A student is performing rate measurements for the reaction of I- with H2O2 in a buffer solution. The rate law for the reaction is known to be Rate = kâ[I- ]^1 [H2O2]^1 . The student mixed 6 ml of DI water, 1.0 ml of Buffer, 1 ml of 0.3 M KI, 1 ml of 0.02 M Na2S2O3, 1 ml of 0.1 M H2O2 and 5 drops of starch and notices a color change after 54 seconds. What time would it take the solution to change the color if:

a) The concentrations of both KI and H2O2 were decreased by a factor of 2.

b) The concentration of Na2S2O3 was increased by a factor of 2.

Question

A student is performing rate measurements for the reaction of I- with H2O2 in a buffer solution. The rate law for the reaction is known to be Rate = kâ[I- ]^1 [H2O2]^1 . The student mixed 6 ml of DI water, 1.0 ml of Buffer, 1 ml of 0.3 M KI, 1 ml of 0.02 M Na2S2O3, 1 ml of 0.1 M H2O2 and 5 drops of starch and notices a color change after 54 seconds. What time would it take the solution to change the color if:

a) The concentrations of both KI and H2O2 were decreased by a factor of 2.

b) The concentration of Na2S2O3 was increased by a factor of 2.

Volume Added to Solution 1	Reaction time (s)	Total Volume (L)	Rate (mol/LÂ·s)
25 mL (NH4)2S2O8	182	0.075
1 mL Na2S2O3	73	0.076
1 mL Na2S2O3	185	0.077
1 mL Na2S2O3	114	0.078

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