hypophosphate ion(H2PO2-) decomposes in alkaline solution as aresult of the folowing reaction.
H2PO2-+OH-----HP032-+H2
the kinetic of this reaction were bstudied at 100 deg c.thefollowing table lists the initial concentations of thereactants(from three seperate experiment)and the concentrationofone of the product(HPO32- after the reaction has run for 30seconds
| [H2PO2]I | [OH-]I | [HPO32-]30S | RATE |
| EXP1 | 0.10M | 1.0M | 1.6*10-5M | |
| EXP2 | 0.30M | 1.0M | 4.8*10-5M | |
| EXP3 | 0.10M | 2.0M | 6.4*10-5M | |
a)complete the chart by calculating the initial rate for eachexpriment (don not forget to include units).hints what is initialconcentration of the product? what is the delta t?how is the raterelated to product change in concentration?
b) determine the rate law for this reaction.
c)determine the value and units of the rate constant.
d)calculate the rate of reaction if [H2PO2-]I=0.20Mand[OH-]I=0.30M
