Step 1: List the given values.
[tex]\begin{aligned} & P = \text{779 mmHg = 1.025 atm} \\ & T = 62^{\circ}\text{C} = \text{335.15 K} \\ & MM = \text{352.02 g/mol} \end{aligned}[/tex]
Step 2: Calculate the density.
[tex]\begin{aligned} d & = \frac{(P)(MM)}{RT} \\ & = \frac{(\text{1.025 atm})(\text{352.02 g/mol})}{\left(0.082057 \: \dfrac{\text{L}\cdot\text{atm}}{\text{mol}\cdot\text{K}}\right)(\text{335.15 K})} \\ & = \boxed{\text{13.12 g/L}} \end{aligned}[/tex]
Hence, the density of uranium hexafluoride at 62°C and 779 mmHg is 13.12 g/L.
[tex]\\[/tex]
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SOLUTION:
Step 1: List the given values.
[tex]\begin{aligned} & P = \text{779 mmHg = 1.025 atm} \\ & T = 62^{\circ}\text{C} = \text{335.15 K} \\ & MM = \text{352.02 g/mol} \end{aligned}[/tex]
Step 2: Calculate the density.
[tex]\begin{aligned} d & = \frac{(P)(MM)}{RT} \\ & = \frac{(\text{1.025 atm})(\text{352.02 g/mol})}{\left(0.082057 \: \dfrac{\text{L}\cdot\text{atm}}{\text{mol}\cdot\text{K}}\right)(\text{335.15 K})} \\ & = \boxed{\text{13.12 g/L}} \end{aligned}[/tex]
Hence, the density of uranium hexafluoride at 62°C and 779 mmHg is 13.12 g/L.
[tex]\\[/tex]
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