The reaction 3 BrO- (aq) --> BrO3- (aq) + 2 Br - (aq) in basic solution is second order in BrO-(aq) with a rate constant equal to 0.056 M-1s-1 at 80 degrees Celcius. If [BrO- ]0 = 0.212 M, then what will [BrO- ] be 1.00 min later?

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Kerouac Kerouac · Answer 1 · 2020-01-22T01:54:05+01:00

Answer:

0.124 M

Explanation:

The reaction obeys second-order kinetics:

[tex]r = k[BrO^-]^2[/tex]

According to the integrated second-order rate law, we may rewrite the rate law in terms of:

[tex]\dfrac{1}{[BrO^-]_t} = kt + \dfrac{1}{[BrO^-]_o}[/tex]

Here:

[tex]k[/tex] is a rate constant,

[tex][BrO^-]_t[/tex] is the molarity of the reactant at time t,

[tex][BrO^-]_o[/tex] is the initial molarity of the reactant.

Converting the time into seconds (since the rate constant has seconds in its units), we obtain:

[tex]t = 1.00 min = 60.0 s[/tex]

Rearranging the integrated equation for the amount at time t:

[tex][BrO^-]_t = \dfrac{1}{kt + \dfrac{1}{[BrO^-]_o}}[/tex]

We may now substitute the data:

[tex][BrO^-]_t = \dfrac{1}{0.056 M^{-1}s^{-1}\cdot 60.0 s + \dfrac{1}{0.212 M}} = 0.124 M[/tex]

trevsmith1000000 trevsmith1000000 · Answer 2 · 2020-12-13T01:48:33+01:00

Answer:

thanks but idk top probably right im not smart

Explanation:

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