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Q: A mixture of 0.423 moles of N2 and 5.73 moles of CO2 has a total...

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Chemistry

Q: A mixture of 0.423 moles of N2 and 5.73 moles ofCO2 has a total pressure of 777 torr. What is thepartial pressure of N2?

Please give the details of the ploblem, thanks.

Answer & Explanation Solved by verified expert
3.9 Ratings (582 Votes)

Answer –
We are given , moles of N2 = 0.423 mole, moles of CO2 = 5.73 mol

Total pressure = 777 torr

We know the relationship between total pressure and partial pressure, Dalton’s law

Mole fraction = partial pressure / total pressure

So, first we need to calculate mole fraction of N2

We know,

Mole fraction of N2 = moles of N2 / total moles

Total moles = 0.423 + 5.73

                   = 6.153 moles

Mole fraction of N2 = 0.423 / 6.153

                                = 0.0687

So, partial pressure of N2 = mole fraction of N2 * total pressure

                                        = 0.0687 * 777 torr

                                         = 53.4 torr
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