Question

How do you find the molar volume of hydrogen gas?

Answer 1

According to the law equal volumes of all gases at the same temperature and pressure contain equal numbers of particles.
A given volume of a gas with small light particles such as hydrogen $({{\text{H}}_{2}})$ contains the same number of particles.

Complete step by step answer:
The molar volume of a gas in the volume of one mole of a gas at STP.
At STP, one mole $(6.02\times {{10}^{23}}$ representative particles) of any gas occupies a volume of $2.4\text{L}$
At standard Temperature and pressure (STP) the molar volume $\text{(}{{\text{V}}_{\text{m}}}\text{)}$ is the volume occupied by one mole of a chemical compound.
The molar volume can be calculated by dividing molar mars by mass density.
Formula: Molar volume $({{\text{V}}_{m}})=\dfrac{\text{molar mass (M)}}{\text{Mass density (}\rho \text{)}}$
where, $\text{(}{{\text{V}}_{\text{m}}}\text{)}$ is the volume occupied by one mole of a chemical compound.
Or
According to Avogadro Law
$\text{Volume }\propto \text{Number of particles}$
by substituting the terms in symbols:
V$\propto$ n
The molar volume of ${{\text{H}}_{2}}$gas is calculated by one experiment in which reaction of link in solid form reacts with Hydrogen Chloride in anguish medium.
$\text{Zn(s) }+\text{2HCl(g) }\to \,\text{2NC}{{\text{l}}_{2}}+{{\text{H}}_{2}}(g)$
By using is ideal gas equation which is
$PV=nRT$
We calculate molar volume of Hydrogen gas. We should take the case that while performing the experiment the laboratory became ${{\text{H}}_{2}}$ gas as flammable. Don’t use burgher form experiment because in open flame ${{\text{H}}_{2}}$ reacts explosively with ${{\text{O}}_{2}}$ which present in air use of $\text{HCl}$ also done in safe mole because if it intalea, or brought contact with eyes or skin at gives bad effect on it.
When the reaction of link and Hydrochloric acid takes place during the experiment then evolution of hydrogen gas takes place we have to quickly collect that gas into a test tube and fix a knob on it then measure it by the experiments method which is performed in laboratory only.

Note: In the cases of ideal gases, the molar volume of gas is calculated by the ideal gas equation. Ideal gas equation gives a good approximation for many common gases at standard temperature and pressure.