A mixture contains 220 mmHg of CO, 350 mmHg of Ne and 840 mmHg of He. What is the total pressure of the mixture

a
1.86 at
b
1.59 atm

c
1.46 atm

d
none of these

Answers

Answer 1

Considering the Dalton's partial pressure, the correct answer is option a.: the total pressure of the mixture is 1.86 atm.

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:

[tex]P_{T} =P_{1} +P_{2} +...+P_{n}[/tex]

where n is the amount of gases present in the sample.

This relationship is due to the assumption that there are no attractive forces between the gases.

In this case, a mixture contains 220 mmHg of CO, 350 mmHg of Ne and 840 mmHg of He. The total pressure of the mixture can be calculated as:

[tex]P_{T} =P_{CO} +P_{Ne} +P_{He}[/tex]

[tex]P_{T} =220 mmHg +350 mmHg+840 mmHg[/tex]

Solving:

[tex]P_{T}[/tex]= 1410 mmHg

Being 760 mmHg=1 atm, then:

[tex]P_{T}=1410 mmHgx\frac{1 atm}{760 mmHg}[/tex]

Solving:

[tex]P_{T}[/tex]= 1.86 atm

Finally, the correct answer is option a.: the total pressure of the mixture is 1.86 atm.

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