A weather balloon is inflated to a volume of 28.5 L at a pressure of 748 mmHg and a temperature of 28.0 degrees C. The balloon rises in the atmosphere to an altitude of 25,000 feet, where the pressure is 385 mmHg and the temperature is - 15.0 degrees C. Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude.

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Genevieve

Chemistry

6 October, 21:18

A weather balloon is inflated to a volume of 28.5 L at a pressure of 748 mmHg and a temperature of 28.0 degrees C. The balloon rises in the atmosphere to an altitude of 25,000 feet, where the pressure is 385 mmHg and the temperature is - 15.0 degrees C. Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude.

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Lizbeth Moss · Answer 1

We are given with the conditions of the weather balloon and required to determine the volume of the balloon when the altitude is raised to 25,000 feet. We determine the number of moles through ideal gas law PV = nRT. Plugging to this equation, the number of moles is 1.1351 moles. We substitute this with another set of conditions, volume is 47.46 liters.