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March 24, 2017

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The equlibrium constant Kc for the reaction: has the value of 4.00 at 500K. If a mixture of 1.00 mol CO and 1.00 mol H2O is allowed to reach equilibrium at this temperature in a 1.00L flask, calculate the equilibrium concentrations of each species in the flask.

  • Chemistry II - ,

    You should have shown the reaction. I assume it is
    CO(g) + H2O(g) ==>H2(g) + CO2(g)
    If not, just ignore what follows.

    Set up an ICE chart and solve.
    initial:
    CO = 1.00 mol/L
    H2O = 1.00 mol/L
    CO2 = 0
    H2 = 0

    change:
    CO = -x
    H2O = -x
    H2 = x
    CO2 = x

    equilibrium:
    CO = 1-x
    H2O = 1-x
    CO2 = x
    H2 = x

    Post your work if you get stuck.

  • Chemistry II - ,

    Kc=(x)(x)/(1-x)(1-x)

    What is x in this equation and is is 4.0 Kc?

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