2006-12-22 13:59:56 · 13 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
Neither - in PV = nRT - the volume is not a function of temperature - it is fixed - i.e there has to be a boundary around the gas without which V would be infinite in this equation.
So this applies when you know the volume - so the pressure increases with the temperature.
Now if the boundary was mutable then the pressure would remain fixed and the volume rise.
2006-12-22 14:09:17 · answer #1 · answered by Andy 2 · 0⤊ 0⤋
The gas law that you need to refer to to is Charles's Law.
For this law to be accurate, pressure must be kept constant.
V1/T1 = V2/T2, Where V is volume and T is temperature. This is saying that the volume of a gas increases with increasing temperature.
To understand this better, you also need to understand directly and indirectly proportional. Directly means that when one rises so does the other, when it decreases so does the other.
Indirectly means that when one rises the other variable decreases. Just as with one decreasing the other variable will increase.
To help you understand the answer to this question think of a hot air balloon. You heat the air (increasing temp)--What happens to the volume of the air?--It increases in volume to inflate the balloon.
2006-12-22 15:14:23 · answer #2 · answered by Chynthia S 2 · 0⤊ 0⤋
Charles Law states that V1/T1 = V2/T2 = constant which shows a direct proportionality. As the temperature goes up, the volume has to go up to preserve the constant. One of the really important things in this equation is that you have to use the temperature in Kelvins (K = C + 273) which is an absolute temperature scale in which 0 K is a theoretical point which we can never go below (no negative Kelvin temperatures). This means that a gas at 20 degrees Celsius would not double its volume at 40 degrees Celsius, otherwise a gas at 0 degrees Celsius would double its volume at................0 degrees Celsius! A gas at 0 degrees Celsius (273 K) would have to be heated to 273 degrees Celsius (546 K) to double its volume.
2006-12-22 15:55:05 · answer #3 · answered by kentucky 6 · 0⤊ 0⤋
PV = nrT So, as you will discover, the strain and quantity are inversely proportional to a minimum of one yet another, and the Temperature is proportional to the different 2. In different words, because of the fact the temperature is going up, the two the strain or the quantity would desire to boost. With the temperature consistent, in case you boost the strain, you decrease the quantity.
2016-12-15 06:31:19 · answer #4 · answered by ? 4 · 0⤊ 0⤋
Directly
When you add energy to the molecules they can travel a longer distance in the same amount of time (like going 50 mph vs. 60 mph). As long as they are in an expandable container (like a balloon) the volume will increase with increasing energy and decrease with decreasing energy.
(The "laws" are good but they don't EXPLAIN WHY; kinetic molecular theory explains why all those gas laws work)
2006-12-23 04:03:36 · answer #5 · answered by The Old Professor 5 · 0⤊ 0⤋
PV=nRT ideal gas law
pressure times volume equals number times constant times temperature
Volume is directly proportional to temperature.
2006-12-22 15:01:54 · answer #6 · answered by Pocket Rocket 2 · 0⤊ 0⤋
When the temperature rises, the volume rises hence they are directly proportional. Cheers.
2006-12-22 14:02:58 · answer #7 · answered by apollo 2 · 0⤊ 0⤋
PV=nRT
volume and temp are directly related
2006-12-22 14:05:01 · answer #8 · answered by Annie 2 · 1⤊ 1⤋
The greater the temp, the greater the volume.
2006-12-22 14:04:06 · answer #9 · answered by eric l 6 · 0⤊ 0⤋
It is actually Charles' Law.... V1T2 = V2T1... think of a helium balloon in the winter...
inside in the warmth, it is fully inflated, but take it outside into the cold and it withers. The gas inside condenses and slows down. Take it back into the warmth and it re-inflates...
2006-12-22 14:07:25 · answer #10 · answered by itutorchem 2 · 0⤊ 0⤋