Chem reaction yield

  • Thread starter Pengwuino
  • Start date
  • #1
Pengwuino
Gold Member
5,124
17
Ok so this problem pissed me off to no end... basically because ih ad 5 minutes to do it and couldn't figure it out.

Consider the following unbalanced reaction:

P4(s) + F2(g) -----> PF3(g)

How many grams of F2 are needed to produce 120. g of PF3 if the reaction has a 84.6 % yield?

Now, i divided the 120g by the molar mass of PF3 and divided by .846 to find the actual amount necessary which gave me 1.612449659 moles. Multply that by the molar mass of F2 and i get 61.26663726. Wasn't correct, wasn't even a matter of significant figures... what went wrong here :D
 

Answers and Replies

  • #2
whozum
2,221
1
Did you remember to balance the equation?
 
  • #3
Pengwuino
Gold Member
5,124
17
oh damn it. They were constantly giving me pre-balanced equations and having to do this so i never noticed that they gave me an unbalanced equation...
 
  • #4
whozum
2,221
1
It says it right there jackass :wink:
 

Suggested for: Chem reaction yield

Replies
2
Views
441
  • Last Post
Replies
6
Views
415
  • Last Post
Replies
3
Views
362
  • Last Post
Replies
3
Views
784
Replies
10
Views
669
Replies
33
Views
359
Replies
2
Views
294
Replies
7
Views
565
Replies
3
Views
603
Top