Weather Balloon Gas Laws

The video tutorial explains how to determine the volume of a weather balloon just before it bursts using the ideal gas law. It starts with a scenario involving a balloon filled with helium gas, launched into the atmosphere. The tutorial covers the ideal gas law, its variables, and how they change with altitude. It then applies the law to calculate the balloon's final volume, considering changes in pressure and temperature. The solution involves converting temperatures to Kelvin and using the formula to find the volume, ensuring the units and significant figures are correct.

What is the initial volume of helium gas in the weather balloon?

• 18.5 liters

• 1.85 times 10 to the third liters

• 185 liters

• 1.85 liters

At what altitude does the weather balloon burst?

• 16 kilometers

• 128 kilometers

• 32 kilometers

• 64 kilometers

Which law is used to solve the problem of the weather balloon's volume change?

• Charles's Law

• Ideal Gas Law

• Boyle's Law

• Avogadro's Law

What remains constant as the balloon ascends to higher altitudes?

• Volume

• Pressure

• Temperature

• Number of moles

What is the initial pressure of the helium gas in the balloon?

• 6.51 torr

• 500 torr

• 1013 torr

• 765 torr

How is the temperature converted from Celsius to Kelvin?

• Add 100

• Multiply by 2

• Add 273

• Subtract 273

What is the final temperature of the helium gas in Kelvin?

• 310 K

• 296 K

• 273 K

• 229 K

What is the final pressure of the helium gas just before the balloon bursts?

• 765 torr

• 6.51 torr

• 500 torr

• 1013 torr

What is the calculated final volume of the balloon in liters?

• 1.68 times 10 to the second liters

• 1.68 times 10 to the third liters

• 1.68 times 10 to the fourth liters

• 1.68 times 10 to the fifth liters

Why does the volume of the balloon increase as it ascends?

• The ideal gas constant changes.

• The number of moles increases.

• The temperature increases with altitude.

• The pressure decreases with altitude.