Consider the following data for air trapped in a flask: Pressure = 0.988 atm Room Temperature = 23.5°C Volume of the flask = 1.042 L For this calculation, assume air is 78.5% nitrogen and 21.5% oxygen (by number of moles). R = 0.0821 L•atm•mol-1•K-1 N = 14.01 g/mol O = 16.00 g/mol What is the mass of air in the flask

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russelllang3820 russelllang3820

03-12-2019
Chemistry

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Consider the following data for air trapped in a flask: Pressure = 0.988 atm Room Temperature = 23.5°C Volume of the flask = 1.042 L For this calculation, assume air is 78.5% nitrogen and 21.5% oxygen (by number of moles). R = 0.0821 L•atm•mol-1•K-1 N = 14.01 g/mol O = 16.00 g/mol What is the mass of air in the flask

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waqaskhan15836 waqaskhan15836 · Answer 1 · 2019-12-03T15:45:08+01:00

Answer:

total mass will be = = 1.207g

Explanation:

First what is given

Pressure P= 0.988 atm Room TemperatureT = 23.5°C= 296.5 K

Volume V= 1.042 L

Nitrogen in air is 80 % (moles number) = 0.8

Ideal gas constant R = 0.0821 L atmmol-1K-1

Given mass of N = 14.01 g/mol

Given mass of oxygen O = 16.00 g/mol

Total number of moles = ?

So first we have to find the total number of moles by using formula

Total number of moles

n = PV/ RT

adding the values

moles n= 0.988atm x 1.042L / (0.0821L-atm/mole-K x 296.6K)

= 1.0294 / 24.35

= 0.042 moles (total number of moles)

So by using Nitrogen percentage

Moles of nitrogen = total moles x 80/100

= 0.042moles x 0.8

So moles of O2= Total moles – moles of N2

= 0.042moles - 0.034moles

Moles of O2 = 0.008moles

Now for finding the mass of the N2 and oxygen

Mass of Nitrogen N2 = no of moles x molar mass

= 0.034 x 28

= 0.952 g

Mass of oxygen O2 = no of moles x molar mass

= 0.008 x 32

= 0.256 g

total mass will be = Mass of Nitrogen N2 + Mass of oxygen O2

=0.952 g + 0.256 g

=1.207g

throwdolbeau throwdolbeau · Answer 2 · 2022-03-10T11:00:16+01:00

The mass of air in the flask = 1.207g

Given:

Pressure, P= 0.988 atm

Room Temperature, T = 23.5°C= 296.5 K

Volume, V= 1.042 L

Nitrogen in air is 80 % (moles number) = 0.8

Ideal gas constant R = 0.0821 L atm [tex]mol^{-1}K^{-1}[/tex]

Molar mass of N = 14.01 g/mol

Molar mass of oxygen O = 16.00 g/mol

To find:

Total number of moles = ?

Calculation for number of moles:

From ideal gas law:

n = PV/ RT

n= 0.988atm * 1.042L / (0.0821 L atm [tex]mol^{-1}K^{-1}[/tex] * 296.6K)

n = 1.0294 / 24.35

n= 0.042 moles

Using mol fraction we will calculate moles for nitrogen and oxygen:

Moles of nitrogen = total moles * 80/100

Moles of nitrogen = 0.042moles * 0.8 = 0.034 moles

So, Moles of O₂ = Total moles – moles of N₂

Moles of O₂ = 0.042 moles - 0.034 moles

Moles of O₂ = 0.008 moles

Calculation for mass:

Mass of Nitrogen N₂ = no of moles x molar mass

= 0.034 x 28

= 0.952 g

Mass of oxygen O₂ = no of moles x molar mass

= 0.008 * 32

= 0.256 g

Total mass will be = Mass of Nitrogen N₂ + Mass of oxygen O₂

=0.952 g + 0.256 g

Total mass = 1.207g

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