Question

Using the reaction mixture 10 mL 4.0 M acetone + 10 mL 1.0 M HCl +...

Using the reaction mixture
10 mL 4.0 M acetone + 10 mL 1.0 M HCl + 10 mL .0050 M I2 + 20 mL H2O
a student found that it took 230 seconds for the color of the I2 to disappear.
a. What was the rate of the reaction?
b. Given the rate from part a, and the initial concentration of acetone, H+ ion, and I2 in the reaction mixture, write the rate equation.
c. What are the 4 unknowns that remain in the equation part b?
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Homework Answers

Answer #1

SOLUTION:

The reaction is iodination of acetone.

CH3COCH3 + I2 + H+ ----------> CH3COCH2I + HI

(A) Rate = - (chane in concentration of I2 / time taken)

chane in concentration of I2 = Final concetration - initial concentratio = (0 - 0.0050) = - 0.005M

t = 230s

Rate = - (chane in concentration of I2 / time taken) = - ( - 0.005 / 230) = 2.173 X 10-5 Ms-1

(B) Rate equation is given as

Rate = k[Acetone]a[I2]b[H+]c

(C) The four unknowns are given below:

1 rate contsant (k), 2. a, 3. b, 4. c

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