A 160.0 L helium tank contains pure helium at a pressure of...

A $160.0 \mathrm{~L}$ helium tank contains pure helium at a pressure of 1855 psi and a temperature of $298 \mathrm{~K}$. How many $3.5 \mathrm{~L}$ helium balloons will the helium in the tank fill? (Assume an atmospheric pressure of $1.0 \mathrm{~atm}$ and a temperature of $298 \mathrm{~K}$.)

Key Concepts

Gas Expansion under Changing Conditions

Gas expansion involves understanding how a gas will occupy a different volume when transferred to conditions of lower or higher pressure and temperature. This concept uses the ideal gas law to predict the new volume a gas will occupy when its state variables are altered, such as when gas from a high-pressure tank is released into balloons at atmospheric pressure.

Mole Concept

The mole is a central concept in chemistry that quantifies the amount of substance. In gas law calculations, determining the number of moles present allows for the application of the ideal gas law to relate volumetric measurements with pressure and temperature. It is crucial for calculating how many individual volumes of a gas, such as that found in a balloon, can be obtained from a known quantity.

Pressure Unit Conversion

Converting between different units of pressure is critical in gas law problems since pressure can be expressed in various units such as psi, atm, or pascals. Accurate conversion ensures that all parameters are in consistent units when applying the ideal gas law, which is particularly important when comparing or combining gas conditions measured in different pressure units.

Ideal Gas Law

The ideal gas law, expressed as PV = nRT, is a fundamental equation in chemistry that relates the pressure (P), volume (V), number of moles (n), gas constant (R), and temperature (T) of an ideal gas. This law is used to calculate any one of these variables when the other three are known, and it is essential for problems involving gas behavior under varying conditions.

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