62 Experiment 20 Rates of Chemical Reuctiors, I. The lodnation of Acetone 3. A s
ID: 574591 • Letter: 6
Question
62 Experiment 20 Rates of Chemical Reuctiors, I. The lodnation of Acetone 3. A second reaction mixture was made up in the following way 5 mL40 M acetone+20 ml 1.0 MH+ 10 ml.0.0050 Mi, I5mL H,O l a. What were the initial concentrations of acetone, H'ion, and I, in the reaction mixture? molas [acetone]-. M: [tle b. It took 250 seconds for the 1, 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? 250 s Write Equation 3 as it would apply to the secoad reaction mixture: rate = Misec Divide the equation in Part (b) by the equation in Problem 2(b). The resulting equation should have the ratio of the two rates on the left side and a ratio of H' concentrations raised to the p power on the right. Write the resulting equation and solve for the value of p, the order of the reaction with respect to H.(Round off the value of p to the nearest integet.) c. 4. A third reaction mixture was made up in the following way: 5mL 4.0 M acetone + 20m1.0 M Ha 5mL 0,0050 M 12 + 20 mL H2O If the reaction is zero order in Iz, how long would it take for the ly color to disappear at the temperature of the reaction mixture in Problem 3? cona. 1e rate secondsExplanation / Answer
3 a. Formula: molarity = no. of mmol/volume in mL
The no. of mmol of acetone = 4 mmol/mL * 5 mL = 20 mmol
The no. of mmol of HCl = no. of mmol of H+ = 1 mmol/mL * 20 mL = 20 mmol
The no. of mmol of I2 = 0.005 mmol/mL * 10 mL = 0.05 mmol
The total volume of the reaction mixture = 5 + 20 + 10 = 35 mL
Now, the initial concentration of acetone in the reaction mixture, [acetone]0 = 20 mmol/35 mL = 0.57143 M
The initial concentration of H+ in the reaction mixture, [H+]0 = 20 mmol/35 mL = 0.57143 M
The initial concentration of I2 in the reaction mixture [I2]0 = 0.05 mmol/35 mL = 0.00143 M = 1.43*10-3 M
b. The disappearance of I2 color indicates that the final concentation of I2 = 0 M
Now, the rate of reaction = -d[I2]/dt = -{[I2]final - [I2]initial}/dt
= -(0 - 0.00143) M/250 s = 5.72*10-6 M/s
Rate equation: Initial Rate = k[H+]0p [aceonte]0q [I2]0r
Explanation: Here, 'p', 'q', and 'r' are the orders of the reaction with respect to H+, acetone, and I2, respectively.
c. Here, the equation in problem 2(b) is not given.
So, please be sure to do it yourself. In case of any doubt, I'm happy to clarify.
All the best!!!!
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