Answer:
4204 K
Explanation:
Step 1: Data
Given data
Required data
Step 2: Calculate the temperature of the gas
We will use the following expression derived from the ideal gas equation.
P × M = ρ × R × T
T = P × M/ρ × R
T = 0.5073 atm × (352.02 g/mol)/(0.5820 g/L) × (0.08206 atm.L/mol.K)
T = 4204 K
The temperature of the uranium hexafluoride has been 3,737.36 K.
The uranium hexafluoride has been the gas. Assuming the gas to follow the ideal equation:
Pressure × Volume = Moles × R × Temperature
Moles can be defined as:
Moles = [tex]\rm \dfrac{mass}{molecular\;mass}[/tex]
The ideal gas equation can be written in terms of mass as:
Pressure × Volume = [tex]\rm \dfrac{mass}{molecular\;mass}[/tex] × R × Temperature
Pressure = [tex]\rm \dfrac{mass}{volume}[/tex] × [tex]\rm \dfrac{1}{molecular\;mass}[/tex] × R × Temperature
Density can be defined as:
Density = [tex]\rm \dfrac{mass}{volume}[/tex]
The equation in terms of density can be written as:
Pressure = Density × [tex]\rm \dfrac{1}{molecular\;mass}[/tex] × R × Temperature
The molecular mass of uranium hexafluoride = 352.02 g/mol
R = 0.0816 L.atm/K.mol
Pressure = 0.5073 atm
Density = 0.5820 g/L
Substituting the values:
0.5073 atm = 0.5820 g/L × [tex]\rm \dfrac{1}{352.02\;g/mol}[/tex] × 0.0821 L.atm/K.mol × Temperature
0.5073 = 0.000135 × Temperature
Temperature = 3,737.36 K.
The temperature of the uranium hexafluoride has been 3,737.36 K.
For more information about the temperature of the gas, refer to the link:
https://brainly.com/question/16957585
