Asked Dec 4, 2019

A mixture consisting of 0.140 mol N2, 0.037 mol O2, 0.104 mol CH4, and an unknown amount of CO2 occupies a volume of 8.48 L at 27°C and 1.06 atm pressure. How many moles of CO2 are there in this sample?

a. 0.719 mol

b. 2.45 mol

c. 0.364 mol

d. 0.0839 mol

e. 3.77 mol


Expert Answer

Step 1

To calculate the moles of carbon dioxide of given sample using the following gas law formula.


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PV=nRT here, pressure(P)-1.06 atm volume(V) 8.48 L temperature(T)=27'C or 300.15K ideal gas costant(R)=0.08206 L.atm/ mol.K number of moles(n)=?

Step 2

Let us take x is the moles of carbon dioxide, then the total moles of the givne sample as follows:


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Total moles of mixture 0.14+0.037+0.104 x (0.281+x)

Step 3

The calculation of moles of carbon diox...


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PV=nRT PV RT 1.06 atmx8.48 L (0.281 x) moles=. 0.08206 L.atm/mol.K x 300. 15 K (0.281 x) moles=0.36494 moles x 0.08394 moles


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