.0 M acetone + 10mL 1.0 M HCl + 10mL 0.0050 MI₂ + 20 ML H₂O2. Using the reaction mixture in Problem 1, a student found that it took 510 seconds for the color of the 1₂ todisappear.a. What was the rate of the reaction? Hint: First find the initial concentration of I₂ in the reaction mix-ture, [1₂]o. Then use Equation 5.[1₂] = 0,001 MMol 1₂.0050m..000=.000050 mol = 0.001 M050Lrate= -A[₂][12] 0.001 m-401] [12]AEErate=5-109000196 m/510 seconds= K[Acetone] [1₂] [4+] P0.40m/sec20 X 10 m/seerate=b. Given the rate from Part (a), and the initial concentrations of acetone, H* ion, and I₂ in the reactionmixture, write Equation 3 as it would apply to the mixture.What are the unknowns that remain in the equation in Part (b)?kmM acetone2.0X102.0 X16-bM/sec = K[020] [0,0010] "B.267PM/secnP(continued on following page) 162Experiment 20 Rates of Chemical Reactions, I. The lodination of Acetone3. A second reaction mixture was made up in the following way:5 mL 4.0 M acetone + 20 mL 1.0 M HCl + 10 mL 0.0050 M 1₂ + 15 mL H₂Oa. What were the initial concentrations of acetone, H ion, and I₂ in the reaction mixture?Molac 4.0 M•.005 L = 0,02 mol = 0.410 M [accion]05LMol 4₁ = 1.0.020=02MolI₂ = 60100050 = 0.00005 = .001 MM; [1₂] .0010 M[acetone]0.40M; [H+]40b. It took 250 seconds for the 1₂ color to disappear from the reaction mixture when it occurred at thesame temperature as the reaction in Problem 2. What was the rate of the reaction?Fate == A[1₂]001 MAt= 0000040 = 4.0 x10-6 M/sec250 Secrate =-4.6x10-6rate =4. A third reaction mixture was made up in the following way:Write Equation 3 as it would apply to the second reaction mixture:K[Acetone] [1₂] "H41.0 x 10-M/sec = .407.0010] [40]c. Divide the equation in Part (b) by the equation in Problem 2(b). The resulting equation should havethe ratio of the two rates on the left side and a ratio of H* concentrations raised to the p power on theright. Write the resulting equation and solve for the value of p, the order of the reaction with respectto H. (Round off the value of p to the nearest integer.)Rate 3b 41,0X10 m/sec_ *[0.40] [0.001] [040]Rate 26k[0.020][0.0010] (0.402.0 x10-6 sec2=P=.105 = 40M5 mL 4.0 M acetone + 20 mL 1.0 M HCl + 5 mL 0.0050 M I₂ + 20 mL H₂OM/secIf the reaction is zero order in I₂, how long would it take for the I₂ color to disappear at the temperature ofthe reaction mixture in Problem 3?seconds

First, lets find the initial concentration of I2. [I2] = Moles of I2Total volume in L Moles = M…

4. A third reaction mixture was made up in the following way: 5 mL 4.0 M acetone + 20 mL 1.0 M HCl + 5 mL 0.0050 M 1₂ + 20 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? seconds

4. A third reaction mixture was made up in the following way: 5 mL 4.0 M acetone + 20 mL 1.0 M HCl + 5 mL 0.0050 M 1₂ + 20 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? seconds

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter15: Principles Of Chemical Reactivity: Equilibria

Section15.6: Disturbing A Chemical Equilibrium

Problem 2.2ACP

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