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------------------------------------------------ Balance the equation below and determine the number of moles of oxygen required to completely burn 5.00 moles of propane.

\[ \text{C}_3\text{H}_8 + \text{O}_2 \rightarrow \text{H}_2\text{O} + \text{CO}_2 \]

A. 15.0

B. 10.0

C. 2.50

D. 5.00

E. 25.0

To balance the equation, we need to ensure that the number of atoms of each element is the same on both sides. Starting with carbon, we have 3 carbon atoms on the left side and 1 carbon atom on the right side. To balance it, we add a coefficient of 3 in front of CO2:

C3H8 + O2 → 3H2O + 3CO2

Next, we balance the hydrogen atoms by adding a coefficient of 4 in front of H2O:

C3H8 + O2 → 4H2O + 3CO2

Finally, we balance the oxygen atoms by adding a coefficient of 5 in front of O2:

C3H8 + 5O2 → 4H2O + 3CO2

The balanced equation indicates that to completely burn 1 mole of propane (C3H8), we need 5 moles of oxygen (O2). Therefore, to burn 5 moles of propane, we would need 5 times the amount of oxygen, which is 5 * 5 = 25 moles of oxygen.

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