A community for students.
Here's the question you clicked on:
 1 viewing
willowdavis97
 2 years ago
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)
willowdavis97
 2 years ago
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)

This Question is Closed

aaronq
 2 years ago
Best ResponseYou've already chosen the best response.1a mole of gas in ideal conditions is 22.414 L you have 8.9L so divide by 22.414L, so you have 0.397 moles in the balanced equation you have a ratio methane:water, 1:2. so you have twice as many moles, 0.397*2= 0.794 moles of H2O vapour, convert that back to Liters by multiplying by 22.414 L and you have 17.8 L of water vapour

aaronq
 2 years ago
Best ResponseYou've already chosen the best response.1you could've just multiplied the amount of litters by 2, but i wanted to show you where it came from
Ask your own question
Sign UpFind more explanations on OpenStudy
Your question is ready. Sign up for free to start getting answers.
spraguer
(Moderator)
5
→ View Detailed Profile
is replying to Can someone tell me what button the professor is hitting...
23
 Teamwork 19 Teammate
 Problem Solving 19 Hero
 Engagement 19 Mad Hatter
 You have blocked this person.
 ✔ You're a fan Checking fan status...
Thanks for being so helpful in mathematics. If you are getting quality help, make sure you spread the word about OpenStudy.