- Determine the concentrations you would use in order to find therate law for a given reaction.
a.   Here is one set ofconditions – fill out the rest of the table with enough sets ofconditions to determine the rate law for the reaction:
A + B àC + D
b.   If you determinethat the reaction is first order in A and first order in B, fillout the table below with the rate you would expect for each of theconditions you described in part a. (You will have to copy theconditions from part a to the new table.)
[A] mol/L | [B] mol/L | Initial rate mol/(L×min) |
1.0 | 1.0 | 2.0 |
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c.   What is the rateequation for the reaction?
d.   What is the valueof the rate constant?  Be sure to include appropriateunits.
e.   If the reaction iszero order in A and 2nd order in B, fill out the tablewith the rates you would expect.
[A] mol/L | [B] mol/L | Initial rate mol/(L×min) |
1.0 | 1.0 | 2.0 |
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f.    What is therate equation for the reaction?
g.   What is the valueof the rate constant?  Be sure to include appropriateunits.
2.   How would youdetermine the initial rates of the reactionexperimentally? What measurements would you record and how wouldyou treat the data?
3.   Lets say you havea new reaction and you think that the reaction has a rateequation:  Rate = k[A]2
However, you only have one set of [A]vs time data. Describe how you would determine what the rateequation is from this one set of data.
4.   For a first orderreaction, graph the concentration of reactant A ([A]) vs time. Onthis same graph indicate two half-life time periods. (That is showwhere the concentration falls by one half, for two timeperiods).
5.   The carbon-14decay rate of a sample obtained from a young live tree is 0.260disintegrations/(s·g). Another sample prepared from anarchaeological excavation gives a decay rate of 0.186disintegrations/(s·g). The half-life of carbon-14 is 5730 years.What is the age of the object?
