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Part A In aqueous solution, hypobromite ion, Bro", reacts to produce bromate ion, Bro, and bromide...
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?
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 rate constant, k, is equal to 0.056 M-1s-1. If the initial concentration of BrO- is 0.80 M, how long will it take* the concentration of the BrO- ion to be 0.40 M? *enter your answer in seconds
just one example/demonstration! Data needed to be calculated is in highlighted in green boxes. And I highlighted in red an equation (not sure if thats what you use to calculate it) And ignore the lab instructions on completeing a graph!! I already know how to do that in excel, just curious how Ln (relative rate) and 1/T in K^-1 is calculated by hand* here is the rest of that lab leading up to the question as I know its typically...