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Need help with an "equilibrium constant" lab report

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hmx9123:
"mol FeNCS2+ (equilibrium) = mol Fe3+ (reacted) --(because of the 1:1 ratio)"

This is correct.  Now, to figure out how much Fe+3 reacted, you use X.  Your X value is the amount that reacted.  The rest of your calculations seem in order from what you posted.  Good luck!

meme:
okay, one last question (I promise!)

Since you said that .17 was too large a value in the beginning since you thought it was moles... is it still too big if its .17M?

hmx9123:
Unless you're evaporating a lot of the solution down, it's way too big.  If you start with .5 mols of each reactant and they react in a 1:1 ratio, how can you get 20 mols back?  In your case, you've got two concentrations that are abysmally small and you're getting something back that is nearly 4 orders of magnitude that size.

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