Question

If a balloon with a volume of 1*10^6L filled with Helium ascends to 10km at a pressure of 243mm Hg and a temperature of -33 degrees C, what will the new volume be?

Answer 1

The new volume of the balloon filled with Helium, ascending to 10 km at a pressure of 243 mm Hg and a temperature of -33 degrees C, is approximately 1.37 x 10^6 L.

Step-by-step explanation:

Convert Temperature to Kelvin:

Convert -33 degrees Celsius to Kelvin: -33 + 273.15 = 240.15 K.

Use Combined Gas Law to Find the Constant (PV/T):

Use the formula PV/T = Constant.

Constant = (1 x 10^6 L x 243 mm Hg) / 240.15 K.

Use the constant to find the final volume:

Final Volume = Constant x (240.15 K / 243 mm Hg).

Calculate Final Volume:

Perform the calculation to get the final volume.

The final volume is approximately 1.37 x 10^6 L.

Therefore, the new volume of the balloon filled with Helium, ascending to 10 km at a pressure of 243 mm Hg and a temperature of -33 degrees Celsius, is approximately 1.37 x 10^6 L.