Please find below the solution to the asked query:
2Pb(NO3)2 (s) → 2PbO(s) +4NO2 (g) + O2 (g)
Molar mass of Pb(NO3)2 = 331 g/mol
Molar mass of NO2 = 46 g/mol
Molar mass of O2 = 32 g/mol
Now, we know that molar mass of a gas contains 22.4 L of gas so,
46 g of Nitrogen dioxide = 22.4 L
32 g of Oxygen = 22.4 L
According to balanced chemical equation,
(2x331)=662g of lead nitrate yields (4x22.4)=89.6 L of nitrogen dioxide and 22.4 L of oxygen gas.
Total volume of gases = 89.6 + 22.4 = 112 L
662 g of lead nitrate produces 112 L of gases
8.5 g of lead nitrate will produce (112x8.5)/662 = 1.44 L of gases
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