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Rates of Chemical Reactions
I. Purpose of the Experiment
The purpose of the lab is to identify reaction rates using three different reagents: iodate, sulfurous acid,
and water. By adding the reagents through series of orders, reactions show and data is used to identify the
reaction rates through a formula,
rate=k[HSO
3

]
y
[H
+
]
. This formula is then deduced to the following
formulas:
rate=k
obs
[IO
3

]
x
to
k
obs
k[HSO
3

]
y
[H+]
2
.
To convert this data into a linear graph, this formula is
used:
ln(rate)=xln[IO
3

]+ln(k
obs
)
–
ln(rate)
being the
y
value,
xln[IO
3

]
being the slope, and
ln(k
obs
)
being
the yintercept.
Before so, this formula, M
1
V
1
=M
2
V
2
(M being the concentration in Molarity and V being
the volume in drops), is used to identify the final concentrations for reaction rate equations.
II. Summary of the Procedure
Two pipets were stretched and cut at an angle to ensure consistent drop size. A five cm marking was
placed on a third pipet. A stretched pipet was used to measure x drops of IO
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This note was uploaded on 06/15/2011 for the course CH 118 taught by Professor March during the Fall '09 term at University of Alabama at Birmingham.
 Fall '09
 March
 Chemistry, Reaction

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