A student carried out reactions A through D as designed in Table 1 in your electronic...

A student carried out reactions A through D as designed in Table 1 in your electronic lab manual, plotted log(rate) vs. log(I-) in EXCEL, and the linear regression yielded the following equation: y = 2..732x-1.032; and the plot of log(rate ) vs. log [IO3-] yield y = 1.368x-1.674.

The order for I- is?

The order for IO3- is?

Solutions

Expert Solution

in the above question we have to find the order .To find the order of reaction we have to use rate law from the above we conclude that the order w.r.t [I^-] and [IO₃^-] is one

according to rate law r = k[I^-]^a where a is not equal to stiochiometric of the balanced chemical equation y = mx + c is a straight line equation where c is the intercept and m is the slope of the line.

queen_honey_blossom answered 8 months ago

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