The times listed in the following table are those required forthe concentration of S2O8^-2 to decrease by 0.00050M as measured inan iodine clock reaction at 23 degree celcius. What is the ratelaw? The net reaction is :

S2O8^-2 + 2I^-1---> I2 + 2SO4^-2

Trial initial[S2O8^-2] Initial[I^-1] Time(Sec)

1 0.0400 0.0800 39

2 0.0400 0.0400 78

3 0.0100 0.0800 156

4 0.0200 0.0200 ?

A. Calculate the expected time in seconds for trial 4

B. What is the rate law?

C. What is the rate constant?

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Nestor RutherfordLv2

6 Nov 2019

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This is Kinetics

Calculate the rest of the rates and record these values into table 2 below (orange column)

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A student prepared the following mixtures and measured the time each took to react. Calculate the average time for each mixture (in seconds).

Mixture	Vol. of 4.0 M acetone (mL)	Vol. of 1.0 M HCl (mL)	Vol. of 0.0050 M I₂ (mL)	Vol. of H₂O (mL)	Time for Trial 1	Time for Trial 2	Average time (s)
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2	20	10	10	10	123	125	124
3	10	20	10	10	121	124	122.5
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To complete the following table:

Determine the initial concentration (molarity) of each reagent using the equation:

The M_stock and V_stock for each reagent are given in problem 1. The total volume is 50 mL for each trial.

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Mixture	[Acetone], M	[H⁺], M	[I₂]₀, M	Rate
1	0.80	0.20	0.0010
2
3
4

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Rate = k[acetone]^m[H⁺]ⁿ[I₂]^p

Use the rate law determined in problem 3 to calculate the rate constant, k for each mixture. Find the average rate constant.

Mixture	1	2	3	4	Average
k

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Concentration (M)				--------------

Use the concentrations for Mixture 5 you just calculated, along with the orders of the reaction (m, n, and p, from problem 3), and the average rate constant (problem 4), to solve Eq. 2 for rate. This is a prediction of how long it will take for the I₂ color to disappear from your mixture.

Rate = k[acetone]^m[H⁺]ⁿ[I₂]^p

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Hi, i completed a kinetic experiment

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