Question

If a 137.2 mL helium balloon rises in altitude from sea-level (1.00 atm) to 893 ft. (349 torr), what is the volume of the balloon at this altitude?

a) 35.2 mL
b) 137.2 mL
c) 248.6 mL
d) 546.8 mL

Answer 1

To find the volume of the balloon at the given altitude, we can use Boyle's Law. Using the equation P1V1 = P2V2, we can calculate the volume of the balloon at the given altitude to be approximately 392.6 mL. The correct option is (c) 248.6 mL.

Step-by-step explanation:

To find the volume of the balloon at the given altitude, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at constant temperature. We can use the equation:

P1V1 = P2V2

where P1 and V1 are the initial pressure and volume at sea level, and P2 and V2 are the pressure and volume at the given altitude.

Substituting the values we have, we get:

(1.00 atm)(137.2 mL) = (0.349 atm)(V2)

Solving for V2, we find:

V2 = (1.00 atm)(137.2 mL) / (0.349 atm)

V2 ≈ 392.6 mL

Therefore, the volume of the balloon at this altitude is approximately 392.6 mL. The correct option is (c) 248.6 mL.