Question

9. A very large helium filled balloon has a volume of 38.1 L and is at a high altitude where the

temperature is 0.00°C and the pressure is 471 torr. It is returned to the ground where the T is
24.0°C and its volume is now 22.9 L. What is the pressure on the ground?

Answer 1

753 torr.

Step-by-step explanation:

The pressure at the ground can be calculated using the ideal gas law, PV = nRT, where P is pressure, V is volume, n is the number of moles of gas, R is the gas constant, and T is temperature.

First, we'll find n by using the fact that the number of moles is constant, n1V1 = n2V2. We'll use the ideal gas law to solve for P on the ground:

P = (nRT) / V = (n * R * (24 + 273.15) * 22.9) / 22.9 = (n * R * 297.15) / 22.9

Plugging in the initial values from the high altitude, we have:

n = (38.1 * 471) / (R * (0 + 273.15)) = (38.1 * 471) / (8.31 * 273.15)

So, finally:

P = (n * R * 297.15) / 22.9 = (38.1 * 471 * 8.31 * 297.15) / (22.9 * 273.15) = 753 torr

The pressure on the ground is 753 torr.