Walk me through this
How many liters of water vapor can be produced if 13.3 liters of methane gas (CH4) are combusted, if all measurements are taken at the same temperature and pressure? Show all of the work used to solve this problem.
CH4 (g) + 2 O2 (g) ---CO2 (g) + 2 H2O (g)

Do I use PV = nRT ?

Question

Walk me through this 
How many liters of water vapor can be produced if 13.3 liters of methane gas (CH4) are combusted, if all measurements are taken at the same temperature and pressure? Show all of the work used to solve this problem. 
CH4 (g) + 2 O2 (g) --->CO2 (g) + 2 H2O (g)

Do I use PV = nRT ?

abmon98 · Answer

nope dont use PV=nrt use mole ratio if 1 mole consumed13.3 liters what if 2 moles were used instead therefore 26.6 is produced of water vapour