Turn on thread page Beta
    • Thread Starter
    Offline

    11
    ReputationRep:
    Hi guys, just doing some summer work but I'm a bit stuck on method.

    I've got a whole sheet of questions like this:

    Work out the actual number of moles of each species present at equilibrium

    N2 + 3H2 -----> 2NH3
    Initial Moles 1 1 0 - respectively
    Equ. Moles 0.8 (of the N2)

    In terms of approaching this question using the method found in my textbook/notes, I would say the eq. moles of the H2 is 0.4 (1-3(0.2)) and the Eq moles of NH3 is 0.4 (2 x 0.2)

    But then the moles don't add up...?

    Do I use this method, or will the Eq. moles of NH3 be 0.8 as 0.8 moles are subtracted from the L.H.S?

    Thanks!!
    Offline

    19
    Yeah, the method described in the text book is correct - the total number of moles of molecules can change, but the overall mass can't change

    For example you can split Cl2 with light to form 2Cl. so one mole of chlorine molecules gives two moles of chlorine atoms.
    • Thread Starter
    Offline

    11
    ReputationRep:
    (Original post by EierVonSatan)
    Yeah, the method described in the text book is correct - the total number of moles of molecules can change, but the overall mass can't change

    For example you can split Cl2 with light to form 2Cl. so one mole of chlorine molecules gives two moles of chlorine atoms.
    Ah of course!

    Yeah, just thought I'd check that out!

    Thanks!
 
 
 
Reply
Submit reply
Turn on thread page Beta
Updated: July 20, 2009

1,779

students online now

800,000+

Exam discussions

Find your exam discussion here

Poll
Should predicted grades be removed from the uni application process

The Student Room, Get Revising and Marked by Teachers are trading names of The Student Room Group Ltd.

Register Number: 04666380 (England and Wales), VAT No. 806 8067 22 Registered Office: International House, Queens Road, Brighton, BN1 3XE

Write a reply...
Reply
Hide
Reputation gems: You get these gems as you gain rep from other members for making good contributions and giving helpful advice.