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Now we will examine a more complex system. Watch the animation portraying the combustion of propane. The unbalanced chemical equation is given below.

[tex]\[ \_ C_3H_8(g) + \ldots O_2(g) \rightarrow \text{CO}_2(g) + \ldots H_2O(l) \][/tex]

Begin by balancing an element that appears in the fewest different formulas. What coefficient must be added to the [tex]\(\text{CO}_2\)[/tex] to balance the element C?

[tex]\[ \square \][/tex]

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GinnyAnsweridn
To balance the given chemical equation for the combustion of propane [tex]\( \text{C}_3\text{H}_8 \)[/tex], follow these steps:

1. Identify the unbalanced chemical equation:
[tex]\[ \_ \text{C}_3\text{H}_8 (g) + \ldots \text{O}_2 (g) \rightarrow \_ \text{CO}_2 (g) + \ldots \text{H}_2\text{O} (l) \][/tex]

2. Balance the carbon (C) atoms:
- Propane ([tex]\(\text{C}_3\text{H}_8\)[/tex]) has 3 carbon atoms.
- To balance the carbon atoms, we need an equal number of carbon atoms on the product side.
- Each molecule of [tex]\(\text{CO}_2\)[/tex] contains one carbon atom.

3. Determine the coefficient for [tex]\(\text{CO}_2\)[/tex]:
- Since there are 3 carbon atoms in propane, we need 3 molecules of [tex]\(\text{CO}_2\)[/tex] to balance the carbon atoms.

Thus, the coefficient for [tex]\(\text{CO}_2\)[/tex] is [tex]\(\boxed{3}\)[/tex].

With this coefficient, the partially balanced equation becomes:
[tex]\(\text{C}_3\text{H}_8 (g) + \ldots \text{O}_2 (g) \rightarrow 3 \text{CO}_2 (g) + \ldots \text{H}_2\text{O} (l)\)[/tex].
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