Final answer:
The temperature at which uranium hexafluoride has a density of 0.9560 g/L at 0.5073 atm is 234.4 K.
Step-by-step explanation:
To determine the temperature at which uranium hexafluoride (UF6) has a density of 0.9560 g/L at 0.5073 atm, we need to use the ideal gas law equation.
The ideal gas law equation is 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. Rearranging the equation to solve for T, we have T = (PV) / (nR).
We can then substitute the given values: P = 0.5073 atm, V = 1 L (since the density is given in g/L and we want to find the temperature at 1 L), n = mass / molar mass, and R = 0.0821 L·atm/(K·mol) (the ideal gas constant).
Molar mass of UF6 = 349.0 g/mol, so the number of moles can be calculated as follows: n = mass / molar mass = (density x volume) / molar mass = (0.9560 g/L x 1 L) / 349.0 g/mol = 0.00274 mol.
Now we can plug in all the values into the equation: T = (PV) / (nR) = (0.5073 atm x 1 L) / (0.00274 mol x 0.0821 L·atm/(K·mol)) = 234.4 K.
Therefore, the temperature at which uranium hexafluoride has a density of 0.9560 g/L at 0.5073 atm is 234.4 K.