# Problem: Imagine you mix 16.05 g of methane (CH4) gas and 96.00 g of oxygen (O2) gas and then ignite the mixture. After a bright flash and a loud bang, some water droplets form on the inside of the reaction vessel.How many moles of carbon dioxide can you make?

###### FREE Expert Solution

We’re being asked to calculate the moles of carbon dioxide, COproduced by the reaction of 16.05 g of methane (CH4) gas and 96.00 g of oxygen (O2) gas.

For this problem, we need to do the following steps:

Step 1: Write and balance a chemical equation for the given reaction.

Step 2: Determine the moles of each reactant from the given mass

Step 3: Determine the limiting reactant and calculate the moles of CO2 formed.

Step 1: From the problem, assuming a complete combustion reaction occurs, the complete reaction is:

CH4 + O2 → CO2 + H2O

This equation is not yet balanced. To balance it, we have to make sure that the number of elements on both sides is equal.

Balance C:C is balanced

CH4 + O2 → CO2 + H2O

Balance H: We have 4 H on the reactant side and 2 H on the product side – add a coefficient of 4 to H2O:

CH4 + O2 → CO2 + H2O

Balance O: We have 2 O on the reactant side and 2 + 8 = 10 O on the product side – add a coefficient of 5 to O2:

CH4 + O2 → CO2 + H2O

###### Problem Details

Imagine you mix 16.05 g of methane (CH4) gas and 96.00 g of oxygen (O2) gas and then ignite the mixture. After a bright flash and a loud bang, some water droplets form on the inside of the reaction vessel.

How many moles of carbon dioxide can you make?