Question

if carbon monoxide reaches a temperature of over 1,100 degrees fahrenheit, it will ignite in a combustion reaction with oxygen. what would the product(s) of the reaction be? 2co + o₂ →? 2co₂ c₂ + o₄ 2co + o₂ h₂o

Explanation:

Step1: Analyze the reactants

The reactants are \(2CO\) (carbon monoxide) and \(O_2\) (oxygen). Carbon monoxide is a compound of carbon (\(C\)) and oxygen (\(O\)).

Step2: Consider the combustion reaction

In a combustion reaction of carbon - containing compounds with oxygen, the general rule is that carbon combines with oxygen. For carbon monoxide (\(CO\)), when it reacts with \(O_2\), the carbon in \(CO\) will form a more stable oxide.

Step3: Balance the chemical equation

The un - balanced equation is \(2CO+O_2
ightarrow\). For carbon: we have \(2\) carbon atoms from \(2CO\). For oxygen: we have \(2 + 2=4\) oxygen atoms from \(2CO\) and \(O_2\). If the product is \(CO_2\), let the coefficient of \(CO_2\) be \(x\). By carbon balance: \(x = 2\) (since there are \(2\) carbon atoms in the reactants). By oxygen balance: \(2x=2 + 2\). Substituting \(x = 2\), \(2\times2=4\) (which is correct as there are \(4\) oxygen atoms in the reactants). So the balanced equation is \(2CO+O_2 = 2CO_2\).

• \(C_2+O_4\): Such species (\(C_2\) and \(O_4\)) do not exist as stable products in this reaction. Carbon exists as \(CO_2\) (not \(C_2\)) and oxygen in di - atomic form (\(O_2\)) is the common form, not \(O_4\).
• \(2CO+O_2\): These are the reactants, not the products.
• \(H_2O\): There is no hydrogen (\(H\)) in the reactants (\(CO\) and \(O_2\)), so \(H_2O\) cannot be a product.

Answer:

\(2CO_2\) (the first option)