[MnJo5h]

 C2H4Br2(aq) + 3 I- (aq) --> C2H4 (aq) + 2 Br- (aq) + I3- (aq)

Find the Keq value, if 1.0 L flask originally containing 1.0 mol of C2H4Br2 and 2.0 mol of I- is found to have a concentration of 0.50 M I- at equilibrium.

[UG]

What have you tried so far? Can you write an expression for K_eq?

[MnJo5h]

I really don't know i kept messing it up got 3 different version of the answer i really just don't feel like dealing with it and would like a solutions so i know how to do it in the future

[UG]

Work with me here, to start these problems, you need an expression for the equilibrium constant, or K_eq as the question mentions, note that for a general reaction

aA + tT  cC + dD

where a, t, c and d are the stoichiometric coefficients of the reactants, and A, T, C and D are the chemical species involved. For example, the stoichiometric coefficient for I^- in your equation is 3.
For this general equation, the equilibrium expression is K_eq = [C]^c[D]^d / [A]^a[T]^t where the [] indicates the concentration
Now if you were to apply this to your question, what would be the expression for K_eq?

[MnJo5h]

Still really have no idea just started chem, and the class was givin this as more of a fun question, im really lost in it

[UG]

Hmmm...ok, lets just say I was in a good mood and I wrote the expression for you:

K_eq = [I₃^-][Br^-]²[C₂H₄] / [I^-]³[C₂H₄Br₂]

Do you know how to set up an ICE table or find the concentration of the products and reactants at equilibrium?

[billnotgatez]

@MnJo5h
Please read forum rules
Spoon feeding answers here is frowned on