A 500.0 g sample of aluminium, I initially at 25.0 degrees, absorbs heat from its surroundings and reaches a final temperature o
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Considering the Dalton's partial pressure, the mole fraction of each gas is:
= 0.14
= 0.76
= 0.10
The pressure exerted by a particular gas in a mixture is known as its partial pressure.
So, Dalton's law states that the total pressure of a gas mixture is equal to the sum of the pressures that each gas would exert if it were alone:
where n is the amount of gases in the gas mixture.
This relationship is due to the assumption that there are no attractive forces between the gases.
Dalton's partial pressure law can also be expressed in terms of the mole fraction of the gas in the mixture. The mole fraction is a dimensionless quantity that expresses the ratio of the number of moles of a component to the number of moles of all the components present.
So in a mixture of two or more gases, the partial pressure of gas A can be expressed as:
In summary, the total pressure in a mixture of gases is equal to the sum of partial pressures of each gas.
Mole fraction of each gas
In this case, you know that:
= 1.25 atm
= 6.73 atm
= 0.895 atm
= 1.25 atm + 6.73 atm + 0.895 atm= 8.875 atm
Then:
Substituting the corresponding values:
- 1.25 atm=
- 6.73 atm=
- 0.895 atm=
Solving:
In summary, the mole fraction of each gas is:
Learn more about Dalton's partial pressure:
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