# For the reaction CH_4 + 2O_2 -> CO_2 + H_2O, how many moles of carbon dioxide are produced from the combustion of 100. g of methane?

May 24, 2017

1 mol of methane is 16 grams that produces 6.25 moles of $C {O}_{2}$ when it is burnt

#### Explanation:

1 mol of methane is 16 grams. Therefore, if you have 100 grams of methane, it means that you have $\frac{100}{16} = 6.25$ moles of methane.

When you burn 6.25 moles of methane, you produce 6.25 moles of carbondioxide.

Your reaction is wrong though. I want to correct it.

$C {H}_{4} + 2 {O}_{2} \to C {O}_{2} + 2 {H}_{2} O$

When you burn 6.25 moles of methane, you need 12.5 moles of oxygen gas.

When you burn 6.25 moles of methane, you produce 6.25 moles of carbondioxide (275 grams of $C {O}_{2}$) and 12.5 moles of water vapour (225 grams of ${H}_{2} O$).