Primarygun Posted August 25, 2004 Share Posted August 25, 2004 PV=RnT And Volume is inversely proportional to pressure. Volume and pressure are both proportional to temperature. What I am confused of is, when T is increased, Which volume or pressure is increased? How to make the pressure remains constant in order to test the relationship between volume and temperature? Also, Increase in pressure would increase the speed of molecules, and aren't them moving faster and make the volume increase? Link to comment Share on other sites More sharing options...
swansont Posted August 25, 2004 Share Posted August 25, 2004 PV=RnTAnd Volume is inversely proportional to pressure. Volume and pressure are both proportional to temperature. What I am confused of is' date=' when T is increased, Which volume or pressure is increased? How to make the pressure remains constant in order to test the relationship between volume and temperature? Also, Increase in pressure would increase the speed of molecules, and aren't them moving faster and make the volume increase?[/quote'] You hold one of them constant - if both are allowed to vary, there are an infinite number of solutions. You could make pressure a constant in a piston - if the force exerted is constant with constant area, P stays the same but the volume can change. The volume won't increase in a sufficiently rigid container. Link to comment Share on other sites More sharing options...
pulkit Posted August 25, 2004 Share Posted August 25, 2004 You must however keep in mind that real gases have much more complex relations than the ideal gas law, so all you would observe that is explained by the ideal gas law is that on increasing temperature, volume increases at constant pressure. The ideal gas law is most valid near about the boyle temperature of the gas. Link to comment Share on other sites More sharing options...
Primarygun Posted August 26, 2004 Author Share Posted August 26, 2004 All gases are 22.4 L for 1 atm , 273 K of 1 mol What would you choose the environment for counting the mol of gases? Link to comment Share on other sites More sharing options...
pulkit Posted August 26, 2004 Share Posted August 26, 2004 All gases are 22.4 L for 1 atm , 273 K of 1 mol True only for ideal gases (and remember there exsist none) What would you choose the environment for counting the mol of gases? Cylinder with a constant pressure of 1atm maintained using a piston, and a large heat source to maintain temperature at 273K (the heat source merely ensures no temperature change). Link to comment Share on other sites More sharing options...
Primarygun Posted August 27, 2004 Author Share Posted August 27, 2004 maintain temperature at 273K Why not use higher temperature? Does the volume of it increase and provide a better ideal gases environment? Link to comment Share on other sites More sharing options...
pulkit Posted August 27, 2004 Share Posted August 27, 2004 Why not use higher temperature? I was just giving an example. If all you wish to do is measure the number of mols, the easiest way would be to just weight the gas. Link to comment Share on other sites More sharing options...
wolfson Posted August 27, 2004 Share Posted August 27, 2004 If all you wish to do is measure the number of mols, the easiest way would be to just weight the gas. weight the gas = calculate the volume. The higher the temperature the faster molecules are moving. Faster the molecules = higher the pressure, as are moving, the harder they hit the wall of the container. It's all kinetic theory/motion. Link to comment Share on other sites More sharing options...
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