“Equal volumes of gases, under the same conditions of temperature and pressure, contain the same number of particles.”
If the temperature and pressure be the same, their volumes shall contain an equal number of molecules.
Even if the number of molecules remains constant, the mass of a substance can change through a change in state (solid, liquid, gas) or through chemical reactions.
The Formula of moles and volume
Volume
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No. of moles | Molar volume
The formula of moles and volume talk about the ratio of the volume and the number of moles in volume per unit
Avogadro’s law – Same volume → Same number of particles (at same temp and pressure)
r.t.p. – Room Temperature and Pressure: 25°C (298K), 101.3 kPa (1 atm)
Molar gas volume – 1 mole of any gas = 24 dm³ at r.t.p.
For gaseous reactions, the volume ratios are the same as mole ratios
Gas Expansion: If you inflate a balloon with 0.5 moles of helium gas and then add another 0.2 moles while keeping temperature and pressure constant, how will the volume change?
Chemical Reaction: In a reaction where carbon dioxide is passed over hot coke, the maximum volume of carbon monoxide formed is 32 mL. If the initial volume of CO₂ was 26 mL, does this follow Avogadro’s Law?
Balloon Experiment: A balloon is filled with 2.25 L of helium gas containing 0.0820 moles. If 0.015 moles of helium are added at constant pressure and temperature, what will be the new volume of the balloon?
Gas Mixing: Two containers hold different gases at the same temperature and pressure. One contains 1 mole of oxygen, and the other contains 1 mole of nitrogen. According to Avogadro’s Law, how do their volumes compare?