3. Atmospheric pressure at the top of Mt. Everest is about 150 mm Hg. That
is why climbers always bring oxygen tanks. If a climber carries a
12.0 liter tank with a pressure of 35,000 mm Hg, what volume will the
gas occupy if it is released at the top of Mt. Everest?
P1V1 = P2V2
To solve this problem, we can use Boyle's Law, which states that the volume of a gas is inversely proportional to its pressure when temperature is constant.
Boyle's Law equation: P1 * V1 = P2 * V2
Where:
P1 = Initial pressure
V1 = Initial volume
P2 = Final pressure
V2 = Final volume
In this case, we are given:
Initial pressure (P1) = 35,000 mm Hg
Final pressure (P2) = 150 mm Hg
We need to find the final volume (V2) when the gas is released at the top of Mt. Everest. The initial volume (V1) is given as 12.0 liters.
Using Boyle's Law equation:
P1 * V1 = P2 * V2
Substituting the given values:
(35,000 mm Hg) * (12.0 liters) = (150 mm Hg) * V2
Now, we can calculate for V2:
V2 = (35,000 mm Hg * 12.0 liters) / 150 mm Hg
V2 = 2800 liters
Therefore, if the gas is released at the top of Mt. Everest, it will occupy a volume of 2800 liters.