P1V1/T1 = P2V2/T2
Change all temps to Kelvin. ( 38 C + 273.15 = 311.15 K and 25 C = 298.15 K )
(1 atm)(20 L)/(298.15 K) = (20 atm)(X L)/(311.15 K)
5963X = 6223
X = 1.0 Liters
===========
you need to know the density of the gas (and temperature and pressure)
Pressure and temperature. As pressure increases, volume decreases; as temperature increases, volume increases with it. At standard temperature and pressure (1 atm, 273 degrees Kelvin), one mole of a gas (6.022 x 1023 particles) has the volume of 22.4 liters.
For this you would use Boyle's Law, P1V1 = P2V2. The first pressure and volume variables are before the change, while the second set are after the change. In this case, the volume is being changed and the pressure has to be solved for. P1 = 1.00 ATM V1 = 2.0 L P2 = Unknown V2 = 4.00 L P1V1 = P2V2 1.00(2.0)=4.00P P= .5 ATM
STP stands for Standard Temperature and Pressure. At STP, the pressure of natural gas is 1 atm, and 1 mole of gas takes up 22.4 liters.
1 liter of water weight about 1 kilo. (The exact weight depends on the pressure and temperature). Therefore the container above holds 3.2 liters.
You don't. Liters is a unit of volume, atmospheres is a unit of pressure.
The answer is 13,89 moles.
atmospheres
The pressure is 2,02 atmospheres.
pressure -- Torr which is equivalent to mmHg, Pascals or kPa, atmospheres, psi, inches Hg Volume -- usually liters Temperature -- Kelvin or Celsius which must be converted to Kelvin to be used in any gas law equations
That is the element potassium at STANDARD TEMPERATURE AND PRESSURE. Standard temperature is 273 K and standard pressure is 1 atm.
Use Boyle's Law, applicable for ideal gases at constant temperature, to solve this problem: P1*V1 = P2*V2
Pressure, volume and temperature, and moles of gas are the four principal variables to describe a gas (for example, see related questions on Ideal Gas Law and others). The standard units are: Pressure: atmospheres (atm) Volume: liters (L) Temperature: Kelvin (K) Number of moles are measure in, well, moles.
- by the variation of the temperature- by the variation of the pressure
It means there are 22.4 liters of an "ideal" gas at STP (standard temperature and pressure), implying that temperature = 273.15 K and pressure = 1 atm.
This problem can be solved with the ideal gas law. The original pressure and volume of the container are proportional the final pressure and volume of the container. The original pressure was 1 atmosphere and the original volume was 1 liter. If the final volume is 1.8 liters, then the final pressure is 0.55 atmospheres.
54 liters at STP (standard temperature and pressure)