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

Q: A mixture of 0.423 moles of N₂ and 5.73 moles of CO₂ has a total pressure of 777 torr. What is the partial pressure of N₂?

Please give the details of the ploblem, thanks.

Solutions

Expert Solution

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

queen_honey_blossom answered 1 year ago

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