A rigid tank contains 2 kg of N2 and 4 kg of Co2 at temperature of 25 C and 1 MPa. Find the partial pressure of each gas respectively?

Partial pressures are 0.6 MPa for nitrogen gas and 0.4 MPa for carbon dioxide.

Explanation: Dalton's Law of Partial Pressure states when there is a mixture of gases the total pressure is the sum of the pressure of each individual gas:

The proportion of each individual gas in the total pressure is expressed in terms of mole fraction:

= moles of a gas / total number moles of gas

The rigid tank has total pressure of 1MPa.

molar mass = 14g/mol

mass in the tank = 2000g

number of moles in the tank: = 142.85mols

molar mass = 44g/mol

mass in the tank = 4000g

number of moles in the tank: = 90.91mols

Total number of moles: 142.85 + 90.91 = 233.76 mols

To calculate partial pressure:

For Nitrogen gas:

= 0.6

For Carbon Dioxide:

0.4

Partial pressures for N₂ and CO₂ in a rigid tank are 0.6MPa and 0.4MPa, respectively.

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