The amount of carbon dioxide evolved upon complete combustion of $116$ g of $n$ -butane is
(Given: atomic mass in amu H $= 1$ , C $= 12$ and O $= 16$ )NEET 2026 (Re-NEET)

Question

The amount of carbon dioxide evolved upon complete combustion of 116 g of n -butane is (Given: atomic mass in amu H = 1 , C = 12 and O = 16 )NEET 2026 (Re-NEET)

TestHub · Accepted Answer

The balanced chemical equation for the combustion of $n$ -butane is:

$C_{4} H_{10} + \frac{13}{2} O_{2} \to 4 C O_{2} + 5 H_{2} O$

Molar mass of $n$ -butane ( $C_{4} H_{10}$ ) $= 4 \times 12 + 10 \times 1 = 58$ g/mol

Number of moles of $n$ -butane $= \frac{116}{58} = 2$ moles

From the balanced equation, $1$ mole of $n$ -butane produces $4$ moles of $C O_{2}$ .

Number of moles of $C O_{2}$ produced $= 2 \times 4 = 8$ moles

Molar mass of $C O_{2} = 12 + 2 \times 16 = 44$ g/mol

Mass of $C O_{2}$ produced $= 8 \times 44 = 352$ g

Answer: $352$ g

Chemistry - Mole Concept Question with Solution | TestHub

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