# 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.Identify the theoretical yields.

###### FREE Expert Solution

We’re being asked to calculate the theoretical yields of the combustion reaction of methane (CH4) 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 limiting reactant and calculate the mass of CO2 formed.

Step 3: Calculate the mass of H2O formed.

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

From the problem, the given combustion 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: We have 1 C on the reactant side and 1 C on the product side – C is balanced

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

CH4 + O2 → CO22 H2O

Balance O: We have 2 O on the reactant side and 2+2 = 4 O on the product side – add a coefficient of 2 to O2

CH4 + O2 → CO22 H2O

Now that we have a balanced equation, we can proceed with the problem. ###### 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.

Identify the theoretical yields.