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4 Questions around this concept.
If a mixture containing 3 moles of Hydrogen and 1 mole of Nitrogen is converted completely into Ammonia, the ratio of initial and final volume under the same temperature and pressure would be:
If a mixture containing 3 moles of Hydrogen and 1 mole of Nitrogen is converted completely into Ammonia, the ratio of initial and final volume under the same temperature and pressure would be:
A and B are two identical vessels. A contains 15 g Ethane at 1atm and 298 K. The vessel B contains 75 g of a gas X2 at same temperature and pressure. The vapour density of X2 is :
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500 ml of a hydrocarbon gas burnt in excess of Oxygen yields 2500 ml of CO2 and 3 of liters water vapours. All volume is measured at the same temperature and pressure. The formula of the Hydrocarbon is
Avogadro’s Law
According to Avogadro's law, "At constant temperature and pressure, equal volume of gases will have same number of molecules or moles "
Molar Volume or Gram Molecular Volume
1 mole of a gaseous substance has 22.4 litre volume at NTP which is known as it's molar volume.
Avogadro Number
1 mole of a substance contains number of molecules.
1 gram atom of any element contains atoms,
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