Calculate the density of oxygen, , under each of the following conditions:
STP
1.00 atm and 25.0 C
Assistance needed
At STP you know 1 mol (32 g) oxygen occupies 22.4 L.
2.6
To calculate the density of oxygen under STP (Standard Temperature and Pressure) and at 1.00 atm and 25.0 °C, we need to use the ideal gas law equation:
PV = nRT
Where:
- P is the pressure
- V is the volume
- n is the number of moles of the gas
- R is the ideal gas constant
- T is the temperature in Kelvin
For STP, the pressure is 1.00 atm, and the temperature is 0 °C or 273.15 K. First, we need to calculate the number of moles using the ideal gas law equation.
n = PV / RT
Substituting the values, we have:
n = (1.00 atm) * V / [(0.08206 L.atm/mol.K) * (273.15 K)]
Now, for the given conditions of 1.00 atm and 25.0 °C, we need to convert the temperature to Kelvin.
T = 25.0 °C + 273.15 = 298.15 K
Once we have the number of moles, we can calculate the density using the formula:
Density = mass / volume
The molar mass of oxygen (O₂) is 32.00 g/mol. Therefore, the mass will be the product of the number of moles and the molar mass.
Mass = n * molar mass
Finally, we substitute the values into the density formula to calculate the density of oxygen under the given conditions.