The gases in a mixture have the following partial pressures at the same volume and temperature 1013000 Pa nitrogen 700 mmHg argon 1.20 ATM of helium 790 torr oxygen and 0.50 ATM of carbon dio?

Answer 1

Convert all the pressures into one unit and then, using Dalton's Law of Partial Pressure, you just add all the pressures together.

Using these conversions(101325Pa equals 1 ATM, 1 ATM equals 760 mmHg, 1 mmHg equals 1 torr), calculate each pressure into one unit(I used mmHg)

1013000 Pa nitrogen equals 7598 mmHg of nitrogen(make sure you round using sig figs)

700 mmHg of argon equals 700 mmHg of argon

1.20 ATM of helium equals 912 mmHg of helium

790 torr oxygen equals 790 mmHg of oxygen

0.50 ATM of carbon dioxide equals 380 mmHg of Carbon Dioxide

Now add all the pressures and you get:

7598+700+912+790+380= 10380 mmHg

If you need to have the answer in a particular unit:

10380 mmHg

= 10380 torr

= 13.66 ATM

= 1384000 Pa

= 1,384 kPa

Answer 2

carbon dioxide

oxygen

nitrogen

argon

helium

from smallest mole fraction to

largest mole fraction

4.24 apexx

Answer 3

5.3

Answer 4

13.7