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

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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

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