A tank contains both nitrogen and hydrogen gas. If the partial pressures are 190mmHg and 303mmHg respectively, what is the mole fraction of nitrogen gas?
a. 0.875
b. 0.625
c. 0.547
d. 0.250
e. 0.385
2006-12-14 02:01:07 · 5 answers · asked by bosox1989 1 in Science & Mathematics ➔ Chemistry
Total pressure=303+190 mm of Hg
=493 mm of Hg.
Mole Fraction of Nitrogen gas= Partial pressur of N2 gas/total pressure
=190/493
=0.385
Hence correct option is e
2006-12-14 02:09:56 · answer #1 · answered by Som™ 6 · 0⤊ 0⤋
Hello!
Pn = partial pressure of nitrogen
Ph = partical pressure of hydrogen
Pt = total pressure
Basic formula: Pp = X*Pt; the partial pressure of a gas is the mole fraction of the gas multiplied by the total pressure.
* Pp = partial pressure of a certain gas
* X = mole fraction of a certain gas
In this problem, we're trying to solve for the mole fraction of nitrogen gas. Let's rearrange the formula and plug in a new variable.
1) Pn = Xn * Pt [Nothing really happened here. We just plugged in two modified variables saying that the partial pressure of nitrogen gas is equal to the mole fraction of nitrogen multiply by the total pressure]
2) Xn = Pn / Pt [Just a little rearrangement. We are trying to solve for the mole fraction of nitrogen gas, right? ^_^]
What is Pt (the total pressure)?
Basic formula: Pt = P1 + P2 + P3...
In this case...
Pt = Pn + Ph
Pt = 190mmHg + 303mmHg
Pt = 493mmHg
Let's solve for the mole fraction of nitrogen gas...
Xn = Pn / Pt
Xn = 190mmHg / 493mmHg
Xn = 0.385
^_^ sorry my answer is so much wordier than the others. Hope you understand it. Good luck.
2006-12-14 22:19:49 · answer #2 · answered by Cinna B 2 · 0⤊ 0⤋
total pressure =190+303=493 mmHg
mole fraction of nitrogen=partialpressureN2/total pressure
hence,
mole fraction of nitrogen=190/493=.385
hence .385 is the answer
2006-12-14 10:09:43 · answer #3 · answered by skr 2 · 0⤊ 0⤋
e. 0.385
2006-12-14 14:35:45 · answer #4 · answered by Anonymous · 0⤊ 0⤋
f. Do your own homework
2006-12-14 10:08:33 · answer #5 · answered by mattoneill 2 · 0⤊ 1⤋