JEE MAIN - Chemistry (2020 - 5th September Morning Slot - No. 17)
The minimum number of moles of O2
required for complete combustion of 1 mole of propane and 2
moles of butane is _____.
Answer
18
Explanation
C3H8(g) + 5O2(g) $$ \to $$ 3CO2(g) + 4H2O(l)
C4H10(g) + $${{13} \over 2}$$O2(g) $$ \to $$ 4CO2(g) + 5H2O(l)
$$ \therefore $$ No. of moles of O2 required to oxidise 1 mole of propane = 5
$$ \therefore $$ No. of moles of O2 required to oxidise 1 mole of butane = $${{13} \over 2}$$
So, No. of moles of O2 required to oxidise 1 mole of
propane and 2 moles of butane = 5 + 2 $$ \times $$ $${{13} \over 2}$$ = 18
C4H10(g) + $${{13} \over 2}$$O2(g) $$ \to $$ 4CO2(g) + 5H2O(l)
$$ \therefore $$ No. of moles of O2 required to oxidise 1 mole of propane = 5
$$ \therefore $$ No. of moles of O2 required to oxidise 1 mole of butane = $${{13} \over 2}$$
So, No. of moles of O2 required to oxidise 1 mole of
propane and 2 moles of butane = 5 + 2 $$ \times $$ $${{13} \over 2}$$ = 18
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