Final answer:
The question appears to be based on a confusion or typo, because under complete combustion conditions, butane reacts with oxygen to produce carbon dioxide and water, not carbon monoxide. Therefore, based on the reaction given, 0 moles of CO would be produced from 3 moles of C4H10.
Step-by-step explanation:
The question is asking for the amount of carbon monoxide (CO) that could be produced from the complete reaction of 3 moles of butane (C4H10) with excess oxygen (O2). However, the reaction provided (C4H10 + O2 → CO2 + H2O) does not produce CO; it produces carbon dioxide (CO2) and water (H2O). This might be a misunderstanding in the original question, since the expected products of the complete combustion of butane are indeed CO2 and H2O, and not CO.
As a result, based on the complete combustion reaction provided, if 3 moles of C4H10 are reacted, one would calculate the moles of CO2 produced, not CO. If the student intends to find the amount of CO instead (assuming incomplete combustion or an error in the provided products), additional information or a different reaction equation would be necessary.
In a stoichiometric analysis involving complete combustion of hydrocarbons, carbon monoxide is not typically a product without specifying conditions for incomplete combustion. Therefore, given the reaction provided, no moles of CO would be produced; the expected products would strictly be CO2 and H2O.