Given the reaction A+B=C+D, determine the equilibrium constant if .6mol of C are formed when 1.0 mol of A and B are presented initially.

 

cannot find anything close to this in the book or in the notes, im dieing!

Well... is this in solution, or in some other situation?

 

You can start by giving the definition of equilibrium constant. You should be able to work out concentrations based off of the information the problem gives.

Thats just it this is ALL the info the problem gives!

That is all you need. Start by righting out an equation that defines the equilbrium constant and then rearrange for C

for a reaction: [ce]nW + mX -> aY + bZ[/ce]

 

[math] K = \frac{[Y]^{a}[Z]^{b}}{[W]^{n}[X]^{m}} [/math]

 

You can just treat the numbers of moles like they are molarities because if you don't know what the compounds are; solubility obviously isn't an issue. The proportions will still work out the same. You can find the amount of "D" formed very easily. After you get that, the equilibrium constant is just plug and chug.