n = 56 g/ (18.0 g/mole) = 3.11 moles water.
P = (108 kPa) / (101.325 kPa/ATM) = 1.065877 ATM
R = universal gas constant = 0.0820574587L · ATM · K-1 · mol-1
V = nRT/P = (3.11 mol) * (0.082057L · ATM · K-1 · mol-1) * (274 K) / 1.06588 ATM
= 65. 6 L
Note: a mole of water vapor (H2O) is 18.0 grams, since it has an molar mass of 18. Oxygen has a molar mass of 16.0, and the two hydrogen atoms each have a molar mass of 1.0.
54 liters at STP (standard temperature and pressure)
pressure / temperature / volume /enthalpy
Using the equation P1V1/T1 = P2V2/T2 we find there are two variables we might influence in order to change the pressure of a gas. (P=pressure, V=volume, T=temperature in degrees Kelvin) By increasing or decreasing the temperature of the bottle, you can increase or decrease the pressure within. If the bottle is made of a flexible material, like plastic, you can apply pressure to the bottle. By either squeezing the bottle or increasing atmospheric pressure outside, you deform the bottle and decrease it's volume. Since the quantity of gas inside the bottle is constant, the decrease in volume increases the pressure. Likewise to decrease the pressure in a sealed flexible bottle, you can decrease air pressure outside.
The lowest temperature is known as absolute zero which is equal to 0K (0 Kelvin) and -273.15 Celsius (-459.67F). Absolute zero has never been recorded but is the theoretical temperature of which no heat can be extracted from a system. It is theoretical because at 0K matter would have no pressure and therefore no volume.
Charle's law of gases say that when pressure and amount of gas remains the same, the volume is directly proportional to the temperature. So the higher the temperature, the larger the volume of the gas A more complete gas law, utilizing other gas laws as well, is the Ideal Gas Equation. It is written as PV = nRT where P is the pressure (usually in ATM) V is the volume (in Liters) n is the moles (amount) of gas R is the gas constant for the units in P , V, and T T is the temperature (usually in Kelvin)
Just convert all the temperatures to Kelvin (add 273 to the Celsius temperature). The volume is directly proportional to the absolute (Kelvin) temperature.
if kelvin temp is halved, the volume is halved if pressure is constant.
Because kelvin temperature has a simple relationship with volume, according to Charles's' law if the kelvin temperature becomes doubled at constant pressure the volume of the gas also becomes doubled, this relation is not with Celsius or Fahrenheit temperature.
The pressure is decreased to 50 %.
Charles' Law says that as pressure on a gas decreases, its volume increases. Charles' Law is an example of an inverse relationship.t It is not Charle's law It is Boyle's law Charles law states at constant volume, pressure is proportional to kelvin temperature And at constant pressure volume is proportional to kelvin temperature But Boyle's law states that at constant temperature pressure is inversely related to volume
Charles' Law says that as pressure on a gas decreases, its volume increases. Charles' Law is an example of an inverse relationship.t It is not Charle's law It is Boyle's law Charles law states at constant volume, pressure is proportional to kelvin temperature And at constant pressure volume is proportional to kelvin temperature But Boyle's law states that at constant temperature pressure is inversely related to volume
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.
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.
3.5 litre if pressure is kept constant.
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
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.
Increased temperature = increased volume of gas The above answer is non-sense. The pressure could increase with temperature and actually yield a smaller volume... here ya go: The ideal gas law is: PV = nRT, where P = pressure, V = volume, n= number of moles, R = ideal gas constant, T = Temperature in K