Trial [I-] (M) [BrO3-] (M) [H+] (M) 1 1.67*10-3 6.67*10-3 1.67*10-2 2 3.33*10-3 6.67*10-3 1.67*10-2 3 1.67*10-3 1.33*10-2 1.67*10-2 4 1.67*10-3 6.67*10-3 3.33*10-2 Reaction time: Trial 1 - 301.90 secs Trial 2 - 213.28 secs Trial 3 - 214.92 secs Trial 4 - 86.45 secs Calculate the rate for each trial and Using the information above determine the rate law (m, n and p) for the reaction. m_____________ n_________________ p ____________ Rate= k[I-]m[BrO3-]n[H+]p
Trial [I-] (M) [BrO3-] (M) [H+] (M) 1 1.67*10-3 6.67*10-3 1.67*10-2 2 3.33*10-3 6.67*10-3 1.67*10-2 3 1.67*10-3 1.33*10-2 1.67*10-2 4 1.67*10-3 6.67*10-3 3.33*10-2 Reaction time: Trial 1 - 301.90 secs Trial 2 - 213.28 secs Trial 3 - 214.92 secs Trial 4 - 86.45 secs Calculate the rate for each trial and Using the information above determine the rate law (m, n and p) for the reaction. m_____________ n_________________ p ____________ Rate= k[I-]m[BrO3-]n[H+]p
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question
6 I- + BrO3- + 6 H+ ----- 3 I2 + Br- + 3 H2O
Rate= k[I-]m[BrO3-]n[H+]p
rate= (∆[I2])/(3*∆time)
| Trial | [I-] (M) | [BrO3-] (M) | [H+] (M) |
| 1 | 1.67*10-3 | 6.67*10-3 | 1.67*10-2 |
| 2 | 3.33*10-3 | 6.67*10-3 | 1.67*10-2 |
| 3 | 1.67*10-3 | 1.33*10-2 | 1.67*10-2 |
| 4 | 1.67*10-3 | 6.67*10-3 | 3.33*10-2 |
Reaction time: Trial 1 - 301.90 secs Trial 2 - 213.28 secs Trial 3 - 214.92 secs Trial 4 - 86.45 secs
Calculate the rate for each trial and Using the information above determine the rate law (m, n and p) for the reaction.
m_____________ n_________________ p ____________
Rate= k[I-]m[BrO3-]n[H+]p
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