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)

The correct answer is Option 1. Full mathematical solution steps and hints are accessible in the interactive StemCET workspace.

Chemistry Q63 – NEET-UG 2026

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Home Chemistry Basic ChemistryQuestion #80

The amount of carbon dioxide evolved upon complete combustion of

116 g

n

-butane is (Given: atomic mass in amu

H = 1

C = 12

and

O = 16

)

Clue 1 of 3: Combustion Reaction

The complete combustion of a hydrocarbon produces carbon dioxide and water.

🥷

Ninja Strategy•Quick Moles and Carbon Count

Recognize that $116 g$ of $n$ -butane is exactly 2 moles, and each $n$ -butane molecule has 4 carbon atoms, meaning 2 moles will produce 8 moles of ${CO}_{2}$ .

🧠 Full Solution Path

Step 1: Write and Balance the Combustion Reaction✦ Active

The complete combustion of $n$ -butane ( $C_{4} H_{10}$ ) with oxygen produces carbon dioxide ( ${CO}_{2}$ ) and water ( $H_{2} O$ ). The balanced chemical equation is:

2 C_{4} H_{10} + 13 O_{2} \to 8 {CO}_{2} + 10 H_{2} O

💡 Teacher's Secret Hint

Ensure all atoms are balanced on both sides of the equation.

Step 2: Calculate Moles of

n

-Butane and

{CO}_{2}

○ Expand

The molar mass of $C_{4} H_{10}$ is $(4 \times 12) + (10 \times 1) = 58 g/mol$ . Moles of $n$ -butane given $= \frac{116 g}{58 g/mol} = 2 moles$ . From the balanced equation, $2 moles of C_{4} H_{10}$ produce $8 moles of {CO}_{2}$ . Therefore, $2 moles of C_{4} H_{10}$ will produce $8 moles of {CO}_{2}$ .

💡 Teacher's Secret Hint

The mole ratio from the balanced equation is crucial for stoichiometric calculations.

Step 3: Calculate the Mass of

{CO}_{2}

Produced○ Expand

The molar mass of ${CO}_{2}$ is $(1 \times 12) + (2 \times 16) = 44 g/mol$ . Mass of ${CO}_{2}$ produced $= moles of {CO}_{2} \times molar mass of {CO}_{2}$ Mass of ${CO}_{2} = 8 mol \times 44 g/mol = 352 g$ .

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Chemistry Question 63 – NEET-UG 2026

Clue 1 of 3: Combustion Reaction

🧠 Full Solution Path