The minimum amount of Ag2CO3(s) required to produce sufficient oxygen for the complete combustion of C2H2 which produces 11.2L of CO2 at STP after combustion is: (Molar mass of Ag=108g/mol) Ag2CO3(s)→2Ag(s)+CO2(g)+12O2(g) C2H2+52O2→2CO2+H2O
A
276g
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B
345g
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C
690g
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D
138g
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Solution
The correct option is B345g Ag2CO3(s)→2Ag(s)+CO2(g)+12O2(g)(1)
C2H2+52O2→2CO2+H2O(2)
11.2 litre of CO2 at STP = 11.222.4=0.5 mol ofCO2
From equation (2), 2 mol of CO2 is produced from 2.5 mol of O2. ∴ 0.5 mol of CO2 will be formed from = 2.52×0.5 = 0.625 mol of O2. From equation (1), 1 mol of Ag2CO3 produces 0.5 mol of O2. 0.625 mol of O2 is formed from = 0.625×2 = 1.25 mol of Ag2CO3.
Molar mass of Ag2CO3=276g mol−1 ∴ Minimum amount of Ag2CO3required=276g/mol×1.25mol=345g