Chemistry Reference
In-Depth Information
Analysis
1. Find the mass of the carbonated drink by subtracting the mass of
the syringe from the mass of the syringe and beverage together.
Record this value on the data table.
2. Subtract the mass of the syringe from the mass of the syringe with
the drink after the carbon dioxide was removed to find the mass of
the beverage without carbon dioxide. Record this value on the data
table as the mass of the beverage in the syringe.
3. Find the mass of the carbon dioxide in the drink by subtracting
the mass of the drink with carbon dioxide removed from the mass
of the syringe with carbonated drink in it. Record this value on the
data table.
4. For the purposes of this lab, assume that the beverage being
tested is pure water, H
2
O. Using the mass of the water to represent
the drink with carbon dioxide removed (from the data table) and
the molar (M) mass for water, calculate the number of moles of
water in the sample.
5. Use the mass of carbon dioxide from the data table and the molar
mass of CO
2
to determine the number of moles of CO
2
collected.
6. Determine the ratio of moles of water to moles of carbon dioxide
found in the drink:
mol H
2
O
mol CO
2
7. Multiply the ratio from Analysis question 6 by the M mass of water.
Add this number to the M mass of carbon dioxide. This is the M
mass of the carbonated drink that you tested.
8. Find the percent composition of carbon dioxide in the drink by
dividing the M mass of carbon dioxide by the M mass of the
carbonated drink and multiplying by 100 to obtain a percentage.
9. Why did the carbon dioxide leave the drink when you pulled the
syringe back?
10. Why was it important for the drink to be cold when you poured it into
the syringe? Why was it warmed before extracting the CO
2
?
What's Going On?
The particles of matter in a gas behave differently from those in a liquid.
In a gas, particles are spread out and move at relatively high speeds;
