# calculatr the rates of the following ifesperiment initial {S2O8^-2} initial { l-} rate1 0.05M 0.05M ----------------2 0.10M 0.05M -----------------3 0.05M 0.10M -----------------Find x y and k in the rate lawcalculate the rate.Note; each experiment has a solution volume OF 100ml with with subsequent addition of one drop of S2O3^-2 several times to upto five drops each against reaction times in seconds.

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calculatr the rates of the following if
esperiment initial {S2O8^-2} initial { l-} rate
1 0.05M 0.05M ----------------
2 0.10M 0.05M -----------------
3 0.05M 0.10M -----------------

Find x y and k in the rate law
calculate the rate.
Note; each experiment has a solution volume OF 100ml with with subsequent addition of one drop of S2O3^-2 several times to upto five drops each against reaction times in seconds.

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Step 1

Question is based on rate law. Using the given data we have to calculate the values of x,y i.e. order of reaction, rate constant k and rate of reaction.
This is incomplete question. Rate values for experiments are not given so we are solving this question by comparing the concentration data of experiment 1 with experiment 2 and 3.

Step 2

Step2. Set up the rate law equation for experiment 2.

In experiment 2 the initial concentration of S2O82- ion is twice that in experiment 1while concentration of I- ion is constant. So the rate law equation for experiment 2 will be

Step 3

Step3. Set up the rate law equation for experiment 3.

In experiment 3 the initial concentration of S2O82- ion is constant while concentration of I- ion is twice...

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