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3. Based on the following balanced equation:

\[2 \text{ C}_4\text{H}_{10} + 13 \text{ O}_2 \rightarrow 8 \text{ CO}_2 + 10 \text{ H}_2\text{O}\]

a. How many moles of \(\text{O}_2\) are required to react completely with 4.00 moles of \(\text{C}_4\text{H}_{10}\)?

- Options: 3.00, 6.00, 8.00, 10.00, 13.00, 16.00, 20.00, 23.00, 26.00

b. How many moles of \(\text{CO}_2\) are produced after the complete reaction of 4.00 moles of \(\text{C}_4\text{H}_{10}\)?

- Options: 3.00, 6.00, 8.00, 10.00, 13.00, 16.00, 20.00, 23.00, 26.00

c. How many moles of \(\text{H}_2\text{O}\) are produced after the complete reaction of 4.00 moles of \(\text{C}_4\text{H}_{10}\)?

- Options: 3.00, 6.00, 8.00, 10.00, 13.00, 16.00, 20.00, 23.00, 26.00

Answer :

Answer:

A. 26 moles O2

B. 16 moles CO2

C. 20 moles H20

Explanation:

a. 4 moles C4H10 x [tex]\frac{13 moles O2}{2 moles C4H10}[/tex] = 26 moles O2

B. 4 moles C4H10 x [tex]\frac{8 moles CO2}{2 moles C4H10}[/tex] = 16 moles CO2

C. 4 moles C4H10 x [tex]\frac{10 moles H2O}{2 moles C4H10}[/tex] = 20 moles H20

Use the coefficients of the balanced equation to make the convertions

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