Question

How many moles of \(\mathrm{CO_2}\) are produced when 4 moles of \(\mathrm{C_2H_6}\) (ethane) combust completely? 
Given reaction: \[ 2 \mathrm{C_2H_6} + 7 \mathrm{O_2} \rightarrow 4 \mathrm{CO_2} + 6 \mathrm{H_2O} \]

• A. 2 moles
• B. 4 moles
• C. 6 moles
• D. 8 moles

Hint:

Use the mole ratio from the balanced chemical equation to find the amount of product formed or reactant consumed.

Answer 1

The Correct Option is D

Step 1: From the balanced chemical equation, \[ 2 \text{ moles of } \mathrm{C_2H_6} \rightarrow 4 \text{ moles of } \mathrm{CO_2} \] Step 2: Find moles of \(\mathrm{CO_2}\) produced from 4 moles of \(\mathrm{C_2H_6}\): \[ \text{If } 2 \text{ moles of } \mathrm{C_2H_6} \rightarrow 4 \text{ moles of } \mathrm{CO_2} \] \[ \Rightarrow 4 \text{ moles of } \mathrm{C_2H_6} \rightarrow x \text{ moles of } \mathrm{CO_2} \] Step 3: Calculate \(x\): \[ x = \frac{4 \times 4}{2} = 8 \text{ moles} \]