Avogadro's law states that the volume of a gas is directly proportional to the number of moles of gas when temperature and pressure are held constant. Mathematically, it can be expressed as $V \propto n$ or $\frac{V}{n} = k$.
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Avogadro's law explains the relationship between volume and amount (moles) of a gas.
The law implies that equal volumes of all gases, at the same temperature and pressure, contain an equal number of molecules.
It can be expressed with the equation $V_1 / n_1 = V_2 / n_2$ for two different states of a gas.
The concept is crucial for understanding molar volume, which is 22.4 L at standard temperature and pressure (STP).
Avogadro's number (6.022 x $10^{23}$) is derived from Avogadro’s hypothesis about equal volumes containing equal numbers of molecules.
Review Questions
Explain how Avogadro's law relates the volume and amount of gas under constant temperature and pressure.
Use Avogadro's law to calculate the new volume if the amount of gas changes from 2 moles to 4 moles while maintaining constant temperature and pressure.
What does Avogadro’s law imply about the volumes of different gases under identical conditions?
A fundamental equation that describes the state of an ideal gas using pressure (P), volume (V), temperature (T), and amount in moles (n): $PV = nRT$.
Boyle’s Law: States that the pressure of a given mass of gas is inversely proportional to its volume at constant temperature: $P \propto \frac{1}{V}$ or $PV = k$.
Charles’s Law: Describes how gases tend to expand when heated; at constant pressure, the volume of a gas is directly proportional to its absolute temperature: $V \propto T$ or $\frac{V}{T} = k$.