At a temperature of 273 K, a 400.-milliliter gas sample has a pressure of one atm of mercury. If the pressure is changed to .5 atm of mercury, at which temperature will this gas sample have a volume of 551 milliliters?
1. 100 K
2. 188 K
3. 273 K
4. 546 K
2007-02-24 15:03:47 · 3 answers · asked by Calvino 1 in Science & Mathematics ➔ Chemistry
Since there is no addition or loss of gas:
pV = nRT
You can solve this for n and then find T for the changed conditions. If we did not change the volume, halving the pressure would halve the absolute temp. Since the new volume is somewhat higher (551 vs 400), the absolute temperature will be somewhat higher. Answer 2 looks best.
2007-02-24 15:09:53 · answer #1 · answered by cattbarf 7 · 0⤊ 0⤋
Just work it out with the ideal gas law PV=nRT, where P is the pressure, V is the volume, n is the number of moles, T is the temperature and R is the Univeral Gas Constant.
2007-02-24 23:10:14 · answer #2 · answered by billybob 2 · 0⤊ 0⤋
Ideal gas law, PV=nRT. n*R are constants. so modify this
P1*V1 / T1 = P2*V2/T2
P1 = 1 atm
V1 = 400 ml
T1 = 273
P2 = .5 atm
V2 = 551 ml
T2 = ?
2007-02-25 00:12:20 · answer #3 · answered by My name is not bruce 7 · 0⤊ 0⤋