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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.
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.
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
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.
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.
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.
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.
If the volume of a cylinder is reduced from 8.0 liters to 4.0 liters the pressure of the gas in the cylinder will change from 70 kilopascals to what?
Assuming the temperature remains constant, we can use Boyle's Law which states that pressure and volume are inversely proportional at constant temperature. If the volume is halved from 8.0 liters to 4.0 liters, the pressure will double from 70 kilopascals to 140 kilopascals.
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.
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
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.
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.
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.
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?
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A metal cylinder contains 1 mol of nitrogen gas what will happen to the pressure if another mole of gas is added to the cylinder but the temperature and volume do not change?
The addition of another mole of gas will double the number of gas molecules in the cylinder, leading to a doubling of the pressure according to Avogadro's law, which states that at constant temperature and volume, the pressure of an ideal gas is directly proportional to the number of moles of gas present.
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.
