please need help 1.)A student conducting the iodine clock experiment accidentall

Question

please need help

1.)A student conducting the iodine clock experiment accidentally makes an S2O32- stock solution that is too concentrated. How will this affect the rate measurement and the calculated value of k?

2.) The iodine clock experiment consists of the following three reactions, where Reaction 1 is slow relative to Reactions 2 and 3. Predict what would happen if Reaction 2 was slow relative to Reaction 1 (assume that Reaction 3 is still fast). Reaction 1: 3I- (aq) + S2O82- (aq) I3- (aq) + 2SO4- (aq) slow Reaction 2: I3- (aq) + 2S2O32- (aq) 3I- (aq) + S4O62- (aq) fast Reaction 3: I3- (aq) + starch (aq) 3I- ---- starch (bluish black) fast

Explanation / Answer

1) If S2O3 2- concentration is too high, all of the iodine is converted back to iodide

Rate of the reaction increases. K value also increases

2) If reaction2 was slow relative to reaction1

rate = k1 [I3-] [S2O3 2-]2 order =3

if not rate law would have been

rate = k2[I-]3 [S2O8 2-] order =4

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