How many liters of methane gas (CH4) need to be combusted to produce 12.4 liters of water vapor, if all measurements are taken at the same temperature and pressure? Show all of the work used to solve this problem

Question

sweetburger · Answer

first set up the balanced reaction

joannablackwelder · Answer

Do you know how to set up the reaction of the combustion of methane?

joannablackwelder · Answer

@princesspenny ?

anonymous · Answer

No, how?

joannablackwelder · Answer

Combustion of a hydrocarbon is always of the form hydrocarbon + O2 -> CO2 + H2O

joannablackwelder · Answer

So, for this case, CH4 + O2 -> CO2 + H2O is the unbalanced reaction. Can you balance it?

anonymous · Answer

$$CH4 + 2 O2 \rightarrow CO2 + 2 H2O$$

anonymous · Answer

is that right?

joannablackwelder · Answer

Sweet! :)

joannablackwelder · Answer

Now, any ideas on what you need to do next?

anonymous · Answer

No idea

joannablackwelder · Answer

Ok, start with what you are given and use conversion factors you know. Since we are at the same temp and pressure, the conversion factor will be the same both ways so it will cancel out. We can use the conversion factor for STP, which is 1 mol of ideal gas = 22.4 L

joannablackwelder · Answer

So, we essentially need to start with L of water vapor, convert to mol of water vapor, convert to mol of methane, and then to L of methane. Make sense?