A balloon contains 2.0 L helium at 1.10 atm . Calculate the work done if the gas expands again

step 1 In this question, we have to recall that the work done is equal to negative P delta V. And this

A balloon contains 2.0 L helium at 1.10 atm . Calculate...

A balloon contains $2.0 \mathrm{~L}$ helium at $1.10 \mathrm{~atm} .$ Calculate the work done if the gas expands against a constant atmospheric pressure of 754 torr. The expansion will stop when the internal pressure equals the external pressure. Use Boyle's law to determine the final volume.

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Key Concepts

Work Done in Gas Expansion under Constant External Pressure

When a gas expands against a constant external pressure, the work done by the gas is defined as the negative product of the external pressure and the change in volume (W = -P_ext ?V). This concept is important in thermodynamics as it quantifies the energy transferred as work during the expansion or compression of gases.

Unit Conversions for Pressure and Energy

Accurate calculations in gas expansion problems often require converting pressure units, such as from torr to atmospheres, because equations in thermodynamics are typically expressed in standard units like atm or Pa. Additionally, converting energy units (for example, from L·atm to Joules) ensures that the final work calculation is in the desired unit of energy, allowing for proper comparison and application in engineering and science contexts.

Boyle's Law

Boyle's Law states that for a fixed amount of gas kept at a constant temperature, the product of the pressure and volume is constant. This relationship (P1V1 = P2V2) is used to determine how the volume of a gas changes as the pressure changes, and is essential for analyzing processes where gases expand or compress under constant temperature conditions.

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