Question

A balloon was partially filled with helium gas at room temperature. It occupied 4.0 liters of volume at 700.0 mmHg atmospheric pressure. When the balloon was released, it traveled upward until it burst at 99 mmHg atmospheric pressure. (Neglect any force exerted to stretch the rubber balloon.) What was the volume of the balloon when it burst? L

Answer 1

I used Boyle's Law. 28.28L

Answer 2

Answer: The new volume was 28 L.

Solution: If we look at the given data then the temperature is constant and from Boyle's law we know that, "At constant temperature, volume is inversely proportional to the pressure of the gas."

The equation used for solving the Boyle's law problems is:

`P_1V_1=P_2V_2`

where,
`P_1` is the initial pressure and
`V_1` is initial volume.

Similarly,
`P_2` is final pressure and
`V_2` is final volume.

From given data, initial volume is 4.0 L, initial pressure is 700.0 mmHg and final pressure is 99 mmHg. We are asked to calculate the final volume.

Let's plug in the values in the equation:

`(700.0mmHg)(4.0L)=(99mmHg)(V_2)`

`V_2=((700.0mmHg)(4.0L))/(99mmHg)`

`V_2` = 28.28 L

If we round the answer to correct number of sig figs then it will be 28 L since the initial given volume has only two sig figs.