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Avogadro's Hypothesis

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↪ This law states, "Under similar conditions of pressure and temperature, equal volume of all the gaseous substance contain equal number of molecules."

Mathematically,

Volume(v) ∝ No. of Molecules (n) {under similar condition of pressure and temperature}

22.4l of Hydrogen at NTP = 6.023x1023 No. of molecules of H2 = 2g
22.4l of Nitrogen at NTP = 
6.023x1023 No. of molecules of N2 = 28g
22.4l of CO2 at NTP = 
6.023x1023 No. of molecules of CO2 = 44g
22.4l of O at NTP = 
6.023x1023 No. of molecules of O2 = 32g
22.4l of CO at NTP = 
6.023x1023 No. of molecules of CO = 28g

 1 mole or mol :

↪ It is the collection of 6.023x1023 No. of chemical species. (atoms, ions, compounds, molecules or electrons)

For examples,

1 mole of Na = 
6.023x1023 No. of Na atoms
1 mole of Ca = 6.023x1023 No. of Ca atoms
1 mole of K = 
6.023x1023 No. of K atoms
1 mole of CO2
6.023x1023 No. of CO2 
1 mole of Nitrogen gas = 
6.023x1023 No. of N2 gas
1 mole of Na+ = 6.023x1023 No. of Na ions
1 mole of H+6.023x1023 No. of H ions
1 mole of e- = 6.023x1023 No. of electrons