The equation for propane burning to form carbon dioxide and water is: C_(3)H_(8)+5O_(2)arrow 3CO_(2)+4H_(2)O If the amount of avallable oxygen is reduced due to limited ventilation, carbon monoxide (CD) is also produced by the reaction: C_(3)H_(8)+4O_(2)arrow CO_(2)+[]CO+4H_(2)O Balance this reaction by selecting the correct coefficient for CO on the pr product side of the equation A 1 B 2 C 3 D 4

To balance the chemical equation for the reaction of propane with oxygen to produce carbon dioxide, water, and carbon monoxide, we need to ensure that the number of atoms of each element is the same on both sides of the equation. The given equation is:<br /><br />\[ C_{3}H_{8} + 4O_{2} \rightarrow CO_{2} + []CO + 4H_{2}O \]<br /><br />We know that there are 3 carbon atoms in propane, so we need 3 carbon atoms on the product side. We already have 1 carbon atom in the carbon dioxide molecule, so we need to find the coefficient for CO that will give us the remaining 2 carbon atoms.<br /><br />The coefficient for CO should be such that the total number of carbon atoms on the product side is equal to the number of carbon atoms in the reactant propane molecule. Since there are 3 carbon atoms in propane and 1 carbon atom in the carbon dioxide molecule, the coefficient for CO should be 2 to balance the carbon atoms.<br /><br />Therefore, the balanced equation is:<br /><br />\[ C_{3}H_{8} + 4O_{2} \rightarrow 3CO_{2} + 2CO + 4H_{2}O \]