Chemistry Reference
In-Depth Information
Data Table 1
Mass of lighter before butane is released
Mass of lighter after butane is released
Mass of butane (lighter mass before
minus lighter mass after)
Temperature (
°
C) of water
Volume of butane (ml)
Barometric pressure
Pressure of butane (barometric pressure
minus partial pressure of water vapor)
2. Which of the following values for the gas constant (
R
) will you use:
0.0821 L ×
atm
× K
or
8.31 L ×
kPa
× K?
mol mol
Hint
: look at the units in your barometric pressure reading.)
3. Using the temperature of the water from Data Table 1, find the
partial pressure of water vapor in your experiment on Data Table
2, which shows how water vapor pressure varies as temperature
increases. Use the value from Data Table 2 as well as the
barometric pressure to determine the partial pressure of butane
using the following equation (
Dalton's law of partial pressure
):
P
total
=
P
1
+
P
2
where
P
total
is the barometric pressure,
P
1
is the vapor pressure of
water, and
P
2
is the pressure of butane.
4. Convert the volume measurement from Data Table 1 from milliliters
to liters by dividing by 1,000.
