In aqueous solution, hypobromite ion, BrO-, reacts to produce bromate ion, BrO3 -, and bromide ion, Br-, according to the following chemical equation. 3 BrO - (aq) → BrO3 - (aq) + 2 Br - (aq) A plot of 1/[BrO-] vs. time is linear and the slope is equal to 0.056 M-1s-1. If the initial concentration of BrO - is 0.80 M, how long will it take one-half of the BrO - ion to react?

Question

Anabella Ross

Chemistry

5 December, 23:05

In aqueous solution, hypobromite ion, BrO-, reacts to produce bromate ion, BrO3 -, and bromide ion, Br-, according to the following chemical equation. 3 BrO - (aq) → BrO3 - (aq) + 2 Br - (aq) A plot of 1/[BrO-] vs. time is linear and the slope is equal to 0.056 M-1s-1. If the initial concentration of BrO - is 0.80 M, how long will it take one-half of the BrO - ion to react?

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Answers (1)

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Gilberto Bartlett · Answer 1

22.73s

Explanation:

The reaction is a second order reaction, we know this by observing the unit of the slope.

rate constant = k = 0.056 M-1s-1

the initial concentration of BrO - [A]o = 0.80 M

time = ?

Final concentration [A]t = one-half of 0.80 M = 0.40M

1 / [A]t = kt + 1 / [A]o

1 / 0.40 = 0.056 * t + 1 / 0.80

t = (2.5 - 1.25) / 0.056

t = 22.73s