Find the volume, in L, of 100g gas mixture containing 10.0 mol% hydrogen in nitrogen at 30.0C and 5.00 atm. Use the avg molecular wt.

what is the molar concentration of hydrogen, in mol/L, in the gas mixture?

what is the average mass denisity in g/L

Avg molar mass H2+N2 where

H2 = 0.1 x 2g/mol = 0.2
N2 = 0.9 x 28g/mol = 25.2
Total = 25.4 g/mol.
Convert 100 g to mols using 25.4 as the molar mass of the mixture and solve for volume in PV = nRT.

part 2.

total mols x 0.1 = mols H2.
molsH2/total volume = M

part 3.
density = g/L
22.4L for a mol of the gas has a mass of 25.4 g so 25.4/22.4 = density.

To find the molar concentration of hydrogen in the gas mixture, we need to first calculate the number of moles of hydrogen present.

Given:
Mass of the gas mixture = 100g
Molar fraction of hydrogen = 10.0 mol%
Temperature = 30.0°C or 303.15K
Pressure = 5.00 atm

To find the number of moles of hydrogen, we can use the formula:

Moles of a component = Mass of the component / Molar mass of the component

First, we need to calculate the mass of hydrogen present in the gas mixture.

Mass of hydrogen = Molar fraction of hydrogen x Mass of the gas mixture
= 10.0 mol% x 100g
= 0.1 x 100g
= 10g

Next, we need to calculate the molar mass of hydrogen, which is approximately 2 g/mol.

Now, we can find the number of moles of hydrogen:

Moles of hydrogen = Mass of hydrogen / Molar mass of hydrogen
= 10g / 2 g/mol
= 5 mol

To find the molar concentration of hydrogen, we can divide the moles of hydrogen by the volume of the gas mixture.

Molar concentration of hydrogen = Moles of hydrogen / Volume of the gas mixture

Since we do not know the volume of the gas mixture, we cannot determine the molar concentration of hydrogen.

Moving on to the next question regarding the average mass density:

To calculate the average mass density, we need to know the volume of the gas mixture. However, the volume is not provided in the given information. Hence, we cannot determine the average mass density either.