what is the density of O2 gas at STP
molar mass/22.4 = ??g/L
To find the density of O2 gas at STP (Standard Temperature and Pressure), you need to know the molar mass of O2 and the values of STP.
1. Find the molar mass of O2:
The molar mass of O2 is the sum of the atomic masses of two oxygen atoms. The atomic mass of oxygen is approximately 16.00 g/mol. Therefore, the molar mass of O2 is 2 * 16.00 g/mol = 32.00 g/mol.
2. Determine the values of STP:
At STP, the standard temperature is 0 degrees Celsius (273.15 Kelvin) and the standard pressure is 1 atmosphere (1 atm).
3. Use the ideal gas law equation:
The ideal gas law equation is given as PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.
4. Rearrange the equation to solve for the density:
The density (ρ) is defined as mass per unit volume. Therefore, density (ρ) = mass (m) / volume (V). We can rewrite the equation as PV = (m / M) * RT, where M is the molar mass of O2.
5. Solve for density:
Rearrange the equation to isolate density:
ρ = (m / V) = (P * M) / (RT)
Substitute the values:
- P = 1 atm (standard pressure at STP)
- M = 32.00 g/mol (molar mass of O2)
- R = 0.0821 L * atm / (K * mol) (ideal gas constant)
- T = 273.15 K (standard temperature at STP)
Plug in the values to calculate:
ρ = (1 atm * 32.00 g/mol) / (0.0821 L * atm / (K * mol) * 273.15 K)
Simplify the equation and calculate the final value to find the density of O2 gas at STP.