You have several identical balloons. You experimentally...

You have several identical balloons. You experimentally determine that a balloon will break if its volume exceeds $0.900 \mathrm{~L}$.The pressure of the gas inside the balloon equals air pressure $(1.00 \mathrm{~atm}) .(\mathrm{a})$ If the air inside the balloon is at a constant $22.0^{\circ} \mathrm{C}$ and behaves as an ideal gas, what mass of air can you blow into one of the balloons before it bursts? (b) Repeat part (a) if the gas is helium rather than air.

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Key Concepts

Ideal Gas Law

The ideal gas law (PV = nRT) relates the pressure, volume, temperature, and amount (in moles) of a gas. This equation is a fundamental tool in thermodynamics for understanding how gases behave under various conditions and is used to calculate one variable when the others are known.

Temperature Conversion to Kelvin

Temperature in the ideal gas law must be expressed in Kelvin because the gas constant (R) is defined using the Kelvin scale. Converting from Celsius to Kelvin ensures accuracy by using an absolute temperature scale, which is critical for applying the ideal gas law correctly.

Molar Mass and Mass-Mole Relationship

Molar mass is a key property that translates between the mass of a substance and the number of moles. This concept is essential when calculating how much mass of a gas corresponds to a particular amount of substance obtained from the ideal gas law.

Application of Gas Properties to Phase Change or Break Conditions

Understanding the limits of a system, such as the maximum volume a balloon can attain before bursting, involves applying gas laws to predict behavior under controlled conditions. This includes calculating how much gas can be introduced into a system before reaching a critical threshold.

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