Question

13. A balloon filled with helium has a volume of 1.28 x 10³ L

at sea level where the pressure is 0.998 atm and the tempera-
ture is 31°C. The balloon is taken to the top of a mountain
where the pressure is 0.753 atm and the temperature is
-25°C. What is the volume of the balloon at the top of the
mountain?

Answer 1

The volume of the balloon at ground level is 202.07 L.

Step-by-step explanation:

The volume of a gas can be calculated using the ideal gas law equation, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin. To solve for the volume, we can rearrange the equation to V = (nRT)/P.

Given the conditions at ground level (0.992 atm, 25 °C) and the number of moles of helium (8.80 moles), we can substitute these values into the equation to find the volume:

V = (8.80 mol x 0.0821 L•atm/mol•K x (273 + 25) K) / 0.992 atm = 202.07 L

Thus, the volume of the balloon at ground level is 202.07 L.