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What happens to the volume of a gas when the number of moles is doubled?
The ideal Gas Law states the following: pV=nRT p=pressure [pa] V=volume [m³] n=number of moles R=constant T=temperature [K] So, if you multiply the number of moles by 2, and all the other variables are not changed, your volume will also be multiplied by 2.
What happens to pressure of constant mass of a gas at constant temperature when the volume is doubled?
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)
According to the ideal gas law what happens to the volume of a gas when the number of moles double and all else is 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.
Why if a gas is present at 27 Celsius its volume becomes doubled when temperature increases to 327 Celsius under constant pressure?
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.
Which law is described by saying that doubling the absolute temperature will double the pressure of a sample of gas in a rigid container?
The law described is Gay-Lussac's Law, which states that the pressure of a gas is directly proportional to its absolute temperature when the volume remains constant. Therefore, if the absolute temperature of a gas in a rigid container is doubled, the pressure will also double, assuming the amount of gas does not change. This relationship highlights the direct correlation between temperature and pressure in gas behavior.
When a sample of gas is compressed from 6.0 L to 2.0 L at a constant temperature the pressure of the gas double?
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.
What happens to the pressure of a confined gas at a constant temperature when the volume is reduced by half?
When the volume of a confined gas is reduced by half at a constant temperature, the pressure of the gas will double according to Boyle's Law. This is because the product of pressure and volume is constant for a given amount of gas at constant temperature. When the volume decreases, the pressure increases to maintain this equilibrium.
What happens to the pressure if the temperature in K is doubled?
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
What does Boyle's Law state?
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.
Does doubling celsius temperature double pressure?
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.
Which temperature change would cause the volume of a sample of an ideal gas to double when the pressure of the?
If the pressure of the ideal gas is kept constant and the volume is desired to double, the temperature must also double according to the ideal gas law: V2 = 2V1 = (2/1)×V1 when T2 = 2T1. This relationship results from the formula PV = nRT, where P is pressure, V is volume, n is the number of moles of gas, R is the ideal gas constant, and T is temperature.
Two cubic meters of a gas at 30 degrees Kelvin are heated at a constant pressure until the volume doubles. What is the final temperature of the gas?
60
What happens to the air pressure inside a balloon when it is squeezed to half its volume at constant temperature?
When a balloon is squeezed to half its volume at constant temperature, the air pressure inside the balloon increases. This is because the number of air molecules remains constant while the volume decreases, leading to the molecules being packed closer together and increasing the pressure.
What temperature change would cause a sample of an ideal gas to double in volume while the pressure was held constant?
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.
What happens to the volume of a gas when the number of moles is doubled?
The ideal Gas Law states the following: pV=nRT p=pressure [pa] V=volume [m³] n=number of moles R=constant T=temperature [K] So, if you multiply the number of moles by 2, and all the other variables are not changed, your volume will also be multiplied by 2.
Do Charles' law indicates that an increase in absolute temperature will cause a corresponding increase in volume?
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.
What happens to pressure of constant mass of a gas at constant temperature when the volume is doubled?
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)
