Question: In a laboratory demonstration, a balloon filled with methane and oxygen was exposed to a
flame. The result was a brief, large flame. The students were asked to formulate an equation for
the reaction. One answer is below.
CH, + 0 = CO,
This equation is incorrect.
A. Explain how and why it is incorrect
B. What would the correct equation be, and how do you know that?

The laboratory demonstration consists of the following;

The compounds present in the combustion reaction = Methane, CH₄ and Oxygen, O₂

The chemical equation for the combustion reaction is given as follows;

CH₄ + 2O₂ → CO₂ + 2H₂O

Therefore;

A. The equation given as CH₄ + O → CO₂ is not correct because;

1) Oxygen gas exist as diatomic molecules, O₂, and given that the experiment involves the mixture of gases, the oxygen gas present which can exist as a separate compound, should be represented as O₂

2) The number of oxygen molecules in the reaction is two rather than one

3) The product also includes two molecules of water (vapor) H₂O

B. The correct equation for the reaction should be given as follows;

CH₄ + 2O₂ → CO₂ + 2H₂O

B i) The constituents of the equation is obtained by the knowledge of the fact that the combustion reaction of an organic substance such as methane in the presence of oxygen yields, carbon dioxide and water (vapor)

The equation showing the relative amounts the reacting compounds is by balancing the basic equation of the combustion of methane in the presence of oxygen

Explanation:

D. The number of atoms present

Explanation:

In a balanced equation, coefficients always represent the number of atoms present.