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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