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What is the product of the unbalanced combustion reaction below?

[tex]\[ C_4H_{10}(g) + O_2(g) \rightarrow \][/tex]

A. [tex]\[ C_6H_{12}O_6(s) \][/tex]

B. [tex]\[ CO_2(g) + H_2O(g) \][/tex]

C. [tex]\[ C(s) + H_2O(g) \][/tex]

D. [tex]\[ CO_2(g) + H_2(g) \][/tex]

Sagot :

GinnyAnswer
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]
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