When 0.63 mol of ethanol (C2H5OH) is combusted, it reacts with oxygen (O2) to produce carbon monoxide (CO) and water (H2O). To find the total moles produced, we first need to consider the balanced chemical equation for the combustion of ethanol under the specified conditions.
The balanced equation for the combustion of ethanol is:
C2H5OH + O2 → CO + H2O
For complete combustion, the balanced equation usually will resemble something like:
C2H5OH + 3O2 → 2CO + 3H2O
However, since the question specifies the production of carbon monoxide and water, we can assume an incomplete combustion reaction where ethanol reacts to form carbon monoxide instead of carbon dioxide:
C2H5OH + O2 → 2CO + 3H2O
From this equation, we can deduce that 1 mole of ethanol produces 2 moles of carbon monoxide and 3 moles of water. This means that:
For every 1 mole of ethanol combusted, a total of 5 moles of products are formed (2 moles CO + 3 moles H2O).
If we have 0.63 mol of ethanol, the total moles of products can be calculated as follows:
Total moles = 0.63 mol C2H5OH × 5 = 3.15 mol of products.
Therefore, when 0.63 moles of ethanol are combusted, a total of 3.15 moles of products (carbon monoxide and water) are produced.