Questions: Question 25 (1 point) Balance the following reaction by filling in the blanks below. Pay attention that this combustion reaction has an oxygen in the carbon reactant. For this one, do not balance it with fractions. Make sure your equation matches this equation. (If you reverse the products on your paper from what is written here, the program will not know you've done this.) Normally, you would not include a '1' but the program requires something in every blank so include any "1" that is needed. C3H6O + O2 → H2O + CO2 □ A C3H6O+ □ A O2 → □ A H2O+□ A CO2

Question 25 (1 point) Balance the following reaction by filling in the blanks below. Pay attention that this combustion reaction has an oxygen in the carbon reactant. For this one, do not balance it with fractions. Make sure your equation matches this equation. (If you reverse the products on your paper from what is written here, the program will not know you've done this.) Normally, you would not include a '1' but the program requires something in every blank so include any "1" that is needed. C3H6O + O2 → H2O + CO2 □ A C3H6O+ □ A O2 → □ A H2O+□ A CO2
Transcript text: Question 25 (1 point) Balance the following reaction by filling in the blanks below. Pay attention that this combustion reaction has an oxygen in the carbon reactant. For this one, do not balance it with fractions. Make sure your equation matches this equation. (If you reverse the products on your paper from what is written here, the program will not know you've done this.) Normally, you would not include a '1' but the program requires something in every blank so include any "1" that is needed. \[ \mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}+\mathrm{O}_{2} \rightarrow \mathrm{H}_{2} \mathrm{O}+\mathrm{CO}_{2} \] $\square$ A $\quad \mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}+$ $\square$ A $\quad \mathrm{O}_{2} \rightarrow$ $\square$ A $\mathrm{H}_{2} \mathrm{O}+\square A / \quad \mathrm{CO}_{2}$
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Solution

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Solution Steps

Step 1: Write the Unbalanced Equation

The given unbalanced chemical equation is: \[ \mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O} + \mathrm{O}_{2} \rightarrow \mathrm{H}_{2} \mathrm{O} + \mathrm{CO}_{2} \]

Step 2: Balance the Carbon Atoms

The reactant side has 3 carbon atoms in \(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}\). Therefore, we need 3 \(\mathrm{CO}_{2}\) molecules on the product side to balance the carbon atoms: \[ \mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O} + \mathrm{O}_{2} \rightarrow \mathrm{H}_{2} \mathrm{O} + 3 \mathrm{CO}_{2} \]

Step 3: Balance the Hydrogen Atoms

The reactant side has 6 hydrogen atoms in \(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}\). Therefore, we need 3 \(\mathrm{H}_{2} \mathrm{O}\) molecules on the product side to balance the hydrogen atoms: \[ \mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O} + \mathrm{O}_{2} \rightarrow 3 \mathrm{H}_{2} \mathrm{O} + 3 \mathrm{CO}_{2} \]

Step 4: Balance the Oxygen Atoms

Now, count the oxygen atoms. The product side has \(3 \times 2 = 6\) oxygen atoms from \(\mathrm{CO}_{2}\) and \(3 \times 1 = 3\) oxygen atoms from \(\mathrm{H}_{2} \mathrm{O}\), totaling 9 oxygen atoms. The reactant side has 1 oxygen atom in \(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}\), so we need 8 more oxygen atoms from \(\mathrm{O}_{2}\). Therefore, we need 4 \(\mathrm{O}_{2}\) molecules: \[ \mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O} + 4 \mathrm{O}_{2} \rightarrow 3 \mathrm{H}_{2} \mathrm{O} + 3 \mathrm{CO}_{2} \]

Final Answer

The balanced chemical equation is: \[ \boxed{1 \, \mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O} + 4 \, \mathrm{O}_{2} \rightarrow 3 \, \mathrm{H}_{2} \mathrm{O} + 3 \, \mathrm{CO}_{2}} \]

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