Question

When filling a weather balloon with gas you have to consider that the gas will expand greatly as it rises and the pressure decreases. Let's say you put about 10.0 moles of He gas into a balloon that can inflate to hold 5000.0L. Currently, the balloon is not full because of the high pressure on the ground. What is the pressure when the balloon rises to a point where the temperature is -10.0°C and the balloon has completely filled with the gas.

Answer 1

0.0432 atm

Step-by-step explanation:

Step 1: Given data for when the balloon is full

• Moles of Helium (n): 10.0 mol

• Volume of the balloon (V): 5000.0 L

• Temperature (T): -10.0 °C

• Ideal gas constant (R): 0.0821 atm.L/mol.K

Step 2: Convert "T" to Kelvin

We will use the following expression.

K = °C + 273.15

K = -10.0°C + 273.15 = 263.2 K

Step 3: Calculate the pressure of He in the balloon

We will use the ideal gas equation.

P × V = n × R × T

P = n × R × T/V

P = 10.0 mol × (0.0821 atm.L/mol.K) × 263.2 K/5000.0 L = 0.0432 atm