In a solution at constant H+ concentration, iodide ions react with hydrogen peroxide to produce iodine.
H+ + I- + 1/2H2O2 --> 1/2I2(aq) + H2O
The reaction rate can be followed by monitoring the appearance of I2. The following data were obtained:
[I-]____[H2O2]____Initial rate (M/min)
.015____ .030 ____.0022
.035____ .030 ____.0052
.055____ .030 ____.0082
.035____ .050 ____.0087
a) Write a rate expression for the reaction.
My answer --> rate= K[I-][H2O2]
b) Calculate K.
My work/answer -->
.0022 M/min= K[.015M][.030M]
.0022 M/min= 4.5 E-4 M^2 * K
4.9 1/M*min= K
c) What is the rate of the reaction when 25.0 mL of a .100 M solution of KI is added to 25.0 mL of a 10.00% by mass solution of H2O2 (d= 1.00 g/mL)? Assume volumes are additive.
My answer -->
I have been unable to figure out this part. I know KI is just used to introduce I- into solution, but I don't know how to go about solving it. Any help would be appreciated.
1 answer