Ideal Gas Law and Soda
Objective: To determine the amount of carbon dioxide in a can of soda
by using the Ideal Gas Law. By weighing
the can, you can determine the mass lost and thus determine the moles. The temperature and atmospheric pressure can
be also determined to find the volume of the gas. We can also compare results between regular
and diet soda to determine if there is a difference in the amount of carbon
dioxide they contain.
Directions:
1. Determine the atmospheric pressure
in Los Angeles today. Convert to mm of Hg then you will need to convert to
atmospheres.
2. Weigh your unopened can on the
balance.
3. Every two minutes weigh the can
again to see how much mass is lost.
4. Record the temperature of the soda
in the can, as this is also the temperature of the gas.
4. While you are waiting the two
minutes to weigh again, start your graph.
5. On the x-axis graph the time in
minutes and on the y-axis graph the mass of the can. The starting mass of the
can should be the highest point on the y-axis.
6. After 24 minutes, determine the
final mass lost and complete your graph.
7. Use the Ideal Gas Law formula (PV=
nRT) to determine the volume of the gas released by the soda.
8. Paste your graph (make sure it is
labeled) inside your composition book.
Data:
Air pressure in LA (in mm Hg) :
_____________
Air pressure in LA (in atm):
_____________
Initial mass of can: __________ Final mass of
can: __________
Temperature of can: __________
Post-Lab Questions:
1. Show your work to determine the
volume of gas released by the soda use the PV= nRT. Make sure to show all of
the steps of your work.
2. What do you think would be the
affect if you did this experiment at a lower atmospheric pressure? Would it
have a difference on the amount of gas released? (Hint: Think about your gas
laws and the relationships.)
3. Which soda has more gas in it? Why
do you think that one soda has more gas than another? Think about what is the
composition of these sodas.
No comments:
Post a Comment