Chapter 5
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.
Step-by-Step
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 |