Question

The equation for the complete combustion of butane is:
$2C_{4}H_{10} + 13O_{2} \rightarrow 8CO_{2} + 10H_{2}O$
What is the amount (in mole) of carbon dioxide formed by the complete combustion of three moles of n-butane?

• A. 24
• B. 12
• C. 8
• D. 4

Hint:

Always simplify your stoichiometric ratios (e.g., 2:8 becomes 1:4) to make calculations faster.

Answer 1

The Correct Option is B

Step 1: Concept
Stoichiometry allows us to calculate the amount of products formed from a given amount of reactants using the balanced chemical equation.

Step 2: Molar Ratio Analysis
From the balanced equation: $2$ moles of $C_{4}H_{10}$ produce $8$ moles of $CO_{2}$. This simplifies to a ratio of $1:4$.

Step 3: Calculation
If $1$ mole of butane produces $4$ moles of $CO_{2}$, then $3$ moles of butane will produce $3 \times 4 = 12$ moles of $CO_{2}$.

Step 4: Conclusion
The amount of $CO_{2}$ formed is $12$ moles. Final Answer: (B)