If the volume is fixed, then doubling the absolute temperature will double the pressure.
At 0° C, the absolute temperature is 273 K. Heat the gas to 273° C = 546 K.
Double quantity of gas in the same volume,
or
compression to half volume for the same quantity of gas.
ALL at the same temperature! of course.
Charles Law states that V = Tk, where k is a constant. So with an ideal gas where k stays the same, for V to double, T must double as well.
Using the Celsius temperature scale, it is not correct. But doubling the temperature using the Kelvin temperature scale, where zero is the absolute minimum gegree possible, will double pressure . p1/T1=p2/T2=constant.
Gases Boyle's law states that the Volume of a given amount of gas at constant Temperature varies inversely proportional to Pressure. You have a given volume of gas, and you double its pressure keeping Temperature constant, the volume will reduce by half.
Charles's law states that at constant pressure, the volume of a given mass of an ideal gas increases or decreases by the same factor as its absolute temperature. For fixed mass of an Ideal Gas at constant pressure the volume it occupies is directly proportional to its absolute temperature. So, if you double the absolute temperature of a gas while holding its pressure constant, the volume has to double. There is no such thing as an Ideal Gas. So, doubling the temperature of a real gas will not exactly double its volume. However, the general principle hold true. If you increase the temperature of any gas at constant pressure the volume it occupies will increase.
For the pressure to remain the same, the temperature would double if the volume also doubled.
When pressure double, the volume halves. However this is only true if the number of molecules and the temperature are both in a constant state.
Are you stating or asking ? If that's a statement, then it's an incorrect one. At constant temperature, the product of (pressure) x (volume) is constant. So, if the volume changed by a factor of 3, the pressure must also change by a factor of 3 ... the pressure must triple.
Using the Celsius temperature scale, it is not correct. But doubling the temperature using the Kelvin temperature scale, where zero is the absolute minimum gegree possible, will double pressure . p1/T1=p2/T2=constant.
pV = nRT we can firstly assume that n (number of moles) and R (gas constant) do not change and as pressure is also kept constant, the temperature must be proportional to the volume. Thus if temperature is increased from 27C (300K) to 327C (600K) and is doubled, the volume must also double.
Gases Boyle's law states that the Volume of a given amount of gas at constant Temperature varies inversely proportional to Pressure. You have a given volume of gas, and you double its pressure keeping Temperature constant, the volume will reduce by half.
For the pressure to remain the same, the temperature would double if the volume also doubled.
Charles's law states that at constant pressure, the volume of a given mass of an ideal gas increases or decreases by the same factor as its absolute temperature. For fixed mass of an Ideal Gas at constant pressure the volume it occupies is directly proportional to its absolute temperature. So, if you double the absolute temperature of a gas while holding its pressure constant, the volume has to double. There is no such thing as an Ideal Gas. So, doubling the temperature of a real gas will not exactly double its volume. However, the general principle hold true. If you increase the temperature of any gas at constant pressure the volume it occupies will increase.
When pressure double, the volume halves. However this is only true if the number of molecules and the temperature are both in a constant state.
assuming the balloon is closed, the air pressure would double
The initial pressure is halved. Use Boyle's law that relates pressure & volume at a constant temperature. P1V1 = P2V2 In this case the V1(initial volume) is doubled so V2 = 2V1 P2 = P1V1/V2 = P1V1/2V1 P2 = (1/2)*P1
If the volume of a container of air is reduced by one half the partial pressure of the oxygen with in the container will be doubled. If the volume of a container of gas is reduced, the pressure inside the container will increase.
Pressure is halved when ONLY volume is doubled (n and T are constant).Remember the General Gas Law:p.V = n.R.T(in which R=general gas constant)
There are three variables in gas work that go into volume: amount of gas, pressure of gas, temperature of gas. If we double the amount of gas - the moles - and maintain the temperature and pressure, the volume must double.