Hi everyone!
My Chem teacher posted this question on our Google Classroom but I'm kind of confused on how to do it heh. How would you guys solve this?
When 2.45 mol of N2(g) and 1.83 mol of H2(g) are mixed in a 3.00L vessel the following reaction takes place:
N2(g) + 3H2(g) <=> 2NH3(g). When equilbirum is reached it was found that there is 0.423mol of NH3. Determine the equilibium constant of the reaction at this temperature and post it, including units with correct significant figures (of course we can't use subscripts and superscripts).
So this is asking you to the the equailibrium constant K
c. The best way to find this is to set up an ICE table.
I= Inital amount (products are 0)
C= is the change you are going to see and is repersented by x
E= is the amount (in mol) at quailibrium
So lets set it up:
Fill out the table with the infomation you have.
No we need to find the C and E for everything.
The C, is what has changed. Reactants (N2 and H2) will loss mass so it will be -x, but if it has a coefficient like 3H2 does, it becomes -3x. For the products since it will gain mass, it will be +x
Lets add this to the table:
Now we need to work out the mole after equailbrium for N2 and H2.
As we can see, we have all the info in the NH3 colum to work out X.
2X=0.423
X=0.2115
So we can use this to find out info in the other tables.
To work out N2, 2.45-X,
So, 2.45-0.2115 = 2.2385.
To work out H2, 1.83- 3X
1.83- 3(0.2115) = 1.955
So we can no imput this into our table:
No Kc is found from conenctrations, not mol.
So we need to convert the numbers found in the E part of the table.
We use C= n/V
The volume in your question is 3.00 L
So for N2 = 2.2385/3.00 = 0.734
For H2 = 1.955/3.00= 0.652
For NH3 = 0.423/3.00 = 0.141
Now, set up the Kc equation and sub these in+
Kc = [NH2]^2/ [N2] [H2]^3
Sub in, Kc= [0.141]^2 / [0.734] [0.652]^3
Kc = 0.0977
For the unit sub in M to the Kc formula = M^2/ M x M^3 = M^2/ M^4 = M-2
So, Kc = 0.0997 M-2.
(I may be wrong on the units)