Question

A sealed 1.0L flask is charged with .500mol I2 and .500mol Br2 and an equilibrium reaction esues: I2(g)+Br2(g)=2IBr(g)
When the container contents achieve equilibrium, the flask contains .84 mol of IBr. What is the value of the eqilibrium constant? (K)

I2(g)+Br2(g)=2IBr(g)
I .500 .500 0

C -x -x +2x

E .500-x .500-x .84

I know K=[product]/[reactant] but I don't know what to do with the information from there.
Never mind I figured it out
ths results cm 4rm table..products/reactants..(84)^2/(416)^2(416)^2

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