Question

A balloon was partially filled with helium gas at room temperature. It occupied 4.0 liters of volume at 700.0 mm Hg atmospheric pressure. When the balloon was released, it traveled upward until it burst at 99 mm Hg atmospheric pressure. What was the volume of the balloon when it burst?

0.55 L
2.8 L
5.6 L
28 L

Answer 1

The correct answer is 28 L

Answer 2

28 L

Step-by-step explanation:

Assuming the temperature of the gas is constant, we can solve the problem by applying Boyle's law, which states that the product between the pressure of the gas (P) and its volume (V) remains constant:

`PV=const.`

`P_1 V_1 = P_2 V_2`

where

`P_1 = 700.0 mm Hg` is the initial pressure

`P_2 = 99 mm Hg` is the final pressure

`V_1 = 4.0 L` is the initial volume

`V_2 = ?` is the final volume

Re-arranging the equation, we can find the final volume:

`V_2 = (P_1 V_1)/(P_2)=((700.0 mmHg)(4.0 L))/(99 mmHg)=28.0 L`