If something takes up space, it must have a mass.
To find it's density
vapor density =density of gas/density of hydrogen gas=mass of a certain vol. of gas/mass of same vol. of hydrogen gas=mass of n molecules of gas/mass of n molecules of hydrogen gas=mass of 1 molecule of gas/mass of 1 molecule of hydrogen gas=molecular mass of gas/molecular mass of hydrogen gas=molecular mass/22 x vapor density=molecular mass
sure. we know that the molarity of gas in a constant temperature and pressure (exp, room temperature, 25 celcius, 1 atm) will have a constant volume. in 25'c, 1 atm, the volume of one mole of gas is 24.5 L. so that if we know the volume of the gas, we can divide it by 24.5, such that we can determine the molarity of that gas. and molarity times molar mass will equal to the mass of a type of gas. calculation : given a known volume V at 25'c , 1atm no of mole of gas = v / 24.5 = q mole of gas. mass of gas = q(no of mole of gas) x Mr(molecular mass of that type of gas) *assumption : it is a pure gas (contain the same type of gas), and we also know the type of gas we are testing( so that we know the molecular mass of that gas) method 2: 1) weight the mass of a balloon(p). 2) pump the gas/ gasses into the balloon, weight the mass of the balloon +gasses(q). 3) p-q = weight of the gasses * disadvantages : we cannot define the mixture of gasses inside the balloon. * since we got analytic chemistry, we can put the gasses into a nuclear magnetic resonance spectorscopy and analyse the substance inside the balloon because of chemial shift.
To calculate the density of a gas, we need to know the molar mass and the pressure and temperature conditions. Without this information, we cannot determine the density of the gas.
There is no such noble gas with an atomic mass of 30. The mass of neon is 20 and the mass of the next noble gas, argon, is 40
To find it's density
vapor density =density of gas/density of hydrogen gas=mass of a certain vol. of gas/mass of same vol. of hydrogen gas=mass of n molecules of gas/mass of n molecules of hydrogen gas=mass of 1 molecule of gas/mass of 1 molecule of hydrogen gas=molecular mass of gas/molecular mass of hydrogen gas=molecular mass/22 x vapor density=molecular mass
sure. we know that the molarity of gas in a constant temperature and pressure (exp, room temperature, 25 celcius, 1 atm) will have a constant volume. in 25'c, 1 atm, the volume of one mole of gas is 24.5 L. so that if we know the volume of the gas, we can divide it by 24.5, such that we can determine the molarity of that gas. and molarity times molar mass will equal to the mass of a type of gas. calculation : given a known volume V at 25'c , 1atm no of mole of gas = v / 24.5 = q mole of gas. mass of gas = q(no of mole of gas) x Mr(molecular mass of that type of gas) *assumption : it is a pure gas (contain the same type of gas), and we also know the type of gas we are testing( so that we know the molecular mass of that gas) method 2: 1) weight the mass of a balloon(p). 2) pump the gas/ gasses into the balloon, weight the mass of the balloon +gasses(q). 3) p-q = weight of the gasses * disadvantages : we cannot define the mixture of gasses inside the balloon. * since we got analytic chemistry, we can put the gasses into a nuclear magnetic resonance spectorscopy and analyse the substance inside the balloon because of chemial shift.
Area of the container and the mass of the gas or liquid inside.
To calculate the density of a gas, we need to know the molar mass and the pressure and temperature conditions. Without this information, we cannot determine the density of the gas.
Yes. Gas Mass = sum of gas atoms= n(gas atoms).
The ideal gas law does not hold that gasses are massless. Gas does indeed have mass. Saturn has a mass of about 5.68*1026 kilograms.
Trapping the gas and measuring its mass...
There is no such noble gas with an atomic mass of 30. The mass of neon is 20 and the mass of the next noble gas, argon, is 40
Fluorine is a gas with a mass number 19.
No. Heat doesn't change the mass of a gas.
The speed of the molecules in a gas is proportional to the temperature and is inversely proportional to molar mass of the gas.