A 10.0 L container of helium gas with a pressure of 230 torr at 0 celsius is heated to give a pressure of 1600 torr . What is the new temperature in degrees Celsius?
i converted torr into atm and got .3026 and 2.105 i diveded those two and got .143 times 273 = 39.2 K = -233...but what do i do with the 10.0 L....im stuck
2007-04-19 20:26:22 · 4 answers · asked by orange_crush_05 6 in Science & Mathematics ➔ Chemistry
The volume is irrelevant.
When you heat a vessel, the pressure goes up, and vice versa.
Try (1600/230) x 273.
2007-04-19 20:33:30 · answer #1 · answered by Gervald F 7 · 0⤊ 0⤋
The three relationships of calculating the properties of a gas is between pressure temperature and volume.
As the container volume stays the same you can ignore it.
The gas law states the P is proportional to temperature. So we can use the equation
P1/ T1 = P2 / T2.
As we are after the final temperature, rearrange the equation for T2.
T2 =P2*T1/P1
= 1600*(0+273)/230
=1899°K
=1626°C
There is no need to change the units of pressure (Torr) as they will cancel out in the equation.
Email me if you need an further help or clarification
2007-04-20 03:47:31 · answer #2 · answered by ktrna69 6 · 0⤊ 0⤋
shouldn't it be 1600/230 instead of the reverse?
I don't think volume matters in this case.
2007-04-20 03:30:46 · answer #3 · answered by DeadmanWalks 3 · 0⤊ 0⤋
Well i am 83yrs so i may be wrong, isint the 10lt, purely a container , if so it has no relevance only in the fact that it was and is a container.
2007-04-20 03:33:49 · answer #4 · answered by Blazing a trail 2 · 0⤊ 0⤋