00:01
Assuming the volume and the temperature are constant and we are not told otherwise, then the partial pressure can be calculated for carbon dioxide by taking the total pressure, 1 .05 atmospheres, and multiplying by the mole ratio, we've got five moles carbon dioxide for every 5 plus 3 plus 1 ,000, for a total of 9 moles.
00:32
Gas.
00:37
So the mole ratio for carbon dioxide multiplied by the total pressure gives us the partial pressure of carbon dioxide which is equal to 0 .58 atmospheres.
01:07
We can do a similar calculation with volumes if it is 30 % by volume helium, then at a total pressure of 4 .00 atm, 30 % expressed as a decimal number is 0 .30.
01:33
Then we're going to get 1 .20 atmospheres that are helium.
01:41
And then if it's 30 % helium, then that means it's got to be 70 % argon.
01:53
So 70 % as a decimal number is zero.
01:56
0 .70 and that gives us 2 .80 atmospheres argon.
02:05
For this next question we have a two bulb system and in one bulb or flask it's 4 liters and it contains nitrogen at 2 .0 atm and for the second flask it's 10 liters and it contains carbon monoxide at 1 .4 atm.
02:45
So although they don't give us a temperature, i find it helpful to assume a temperature and solve for an estimated moles of gas in each...