How many liters of water vapor can be produced if 102 grams of methane gas (CH4) are combusted at 315 K and 1.2 atm? Show all of the work used to solve this problem.

CH4 (g) + 2 O2 (g) yields CO2 (g) + 2 H2O (g)

Question

How many liters of water vapor can be produced if 102 grams of methane gas (CH4) are combusted at 315 K and 1.2 atm? Show all of the work used to solve this problem.

CH4 (g) + 2 O2 (g) yields CO2 (g) + 2 H2O (g)

matt101 · Answer

STEP #1: To know how much H2O is produced, we need to know how much CH4 reacted. You're given the mass of CH4, so you can use that to find out how many moles of CH4 you're working with.

STEP #2: Based on the chemical reaction, you can see that for however much CH4 reacts, TWICE as much H2O is produced. That means the moles of H2O produced is DOUBLE the moles of CH4 reacted.

STEP #3: Use PV=nRT along with the moles of H2O you just found and the other information given in the question to solve for V!