Assuming ideal behavior, how many grams of acetylene are in the tank?
A. 4.33 g
B. 6.01 g
C. 113 g
D. 1650 g
2007-08-27 04:44:52 · 5 answers · asked by william b 2 in Science & Mathematics ➔ Chemistry
OK, ideal behaviour, so get out your ideal gas law:
PV = nRT
You have pressure in atmospheres, so make sure you use the right R constant, in this case 0.08206 atm L mol-1 K-1.
Convert temperature to Kelvin. Add 273 + 20 = 293 K
Plug in the numbers: 1.39*75 = n (0.08206)*293
n = 4.33
That's moles acetylene. Molecular weight of acetylene is 26 (2x12 + 2x1). Multiply moles by molecular weight to get 113 g acetylene.
2007-08-27 05:00:06 · answer #1 · answered by balibfe 2 · 0⤊ 0⤋
Use the ideal gas equation PV=nRT
P = 1.39 atm
V = 75.0L
T = 20 C = 293 K
R = .082
n = moles. Since C2H2 has a molecular mass of 26 g / mol you can substitute n with grams / mol mass.
You have all the data. Now just solve for grams
2007-08-27 04:56:24 · answer #2 · answered by reb1240 7 · 1⤊ 0⤋
The PV =NrT formula will give you the answer but not the warning. At ~ 30 psi. Acetylene gas will detonate in a tank. That is why it is adsorbed in acetone and diatomaceous earth in tanks. Acetylene is anything but an ideal gas.
2007-08-27 06:03:40 · answer #3 · answered by Brian T 6 · 1⤊ 0⤋
This is approximate. I can't remember the exact figure in the first part.
I mol of gas at stp occupies ~23L(gas irrelevant)
stp is 1 atm at 20C.
gmw of C2H2 is 26, so 26g C2H2 occupies 23L at 20C at 1 atm.
We have 75L at 1.39atm so grams =
26 * 75/23 * 1.39 = 117 approx
Nearest figure given is 113g so I'd say that is the answer.
2007-08-27 05:03:37 · answer #4 · answered by RobRoy 3 · 1⤊ 0⤋
Since you didn't provide us some useful info, all I can provide is a formula
mass = (Volume*Pressure)/(Gas Constant * Temperature)
2007-08-27 04:52:04 · answer #5 · answered by civil_av8r 7 · 1⤊ 1⤋