At what temperature does uranium hexafluoride have a density of 0.8980 g/L at 0.5073 atm?

Answer 1

Since density is defined as mass/volume, we can use the ideal gas law to solve this problem.

Given the density of 0.8980 g UF6 / L and a pressure of 0.5073 atm.

molar mass UF6 = 352 g/mol

0.8989 g / L x 1 mol / 352 g = 0.00255 mol/L

So, using the ideal gas law PV = nRT , we have...

P = pressure = 0.5073 atm

V = volume = 1 L

n = moles = 0.00255 mol

R = gas constant = 0.0821 Latm/Kmol

T = temperature in Kelvin = ?

Solving for T, we have..

T = PV/nR = (0.5073)(1) / (0.00255)(0.0821)

T = 2423 K

T = 2423 - 273 = 2150 ºC