Question

A balloon is filled to a volume of 1.50 L with 2.50 moles of gas at 25 °C. With pressure and temperature held constant, what will be the volume of the balloon if 0.35 moles of gas are released? Incorrect, 1 attempt remaining Your submitted answer contains too few significant figures. Your submission: 0.21L Feedback: You have used the moles removed as the final amount of moles. Remember that these moles are removed from the balloon. Tap here or pull up for additional resources

Answer 1

The volume of the balloon will remain at 1.50 L even after 0.35 moles of gas are released.

According to Boyle's law:

`\[ P_1V_1 = P_2V_2 \]`

where
`\( P_1 \)` and
`\( V_1 \)` are the initial pressure and volume, and
`\( P_2 \)` and
`\( V_2 \)` are the final pressure and volume.

Since the pressure and temperature are held constant, we can simplify the equation to:

At constant pressure:
`P_1 = P_2`, hence, the pressure will cancel out.

Thus, the equation remains:

`\[ V_1 = V_2 \]`

This means that the initial volume
`(\( V_1 \))` is equal to the final volume
`(\( V_2 \))`.

Therefore, the volume of the balloon will remain at 1.50 L even after 0.35 moles of gas are released, as long as the pressure and temperature remain constant.