# Given this reaction: CH_4 + 2O_2 -> CO_2 + H_2O, 16 g of CH_4 react with 64 g of O_2, producing 44 g of CO_2. How many grams of water are produced?

Nov 29, 2016

$36$ grams of water will get formed.

#### Explanation:

There are actually two methods of doing it - stoichimetry & also with the help of law of conservation of mass.

First by stoichiometry:

$16$grams of $C {H}_{4}$ means $1$mole of it.

Now, after balancing the entire equation we get:

$C {H}_{4} + 2 {O}_{2} \rightarrow C {O}_{2} + 2 {H}_{2} O$.

So, 1 mole of methane produces 2 moles of water. Hence, $36$ grams of water is formed.

Now by law of conservation of mass:

The entire mass of the reactants will be equal to the entire mass of the products after the reaction.

So, mass of water formed $= \left(16 + 64\right) - 44$ grams, i.e. $36$ grams.