To determine the products of the unbalanced combustion reaction of butane ([tex]\( \text{C}_4\text{H}_{10} \)[/tex]), we need to consider the general form of combustion reactions for hydrocarbons.
Combustion reactions for hydrocarbons typically follow this pattern:
[tex]\[ \text{Hydrocarbon} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \][/tex]
Given the combustion reaction:
[tex]\[ \text{C}_4\text{H}_{10}( g ) + \text{O}_2( g ) \rightarrow \][/tex]
The products of the complete combustion of a hydrocarbon (in this case, butane [tex]\( \text{C}_4\text{H}_{10} \)[/tex]) are carbon dioxide ([tex]\( \text{CO}_2 \)[/tex]) and water ([tex]\( \text{H}_2\text{O} \)[/tex]).
So, we have:
[tex]\[ \text{C}_4\text{H}_{10}( g ) + \text{O}_2( g ) \rightarrow \text{CO}_2( g ) + \text{H}_2\text{O}( g ) \][/tex]
Therefore, the correct product of the unbalanced combustion reaction is:
[tex]\[ \text{CO}_2( g ) + \text{H}_2\text{O}( g ) \][/tex]
The correct answer is:
B. [tex]\(\text{CO}_2( g ) + \text{H}_2\text{O}( g )\)[/tex]
