6 I- + BrO3- + 6 H+ ----- 3 I2 + Br- + 3 H2O Rate= k[I-]m[BrO3-]n[H+]p rate= (∆[I2])/(3*∆time) [I-] 0.010M [S2O3-2] 0.0010M H2O [BrO3-] 0.04M HCl 0.10M Starch Indicator (sec.) Volume, ml Volume, ml Volume, ml Volume, ml Volume, ml 1 10 10 20 10 10 1-3 drops 301.90 2 20 10 10 10 10 1-3 drops 213.28 3 10 10 10 20 10 1-3 drops 214.92 4 10 10 10 10 20 1-3 drops 86.45 Temperature of Reaction: _20 C 1. Using the dilution equation (M1V1 = M2V2) calculate the concentration of the I-, BrO3- and the H+ (HCl) in the final mixture just prior to any reaction. 2. Calculate the rate for each experiment as explained in the background information. 3. Using the information above determine the rate law (m, n and p) for the reaction. Show all calculations/reasoning in your notebook. m_ n_ p Rate= k[I-]m[BrO3-]n[H+]p Calculate the rate constant for each experiment and then the average. k k k k Average value of k __________ (include units) Rewrite rate law including values for m, n, p and the average value of k:

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy

Section: Chapter Questions

Problem 59GQ: Sulfur undergoes a phase transition between 80 and 100 C. S8(rhombic) S8(monoclinic) rH = 3.213...

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6 I^- + BrO₃^- + 6 H⁺ ----- 3 I₂ + Br^- + 3 H₂O

Rate= k[I^-]^m[BrO₃^-]ⁿ[H⁺]^p

rate= (∆[I₂])/(3*∆time)


	[I^-] 0.010M	[S₂O₃^-2] 0.0010M	H₂O	[BrO₃^-] 0.04M	HCl 0.10M	Starch Indicator	(sec.)
	Volume, ml	Volume, ml	Volume, ml	Volume, ml	Volume, ml
1	10	10	20	10	10	1-3 drops	301.90
2	20	10	10	10	10	1-3 drops	213.28
3	10	10	10	20	10	1-3 drops	214.92
4	10	10	10	10	20	1-3 drops	86.45

Temperature of Reaction: _______20 C________

1. Using the dilution equation (M1V1 = M2V2) calculate the concentration of the I-, BrO3- and the H+ (HCl) in the final mixture just prior to any reaction.

2. Calculate the rate for each experiment as explained in the background information.

3. Using the information above determine the rate law (m, n and p) for the reaction. Show all calculations/reasoning in your notebook.

m_____________ n_________________ p ____________

Rate= k[I^-]^m[BrO3^-]ⁿ[H⁺]^p

Calculate the rate constant for each experiment and then the average.

k______________ k________________ k________________ k ____________

Average value of k __________________ (include units)

Rewrite rate law including values for m, n, p and the average value of k:

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