How many liters of water vapor can be produced if 8.9 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)

Question

How many liters of water vapor can be produced if 8.9 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)

anonymous · Answer

Hint: What is the moles of methane gas combusted?

photon336 · Answer

are you given any other information?

anonymous · Answer

The information is sufficient to solve the problem

simplymarie_x · Answer

I have no idea how to do this at all. But that's all that is given to me. @Photon336 @thushananth01

anonymous · Answer

Moles of a gas = Volume of gas/ molar volume
= 8.9 /24

anonymous · Answer

The ratio of moles between CH4 and H20 = 1 :2

photon336 · Answer

yeah,  this could be based off the fact that 1 mole of every gas occupies 22.4L at STP, then you could easily find out the number of moles from this.

anonymous · Answer

@Photon336 That's right

photon336 · Answer

@simplymarie_x follow what @thushananth01 said and then tell us what you get.

simplymarie_x · Answer

So 8.9/24 = 0.397 moles

then since the ratio is 1:2, I'd do 0.397*2 = 0.794 then I'd have to convert it back to liters so 0.794 * 22.414 giving me an answer of 17.8 L of water vapor?

anonymous · Answer

Divide 8.9 by 22.4 and then use that moles to find moles of water vapor

simplymarie_x · Answer

So I'm not right? Couldn't you also just do the  8.9 liters of methane gas x 2 to get the answer?

simplymarie_x · Answer

which would be 17.8 ? @thushananth01 @photon336

anonymous · Answer

That's right! Good job!

simplymarie_x · Answer

Okay thank you so much! :D

anonymous · Answer

Assuming that it is at standard room temperate and pressure