Answer
Balanced equation:
$C_4H_8(g) + 6O_2(g) --\gt 4CO_2(g) + 4H_2O(g)$
Reaction type: Combustion.
Work Step by Step
1. Count the atoms of each element in both sides of the reaction.
$C_4H_8(g) + O_2(g) --\gt CO_2(g) + H_2O(g)$
Reactants: $C = 4$, $H = 8$ and $O = 2$
Products: $C = 1$, $H = 2$ and $O = 3$
2. Balance the number of carbons, by putting a "4" in front of $CO_2$.
$C_4H_8(g) + O_2(g) --\gt 4CO_2(g) + H_2O(g)$
3. Balance the number of hydrogens, by putting a "4" in front of $H_2O$
$C_4H_8(g) + O_2(g) --\gt 4CO_2(g) + 4H_2O(g)$
4. There is a total of 12 oxygens on the products side. Put a "6" in front of $O_2$ to balance that element.
$C_4H_8(g) + 6O_2(g) --\gt 4CO_2(g) + 4H_2O(g)$
5. Classify the reaction.
That reaction follows the pattern of a combustion. Where a carbon-containing compound reacts with oxygen gas, to produce carbon dioxide and water.
