Could someone double check my results from an investigating the
rates of reaction lab session I did recently? Also I'd be very
grateful if someone could help me with filling out the second page
and if its first, second order etc as I don't properly understand
that.
Could Someone Double Check My Results From An Investigating The Rates Of Reaction Lab Session I Did Recently Also I D B 1 (82.59 KiB) Viewed 27 times
Results: Fill your results in the following table. Initial Row # Initial [S208?) Volume of thiosulphate used (Vthio) mL [12] produced after 10 minutes of reaction Average initial rate of reaction (d[12]inid/dt = [12]10min/10 min) M min-1 M M ml M 1 0.2 0.028 5.76 10.00288 0.000288 2 0.1 0.028 2.52 0.00126 0.000126 3 0.05 0.028 1.35 0.000675 10.0oo0675 Initial Initial [0] Volume of thiosulphate used (Vthio) mL [12] produced after 10 minutes of reaction Row # Average initial rate of reaction (d[12]init/dt = [12] 10min/10 min) [S2082') M M min-1 ml M M 2 0.1 0.028 2.52 0.00126 10.000126 4 4 0.1 0.056 10.00279 5.58 10.000279 5 0.1 0.112 10.71 0.005355 10.0005355
the [1] will halve the rate; doubling the [1] should double the rate, etc. If the reaction is second order in iodide, x = 2, the rate is proportional to and halving the [l] will reduce the rate by a factor of four. Look at the data and decide what the order of reaction is with respect to iodide: order X = ********************* Now, do the same thing with the second data set, where is kept constant and [S2O8?] changes (i.e. Row #s 3 - 5). Look at the data and decide what the order of reaction is with respect to persulphate: y = order Thus the rate law for the reaction is: The overall order of the reaction is
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