0.21 mol
Universal Gas Law: P*V/T = a constant, where P = gas pressure [Pa], V = volume [m3], and T = gas temperature [K]. Therefore, when the gas temperature increases, the pressure increases linearly with it, when the volume is constant.
Increasing the temperature of a gas will increase it's pressure ONLY if the volume is held constant.
The universal gas equation is PV = nRT (Pressure x Volume = Number of moles x Universal Gas Constant x Temperature in Kelvin/Rankin). So - if Pressure is constant, the number of moles is constant, but the temperature increases from 25C (298 K) to 125C (398K) - a 34% increase, a similar 34% increase in volume will occur.
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.
as the pressure decreases the volume of gas increases at constant temperature
The Universal Gas constant can be used to relate the volume, temperature, pressure, and quantity of a gass to each other. The relationship is PV=nRT, or the pressure times the volume equals the number of moles times the universal gass constant times the temperature.
The volume is constant. The pressure will increase.The volume is constant. The pressure will increase.
Boyles law is Pv= k and refers to any mass of gas under observation. It is often stated as p1V1 = p2V2 In words :- the product of pressure and volume remain the same (constant) as you change pressure or volume in your experiment. The constant k in the equation is not a universal constant (like R the universal gas constant) just a constant for that particular experiment.
Universal Gas Law: P*V/T = a constant, where P = gas pressure [Pa], V = volume [m3], and T = gas temperature [K]. Therefore, when the gas temperature increases, the pressure increases linearly with it, when the volume is constant.
One is for constant pressure, the other is for constant volume. These are not the same; for example, if the pressure is maintained constant, and the gas is heated, the volume changes.
Increasing the temperature of a gas will increase it's pressure ONLY if the volume is held constant.
From the Universal Gas Law: PV/T = a constant, where P = gas pressure, V = gas volume, and T = gas temperature. I would say the two factors that determine volume are pressure and temperature.
At constant temperature p.V=constant, so pressure INcreases when decreasing the volume.
The universal gas equation is PV = nRT (Pressure x Volume = Number of moles x Universal Gas Constant x Temperature in Kelvin/Rankin). So - if Pressure is constant, the number of moles is constant, but the temperature increases from 25C (298 K) to 125C (398K) - a 34% increase, a similar 34% increase in volume will occur.
Volume & pressure are inversely proportionate, if temperature stays constant volume would decrease at a factor proporionate to the increase in pressure.
At constant temperature, the product of pressure and volume is a constant, or pressure is inversely proportional to volume, is known as Boyle's Law.
You can't compare pressure with volume. Presumably, somebody was talking about something being greater AT constant pressure, compared to constant volume.