How do you handle the calculations and data for the gas law lab (molar mass of butane)? February 27.
-
Upload
jane-morgan -
Category
Documents
-
view
214 -
download
0
Transcript of How do you handle the calculations and data for the gas law lab (molar mass of butane)? February 27.
How do you handle the calculations and data for the gas law lab (molar
mass of butane)?February 27
Finishing up the Gas UnitData Calculations: Trial 1
Calculate pressure of gas sample:PT = Pgas + Pwater
759.0 mmHg = Pgas - 23.1 mmHg
Pgas = 735.9 mmHg or 0.9683 atm
Calculate mass of butane in gas sample:Mass of butane = Initial mass – Final mass
Calculate moles of butane in gas sample:PV = nRT
Calculate molar mass for this Trial:Mass of butane / Moles of butane
Trial 1
Atmospheric Pressure (PT)
759.0 mmHg
Water Temperature in K 24.5 C or 297.5 K
Water vapor pressure at temperature recorded.
23.1 mmHg
Initial Mass of Lighter
16.9523 g
Final Mass of Lighter.
16.8501g
Volume of gas sample in Liters
47.80 mL or0.04780 L
Click on number for water vapor table.
Finishing up the Gas Unit
Data
Calculations: Trial 1Calculate pressure of gas sample:PT = Pgas + Pwater
Calculate mass of butane in gas sample:Mass of butane = Initial mass – Final mass16.9523 g – 16.8501 g = 0.1002 g
Calculate moles of butane in gas sample:PV = nRT
Calculate molar mass for this Trial:Mass of butane / Moles of butane
Trial 1
Atmospheric Pressure (PT)
759.0 mmHg
Water Temperature in K 24.5 C or 297.5 K
Water vapor pressure at temperature recorded.
23.1 mmHg
Initial Mass of Lighter
16.9523 g
Final Mass of Lighter.
16.8501g
Volume of gas sample in Liters
47.80 mL or0.04780 L
Finishing up the Gas Unit
Data
Calculations: Trial 1Calculate pressure of gas sample:PT = Pgas + Pwater
759.0 mmHg = Pgas + 23.1 mmHg
Pgas = 735.9 mmHg or 0.9683 atm
Calculate mass of butane in gas sample:Calculate moles of butane in gas sample:PV = nRT0.9863 atm ( 0.04780 L) = n (.0821 Latm/(molK) 297.5K
0.9863 X 0.04780 / 0.0821/297.5 =
0.001930 molesCalculate molar mass for this Trial:Mass of butane / Moles of butane
Trial 1
Atmospheric Pressure (PT)
759.0 mmHg
Water Temperature in K 24.5 C or 297.5 K
Water vapor pressure at temperature recorded.
23.1 mmHg
Initial Mass of Lighter
16.9523 g
Final Mass of Lighter.
16.8501g
Volume of gas sample in Liters
47.80 mL or0.04780 L
Finishing up the Gas Unit
Data
Calculations: Trial 1Calculate pressure of gas sample:
Calculate mass of butane in gas sample:Mass of butane = Initial mass – Final mass16.9523 g – 16.8501 g = 0.1022 g
Calculate moles of butane in gas sample:PV = nRT
0.001930 moles
Calculate molar mass for this Trial:Mass of butane / Moles of butane 0.1022 g / 0.001930 = 52.95 g/mol
Trial 1
Atmospheric Pressure (PT)
759.0 mmHg
Water Temperature in K 24.5 C or 297.5 K
Water vapor pressure at temperature recorded.
23.1 mmHg
Initial Mass of Lighter
16.9523 g
Final Mass of Lighter.
16.8501g
Volume of gas sample in Liters
47.80 mL or0.04780 L