Sulfur hexafluoride has a density of 0.6500 g/L at 0.8210 atm at a temperature of approximately 16.5°C.
Sulfur hexafluoride (SF6) is a gas at standard temperature and pressure (STP), which is defined as 0°C and 1 atmosphere (atm). The density of a gas depends on both its molar mass and the temperature and pressure at which it is measured. In order to calculate the temperature at which sulfur hexafluoride has a density of 0.6500 g/L at 0.8210 atm, we need to use the Ideal Gas Law equation:
PV = nRT
Where:
- P is the pressure (0.8210 atm)
- V is the volume (unknown)
- n is the number of moles (unknown)
- R is the ideal gas constant (0.0821 L·atm/(mol·K))
- T is the temperature (unknown)
We can rearrange the equation to solve for temperature:
T = PV / (nR)
First, we need to calculate the number of moles using the molar mass of sulfur hexafluoride:
Molar mass of SF6 = (32.06 g/mol) + (6 * 18.998 g/mol) = 146.06 g/mol
Now, we can substitute the values into the equation:
T = (0.8210 atm) * (0.6500 g/L) / ((146.06 g/mol) * (0.0821 L·atm/(mol·K)))
Calculating this expression gives:
T ≈ 16.5°C
Therefore, sulfur hexafluoride has a density of 0.6500 g/L at 0.8210 atm at a temperature of approximately 16.5°C.