For the following reaction, the equilibrium constant
KC = 97.0 at 900 K. If the initial concentrations of NH3 and H2S are both 0.20 M, what is the equilibrium concentration of H2S?
H2S (g) + NH3 (g) ---> NH4HS (s)
Make an ICE chart and substitute into Kc and solve.
Could you help me on the ice table..........I could only get the I part :(
I: 0.2 0.2 0
Wait is this right?
I: 0.2 0.2 0
C: -x -x x
E: 0.2-x 0.2-x x
Wait is this right?
I: (0.2) (0.2) (0)
C: (-x) (-x) (x)
E: (0.2-x) (0.2-x) (x)
Now what do I do next once I have the ice table?
Set Kc = (x)(0.2-x)/(0.2-x) .
Solve for x.
0.2-x is H2S equilibrium concentration
Ummmmm I'm waiting to confirm this with DrBob222...Thanks anyways ;D
That looks pretty good.
We can't space on the board; let me show you how to do it. You trick it with periods.
..........NH3(g) + H2S(g) ==> NH4HS(s)
initial....0.2......0.2.........0
change.....-x........-x..........x
equil....0.2-x...0.2-x............
Kc = 97.0 = 1/[(0.2-x)(0.2-x)]
Solve for x. You can do it the long with with the quadratic formula but there is a short way to do it if you notice that the denominator is a perfect square.
initial....0.2......0.2.........0
change.....-x........-x..........x
equil....0.2-x...0.2-x............
equil....0.2-x...0.2-x............ <----what goes here
Did you forget to put an x?????