A mixture of gases contains 0.75 mol N2, 0.30 mol O2, and 0.15 mol CO2. If the total pressure of the mixture is 1.56 atm, what is the partial pressure of each component?
2007-12-06 01:16:22 · 4 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
You can multiply the total pressure by the proportion of each gas in the mixture (the mole fraction).
So, you have a total number of moles of gas of 0.75 +0.30+0.15 = 1.2 moles. The mole fraction of nitrogen is 0.75/1.20 = 0.625.
If you multiply the total pressure (1.56) by the mole fraction of nitrogen (0.625) you have the partial pressure of nitrogen in the mixture.
Do the same thing for oxygen and CO2.
2007-12-06 01:27:19 · answer #1 · answered by hcbiochem 7 · 17⤊ 1⤋
Partial Pressure
2016-12-11 12:08:22 · answer #2 · answered by moncalieri 4 · 0⤊ 0⤋
How To Find Partial Pressure
2016-09-29 05:40:58 · answer #3 · answered by ? 4 · 0⤊ 0⤋
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How do you find the partial pressure?
A mixture of gases contains 0.75 mol N2, 0.30 mol O2, and 0.15 mol CO2. If the total pressure of the mixture is 1.56 atm, what is the partial pressure of each component?
2015-08-07 05:05:10 · answer #4 · answered by Anonymous · 0⤊ 2⤋
write down the ratio of moles
0.75 : 0.3 : 0.15
add them up
0.75 + 0.3 + 0.15 = 1.2
work out what fraction of the mixture is what.
0.75/1.2 = 0.625 N2
0.3/1.2 = 0.25 O2
0.15/1.2 = 0.125 CO2
multiply each respective component decimal by the total pressure
0.625 * 1.56 = 0.975 atm N2
0.25 * 1.56 = 0.39 atm O2
0.125 * 1.56 = 0.195 atm CO2
2007-12-06 01:27:52 · answer #5 · answered by mountainpenguin 4 · 18⤊ 1⤋
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2015-08-04 09:00:37 · answer #6 · answered by ? 1 · 0⤊ 1⤋