In Aqueous Solution,hypobromite Ion,BrO^-,reacts to Produce Bromate Ion,BrO₃^-,and Bromide Ion,Br^-,according $$3 \mathrm { BrO } ^ { - } ( a q ) \rightarrow \mathrm { BrO } _ { 3 } ^ { - } ( a q ) + 2 \mathrm { Br } ^ { - } ( a q )$$

In aqueous solution,hypobromite ion,BrO^-,reacts to produce bromate ion,BrO₃^-,and bromide ion,Br^-,according to the following chemical equation: $$3 \mathrm { BrO } ^ { - } ( a q ) \rightarrow \mathrm { BrO } _ { 3 } ^ { - } ( a q ) + 2 \mathrm { Br } ^ { - } ( a q )$$ A plot of 1/[BrO^-] vs.time is linear and the slope is equal to 0.056 L mol^-1 s^-1.If the initial concentration of BrO^- is 0.80 mol L^-1,how long will it take one-half of the BrO^- ion to react?

A) 4.5 × 10^-2 s
B) 7.1 s
C) 12 s
D) 22 s

Correct Answer:

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