The combined gas law say PV/T=k. 1.3*18/300=k=V*24/340 V=1.3*18*340/(300*24)=11.05 litres
1 mole of gas at STP occupies 22.4 liters.
13500 litres of water weights approx 132.3 newtons.
meters, seconds, meters/second, liters, newtons
Density = 10 kg / 5 litres = 2 kg per litre.
If the volume is reduced, and all else remains the same, then the pressure will increase by a factor of 2, or it will double.
pressure = .490 atm
Assuming standard temperature and pressure: 1 mole (64.1 g) of SO2 occupies 22.4 liters 72.0 g SO2 occupies (72.0/64.1) x 22.4 liters
This is the molar volume of an ideal gas at a given temperature and 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.
5.3 liters
contains the same number of molecules
The answer is 1,83 moles.
1 mole occupies 22.4 liters. 0.5 moles occupies 11.2 liters at STP.
1 mole (or 4 g of He) occupies 22.414 liters. So, 2.3 mole occupies 2.3 x 22.414 liters = 51.5522 liters
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.
At STP, 1 mol or 6.02x10^23 representative particles, of any gas occupies a volume of 22.4 Liters. (chemistry)
1 mole occupies 22.414 liters So, 1.84 moles will occupy 41.242 liters