Chemistry

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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)

  • Chemistry -

    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.

  • Chemistry -

    Never mind I figured it out

  • Chemistry -

    ths results cm 4rm table..products/reactants..(84)^2/(416)^2(416)^2

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