Question

In a reaction involving the ionization of acetone, the following reaction reaction mixture was used: 5.00mL 4.0M acetone, 5.00mL 1.00M HCl, 5.00mL 0.0050M 12 and 10.0mL water.

1. what was the molarity of the acetone in the reaction mixture? (recall that M1 x V1 = M2V2)

2. the color of the above reaction mixture disappeared in 250 seconds. what was the rate of the reaction? (hint: first dertimine the initial concentration of the iodine)

Answer 1

1.)

M1 x V1 = M2 x V2

4 x 5 = M2 X ( 5+5+5+10)

20 = M2 x 25

M2 = 4/5

M2 = 0.8 M

2.)

Rate = [I₂]/t (standard formula)

= 0.005/250

= 2 x 10^-5 M/s