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## Q. 5.3

Sulfur hexafluoride is a gas used as a long-term tamponade (plug) for a retinal hole to repair detached retinas in the eye. If 2.50 g of this compound is introduced into an evacuated 500.0-mL container at 83°C, what pressure in atmospheres is developed?

 ANALYSIS V (500.0 mL); T (83°C); mass of $SF_{6}$ (2.50 g) Information given: molar mass of $SF_{6}$ ideal gas law (one state) value for R Information implied: pressure (P) in atm Asked for:

STRATEGY

1. Change the given units to conform with the units for R (mL → L; °C → K).
2. You need to find n before you can use the ideal gas law to find P.
3. Substitute into the ideal gas law: PV = nRT.

## Verified Solution

 1. Change units. 500.0 mL = 0.5000 L           83°C + 273 K = 356 K 2. Find n. 2.50 g ×$\frac{1 mol}{146.07 g}$ = 0.0171 mol 3. P P = $\frac{nRT}{V}$ =$\frac{0.0171 mol × 0.0821 L · atm/(mol · K) × 356 K}{0.5000 L}$ = 1.00 atm