Ideal Gas Law:
The density of an ideal gas can be calculated using the Ideal Gas Law:
* PV = nRT
Where:
* P is the pressure (in Pascals or atmospheres)
* V is the volume (in cubic meters or liters)
* n is the number of moles of the gas
* R is the ideal gas constant (8.314 J/mol·K or 0.0821 L·atm/mol·K)
* T is the temperature (in Kelvin)
Deriving Density:
To get density (ρ = mass/volume), we need to manipulate the ideal gas law:
1. n = m/M (where m is the mass of the gas and M is the molar mass)
2. Substitute n in the ideal gas law: PV = (m/M)RT
3. Rearrange to solve for density (ρ = m/V): ρ = (PM)/(RT)
Density of Hydrogen at Standard Conditions:
At standard temperature and pressure (STP):
* T = 273.15 K
* P = 1 atm
* M (molar mass of H₂) = 2.016 g/mol
Plugging these values into the equation:
ρ = (1 atm * 2.016 g/mol) / (0.0821 L·atm/mol·K * 273.15 K)
ρ ≈ 0.0899 g/L
Important Note: The density of hydrogen gas changes significantly with temperature and pressure. At higher temperatures and pressures, the density will increase.
Let me know if you need the density of hydrogen at specific conditions.
