Dalton says: "The partial pressure of a (non-condensing) gas in the mixture is proportional to its concentration." Since your total pressure is 1000 mmHg and the volumes all total to 1000 mL, you don't even need to take your shoes off to do the math.
The nitrogen's volume is 780 ml of the total 1000 ml so its partial pressure is 780 mmHg of the total 1000 mmHg.
The pressure is 103,5 at.
In a sample of air, an increase in temperature will result in an increase in the partial pressure of oxygen.
781ml of N2 and 209ml of O2
300. mL
419 mL
The pressure is 103,5 at.
In a sample of air, an increase in temperature will result in an increase in the partial pressure of oxygen.
23
Use a sample of pyrogallol (C6H6O6) in the sample followed by a combustion reaction. This compound absorbs oxygen present.
It would be freely mixed, so yes.
747 mmHg
it decreases
1100
1100
The mass of the elements that are not oxygen equals 194.8g. The mass of oxygen is 230g - 194.8g = 35.2g of oxygen. Mass percent of oxygen = 35.2g O/230g x 100 = 15% O
1300<--- torr
150 (50 x 3)