I strongly suggest you find the caps key and use it. If you are working on equilibrium problems SURELY you've had enough chemistry to know that lower case and upper case mean something different. See CO, Co, co. You have used m; I assume that should be M since you didn't find the caps key for anything else. m = molality; M = molarity.
Your Q is ok and K is ok. Q<K which means the reaction will shift to the right upon addition of the extra F2.
So how much F2 is added? Whatever 0.200 ml means. Convert that value, whatever it is, to molarity = M.
The new equilibrium is this.
.........H2 + F2 ==> 2HF
E(old)..0.05..0.01...0.400
I....0.0500..0.0100..0.400
add........0.200ml converted to M.
C.......-x....-x.....+2x
E...0.05-x...(?-x)...0.4+2x
Plug the E line into the Keq expression and solve for x, then evaluate the other concentrations.
Post your work if you get stuck.
the following reaction occurred at 45 degrees
all gases h2+f2=2hf
the equlibrium conc in a 5ml container are h2=.0500m, f2=.0100m and hf =.400m. if .200ml of f2 is added calculate the concentrations and pressures of all gases once equlibrium is rfeestablished
q = [hf]^2/[h2][f2]=.4^2/(.05)(.21)=15.238
k=[hf]/[h2][f2]= .4^2/(.05)(.01)=320
then i am lost
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