Answer :
The density of uranium hexafluoride at 779 mmHg and 62 degrees Celsius is approximately 12.26 g/L, calculated using the ideal gas law.
To calculate the density of uranium hexafluoride (UF6) at 779 mmHg and 62 degrees Celsius, we can use the ideal gas law PV=nRT, where P is pressure, V is volume (L), n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin. Given the molar mass of 352 g/mol for UF6, we can rearrange the ideal gas law to solve for density (d = m/V = PM/RT), where M is the molar mass of the gas.
First, convert the temperature to Kelvin (K):
T(K) = 62 "+ 273.15 = 335.15 K.
Next, convert the pressure from mmHg to atm:
P(atm) = 779 mmHg * (1 atm / 760 mmHg) = 1.025 atm.
Now, substitute the values into the density equation and solve:
d = (1.025 atm * 352 g/mol) / (0.0821 L atm/mol K * 335.15 K) = 12.26 g/L. Therefore, the density of uranium hexafluoride at the given conditions is approximately 12.26 g/L.
