Question

The equation for the complete combustion of ethanol is
C2H5OH1+3O2 ---- 2CO2+3H2O
5.0 mole of ethanol is completely burnt in excess oxygen
Calculate the
Moles of C2O produced
Moles of steam produced

Answer 1

To determine the moles of \(CO_2\) and \(H_2O\) produced from the complete combustion of ethanol (\(C_2H_5OH\)), we can use the balanced chemical equation:

\[
C_2H_5OH + 3O_2 \rightarrow 2CO_2 + 3H_2O
\]

From the equation, we can see the following stoichiometric ratios:
- 1 mole of ethanol produces 2 moles of carbon dioxide (\(CO_2\))
- 1 mole of ethanol produces 3 moles of water (\(H_2O\))

Given that we have 5.0 moles of ethanol, we can calculate the moles of \(CO_2\) and \(H_2O\) produced as follows:

### Moles of \(CO_2\) Produced
From the equation:
\[
1 \text{ mole of } C_2H_5OH \rightarrow 2 \text{ moles of } CO_2
\]

Thus, for 5.0 moles of ethanol:
\[
5.0 \text{ moles of } C_2H_5OH \rightarrow 5.0 \times 2 = 10.0 \text{ moles of } CO_2
\]

### Moles of \(H_2O\) Produced
From the equation:
\[
1 \text{ mole of } C_2H_5OH \rightarrow 3 \text{ moles of } H_2O
\]

Thus, for 5.0 moles of ethanol:
\[
5.0 \text{ moles of } C_2H_5OH \rightarrow 5.0 \times 3 = 15.0 \text{ moles of } H_2O
\]

### Summary
- Moles of \(CO_2\) produced: **10.0 moles**
- Moles of \(H_2O\) produced: **15.0 moles**