A second reaction mixture was made up in the following way: 20 mL 4.0 M acetone

ID: 481812 • Letter: A

Question

A second reaction mixture was made up in the following way: 20 mL 4.0 M acetone + 10 mL 1.0 M HCl + 10 mL 0.0050 M I_2 + 10 mL H_2O What were the initial concentrations of acetone, H^+ ion. and I_2 in the reaction mixture? (acetone) _____ M: (H^+) _____ M; (I_2)_0 = _____ M It took 120 seconds for the I_2 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: 20 mL 4.0 M acetone + 10 mL 1.0 M HCl + 20 mL 0.0050 M I_2 If the reaction is zero order in I_2, how long would it take for the I_2 color to disappear at the temperature of the reaction mixture in Problem 3? _____ Seconds

Explanation / Answer

3. From the given data

a. Initial concentration of,

[acetone] = 4 M x 20 ml/50 ml = 1.6 M

[H+] = 1.0 M x 10 ml/50 ml = 0.2 M

[I2] = 0.005 M x 10 ml/50 ml = 0.001 M

b. rate of reaction = -d[I2]/dt

= 0.001/120

= 8.33 x 10^-6 M/s

4. From the given data

If the reaction is zero order with respect to acetone,

tehe overall rate of reaction becomes dependent only on HCl concentration

rate = -d[HCl]/dt

So the rate of reaction would be independent of concentration of acetone and would follow a zero order overall kinetics.

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A second reaction mixture was made up in the following way: 20 mL 4.0 M acetone

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