Final answer:
Using Boyle's Law, the volume of oxygen when it is released from a tank with an internal pressure of 3.70 x 10⁴ mmHg containing 15.00 L at the atmospheric pressure on the peak of Mt. Everest (155.0 mmHg) is approximately 3,580 L.
Step-by-step explanation:
The question involves the application of the ideal gas law and conversion of gas volumes under different pressures. Given that the atmospheric pressure on the peak of Mt. Everest can be as low as 155.0 mmHg, and climbers carry oxygen tanks with an internal pressure of 3.70 x 10⁴ mmHg containing 15.00 L of gas, we want to find out the volume of the oxygen when it is released.
To find the new volume when the gas is released, we can use Boyle's Law, which states that the pressure of a gas times its volume is constant at a constant temperature (P1V1 = P2V2). We have P1 = 3.70 x 10⁴ mmHg, V1 = 15.00 L, and P2 = 155.0 mmHg. Solving for V2 gives us V2 = (P1 * V1) / P2 = (3.70 x 10⁴ mmHg * 15.00 L) / 155.0 mmHg, which simplifies to approximately 3,580 L.
Therefore, the volume of the gas when it is released from the tanks under the conditions at the peak of Mt. Everest is approximately 3,580 L, which corresponds to option A.