calculate the density of oxygen at STP?
Doesn't one mole occupy 22.4 liters?
haha dunno
bhavika is your surname Nayee!!!! if it is.....I KNOW YOU!!!!!!! please reply
To calculate the density of oxygen at STP (Standard Temperature and Pressure), we need to know the molar mass of oxygen and the STP conditions.
1. Molar mass of oxygen:
The molar mass of oxygen (O2) is the sum of the atomic masses of two oxygen atoms. Oxygen has an atomic mass of approximately 16 g/mol. Therefore, the molar mass of oxygen is 2 * 16 g/mol = 32 g/mol.
2. STP conditions:
At STP, the temperature is 0 degrees Celsius (273.15 Kelvin) and the pressure is 1 atmosphere (atm).
3. Use the Ideal Gas Law:
The ideal gas law relates the density of a gas (ρ) to its molar mass (M), temperature (T), and pressure (P) using the formula:
density (ρ) = (M * P) / (R * T)
Where:
- ρ is the density (in g/L or g/cm³).
- M is the molar mass (in g/mol).
- P is the pressure (in atm).
- R is the ideal gas constant (0.0821 L·atm/(mol·K)).
- T is the temperature (in Kelvin).
4. Calculate the density of oxygen at STP:
Substitute the known values into the formula:
density (ρ) = (32 g/mol * 1 atm) / (0.0821 L·atm/(mol·K) * 273.15 K)
Simplifying the equation:
density (ρ) = 1.429 g/L
Therefore, the density of oxygen at STP is approximately 1.429 g/L or 1.429 g/cm³.