A community for students.
Here's the question you clicked on:
 0 viewing
anonymous
 3 years ago
How many liters of hydrogen gas are needed to react with cs2 to produce 3.2 liters of ch4 at stp?
anonymous
 3 years ago
How many liters of hydrogen gas are needed to react with cs2 to produce 3.2 liters of ch4 at stp?

This Question is Open

abb0t
 3 years ago
Best ResponseYou've already chosen the best response.1It's absolutely crucial that you are able to write out a BALANCED chemical equation. You have: \[H_{2(g)} + CS_{2(l)} \rightarrow CH_{4(g)}+H_2S_{(g)}\] I'll leave it to you to balance the equation. From the equation, "n" mole H2 is equivalent to 1 mole CH4 22.4 L (at STP) of CH4 is produced from "n"x22.4 L of H2 Hence, _____ L of CH4 will be produced from "n" x ____ L = 1 Thats how you solve. in this case "n" represents mole (which you should be able to get after you balance the chemical equation I gave you).
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.