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harina [27]
3 years ago
5

In aqueous solution, hypobromite ion, BrO-, reacts to produce bromate ion, BrO3 -, and bromide ion, Br-, according to the follow

ing 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?
Chemistry
1 answer:
maw [93]3 years ago
5 0

Answer:

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

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Hi, the given equation has some missing parts. Actual equation is- 'Mn(OH)_{2}(s)+MnO_{4}^{-}(aq.)\rightarrow MnO_{4}^{2-}(aq.)'

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Mn(OH)_{2}(s)\rightarrow MnO_{4}^{2-}(aq.)

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