Questions: Let's start by balancing the following chemical reaction fill in blank C2H5OH(l)+ fill in blank O2(g) → fill in blank. CO2(g)+ fill in blank H2O(g)

Transcript text: Lets start by balancing the following chemical reaction fill in blank $\quad \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l)+$ fill in blank $\quad \mathrm{O}_{2}(\mathrm{~g}) \rightarrow$ fill in blank. $\mathrm{CO}_{2}(\mathrm{~g})+$ fill in blank $\mathrm{H}_{2} \mathrm{O}(\mathrm{g})$

Solution

Solution Steps

Step 1: Write the Unbalanced Chemical Equation

The unbalanced chemical equation for the combustion of ethanol ($\mathrm{C}_2\mathrm{H}_5\mathrm{OH}$) is: \[ \mathrm{C}_2\mathrm{H}_5\mathrm{OH}(l) + \mathrm{O}_2(g) \rightarrow \mathrm{CO}_2(g) + \mathrm{H}_2\mathrm{O}(g) \]

Step 2: Balance the Carbon Atoms

Ethanol contains 2 carbon atoms, so we need 2 $\mathrm{CO}_2$ molecules on the product side: \[ \mathrm{C}_2\mathrm{H}_5\mathrm{OH}(l) + \mathrm{O}_2(g) \rightarrow 2\mathrm{CO}_2(g) + \mathrm{H}_2\mathrm{O}(g) \]

Step 3: Balance the Hydrogen Atoms

Ethanol contains 6 hydrogen atoms, so we need 3 $\mathrm{H}_2\mathrm{O}$ molecules on the product side: \[ \mathrm{C}_2\mathrm{H}_5\mathrm{OH}(l) + \mathrm{O}_2(g) \rightarrow 2\mathrm{CO}_2(g) + 3\mathrm{H}_2\mathrm{O}(g) \]

Step 4: Balance the Oxygen Atoms

Now, count the oxygen atoms on the product side: $2 \times 2$ from $\mathrm{CO}_2$ and $3 \times 1$ from $\mathrm{H}_2\mathrm{O}$, totaling 7 oxygen atoms. Ethanol provides 1 oxygen atom, so we need 6 more from $\mathrm{O}_2$, which means 3 $\mathrm{O}_2$ molecules: \[ \mathrm{C}_2\mathrm{H}_5\mathrm{OH}(l) + 3\mathrm{O}_2(g) \rightarrow 2\mathrm{CO}_2(g) + 3\mathrm{H}_2\mathrm{O}(g) \]

Final Answer

The balanced chemical equation is: \[ \boxed{\mathrm{C}_2\mathrm{H}_5\mathrm{OH}(l) + 3\mathrm{O}_2(g) \rightarrow 2\mathrm{CO}_2(g) + 3\mathrm{H}_2\mathrm{O}(g)} \]

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