As we will be using the Ideal Gas Law it doesn't matter what gas we are using.
PV=nRT
P= 1 atm
n=2.1
T=273.15K
R=0.0821 atm liters3/mole K
V= 47.1 L3
The volume of one mole of gas at a standard temperature and pressure is 22.4 liters. Multiply 22.4 liters by 0.25 moles to get a volume of 5.6 liters.
smalles volume element
STP means standard temperature and pressure and VTP means volume temperature and pressure oh and btw standard temperature and pressure is 0 degrees Celsius and 1 atmosphere
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.
Molar gas volume is the volume of ONE moel of gas. It only depends on the pressure and temperature, not on the kind of gas. Molar volume at standard temperature and standard pressure is always 22,4 Litres (for any gas)
54 liters at STP (standard temperature and pressure)
The mass of the Chlorine will depend upon the density of the Chlorine which depends upon the temperature and pressure of the Chlorine. Assuming stp (standard temperature and pressure) the density of Chlorine is 0.0032 g/ml. density = mass / volume → mass = volume × density = 100 ml × 0.0032 g/ml = 0.32 g.
The volume of one mole of gas at a standard temperature and pressure is 22.4 liters. Multiply 22.4 liters by 0.25 moles to get a volume of 5.6 liters.
Gross volume is the volume at actual condition whereas standard volume is at standard Pressure/Temperature condition.
smalles volume element
STP means standard temperature and pressure and VTP means volume temperature and pressure oh and btw standard temperature and pressure is 0 degrees Celsius and 1 atmosphere
Chlorine is a gas. Its density depends on pressure, temperature and volume of the container.
One kilogram of pure water at standard temperature and pressure has a volume of 1 liter. So if your temperature and pressure are standard and your water is pure, then the volume of 100.0 kilograms of it is 100.0 liters.
I would assume chlorine gas and standard temperature an atmospheric pressure. Using the ideal gas equation. PV = nRT (1 atm)(X volume) = (2.4 moles Cl2)(0.08206 Mol*K/L*atm)(298.15 K) Volume = 59 Liters of chlorine gas --------------------------------------------
At STP, 1 mole of gas occupies a volume of 22.4 liters. Thus, 4/5 moles of gas will occupy .8*22.4 liters.
STP = Standard Temperature and Pressure After the IUPAC rules the standard temperature is 0 0C and the standard pressure is 100 kPa (0,986 atm). The molar volume of an ideal gas at STP is 22,710 980(38) L.
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.