The temperature of an ideal gas was held at 400degrees C. the initial pressure and volume were 750 torr and 500 ml respectively. What would the fina pressure be of the volume were increased to 1500ml?
Could someone explain please?
2006-06-16 01:47:08 · 5 answers · asked by Gatlas 3 in Science & Mathematics ➔ Mathematics
Ideal Gas Law: PV = nRT
You are holding n and T constant, and R is a constant, so:
P1V1 = P2V2
(750 torr)(500ml) = (x torr)(1500 ml)
x torr = (750 torr)*(500/1500) = 750 torr *1/3 = 250 torr
2006-06-16 03:34:19 · answer #1 · answered by Dave_Stark 7 · 3⤊ 0⤋
If you expand a gas while keeping its temperature the same, its pressure decreases in direct proportion to the expansion.
You have increased the volume by a factor of 3 (from 500 to 1500 ml) so the pressure will fall by a factor of 3 - from 750 torr to 250 torr.
2006-06-16 01:55:01 · answer #2 · answered by Epidavros 4 · 0⤊ 0⤋
for ideal gas PV=nRT
when T is constnat then we have P1V1= P2V2..
Hence Final Volume= P1V1/P2
= 750*500/ 1500 = 250 ml.
2006-06-16 02:05:39 · answer #3 · answered by Vivek 4 · 0⤊ 0⤋
(pV)begin = (pV)end
750 torr x 500 ml = p x 1500 ml
750 torr x 500 ml / 1500 ml = p
p = 250 torr
V x3 , then p /3
2006-06-16 11:28:35 · answer #4 · answered by Thermo 6 · 0⤊ 0⤋
no sorry
2006-06-16 01:51:37 · answer #5 · answered by paaulll20005 1 · 0⤊ 0⤋