Question

The following equation shows the correct molecules formed in the reaction, but the products are incorrect. CH4 +2O2 → H2O + CO2 How would you correct the products? Explain your reasoning

Answer 1

The reaction shows the burning of methane in presence of oxygen gas. The products formed as a result of burning will be carbon dioxide and water. However, in the given reaction, the stochiometric constants for the products are incorrect.

CH4 +2O2 → H2O + CO2, there are 4 atoms of hydrogen present in methane but only 2 are present in water. To balance this, we put 2 in front of water. Hence 2 molecules of water will be formed in the combustion of methane.

Answer 2

What you have to do here is to balance the equation.

To do this, you need to have the same amount of atoms on each side of the equation.

Here, they give you a hint saying you have TWO molecules of oxygen.

Gases, like oxygen, when they are alone the molecule is double atom to be stabilized.

In this case, what you need to do is to put TWO molecules of water H2O to balance it.