Answer
Balanced equation:
$C_3H_4(g) + 4O_2(g) -^{\Delta}-\gt 3CO_2(g) + 2H_2O(g) $
Reaction type: Combustion.
Work Step by Step
$C_3H_4(g) + O_2(g) -^{\Delta}-\gt CO_2(g) + H_2O(g) $
1. Balance the number of carbon atoms, by putting a "3" in front of $CO_2$.
$C_3H_4(g) + O_2(g) -^{\Delta}-\gt 3CO_2(g) + H_2O(g) $
2. Balance the number of hydrogen atoms, by putting a "2" in front of $H_2O$.
$C_3H_4(g) + O_2(g) -^{\Delta}-\gt 3CO_2(g) + 2H_2O(g) $
3. There is a total of 8 oxygen atoms on the products side. Balance the number of oxygen atoms, by putting a "4" in front of $O_2$.
$C_3H_4(g) + 4O_2(g) -^{\Delta}-\gt 3CO_2(g) + 2H_2O(g) $
4. Classify the reaction.
That reaction follows the pattern for a combustion. Where a carbon-containing compound reacts with oxygen gas to produce carbon dioxide and water.
