Question

A second reaction mixture was made up in the following way:

10 mL 4.0 M acetone + 20 mL 1.0 M HCl + 10 mL 0.0050 M I2 + 10 mL H2O
a. What were the initial concentrations of acetone, H+ ion, and I2 in the reaction mixture?
(acetone) ___________ M; (H+) ___________ M; (I2)0 ___________ M
b. It took 120 seconds for the I2 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?

Answer 1

The initial concentrations of acetone, H+ ion, and I2 in the reaction mixture are 4.0 M, 1.0 M, and 0.0050 M, respectively. The rate of the reaction cannot be calculated without knowing the specific reaction.

Step-by-step explanation:

The initial concentrations of acetone, H+ ion, and I2 in the reaction mixture are as follows:

• (acetone) 4.0 M
• (H+) 1.0 M
• (I2)0 0.0050 M

The rate of the reaction can be determined using the given information. However, there is no information provided about the reaction itself, so it is not possible to calculate the rate without knowing the specific reaction.

Answer 2

A. We can calculate the initial concentrations of each by the formula:

initial concentration ci = initial volume * initial concentration / total mixture volume

where,

total mixture volume = 10 mL + 20 mL + 10 mL + 10 mL = 50 mL

ci (acetone) = 10 mL * 4.0 M / 50 mL = 0.8 M

ci (H+) = 20 mL * 1.0 M / 50 mL = 0.4 M (note: there is only 1 H+ per 1 HCl)

ci (I2) = 10 mL * 0.0050 M / 50 mL = 0.001 M

B. The rate of reaction is determined to be complete when all of I2 is consumed. This is signified by complete disappearance of I2 color in the solution. The rate therefore is:

rate of reaction = 0.001 M / 120 seconds

rate of reaction = 8.33 x 10^-6 M / s