In a reaction involving the iodination of acetone, the following volumes were used to make up the reaction mixture:

Question

10 mL 5.0 M acetone + 10 mL 1.5 M HCl + 10 mL 0.005 M I2 + 20 mL H2O

A student found that it took 400 seconds for the color of the I2 to disappear.

a) How many moles of acetone were in the reaction mixture?

b) What was the molarity of acetone in the reaction mixture?

c) What was the rate of the reaction?

d) What was the rate of reaction?

A second reaction mixture was made up in the following:
20 mL 5.0 M acetone + 10 mL 1.5 M HCl + 10 mL 0.005 M I2 + 10 mL H2O
A student found that it took 100 seconds for the color of the I2 to disappear.

e) What were the initial concentration of each solution?

f) What was the rate of the reaction?

i) Write unknowns in either d or f, and calculate each unknown.

Answer 1

A. mols acetone = M x L = ?
B. 5.00 M x (10 mL/total volume)= ?
C. final (I2) = 0.005M x (10 mL/total volume) = ?. Then rate rxn = final (I2)/400
D. repeat of C.

You should be able to use these numbers to do part B yourself.

Answer 2

Do it yourself. Stop Copying.