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Question
The reaction between selenous acid and the iodide ion in acid solution is
H2SeO3(aq) + 6I-(aq) + 4H+(aq) → Se(s) + 2I3-(aq) + 3H2O(l)
The data in the following table were measured at 0C.
| Experiment | [H2SeO3]0(M) | [H+]0(M) | [I"]0(M) | Initial Rate [mol/(L·s)] |
| 1 | 1.00 x 10-4 | 2.00 x 10-2 | 3.00 x 10-2 | 5.30 x 10-7 |
| 2 | 2.00 x 10-4 | 2.00 x 10-2 | 3.00 x 10-2 | 1.06 x 10-6 |
| 3 | 3.00 x 10-4 | 4.00 x 10-2 | 3.00 x 10-2 | 6.36 x 10-6 |
| 4 | 3.00 x 10-4 | 8.00 x 10-2 | 3.00 x 10-2 | 2.54 x 10-5 |
| 5 | 3.00 x 10-4 | 8.00 x 10-2 | 6.00 x 10-2 | 2.04 x 10-4 |
| 6 | 2.00 x 10-4 | 2.00 x 10-2 | 6.00 x 10-2 | 8.48 x 10-6 |
What is the rate constant for this reaction?
A) 1.5 x 104L5/(mol5·s)
B) 1.5 x 1010L5/(mol5·s)
C) 4.9 x 105L5/(mol5·s)
D) 294 L5/(mol5·s)
E) 8.8 L5/(mol5·s)
Answer
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