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    Finding Equilibrium Constant and Delta G

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    Part 1:
    Ammonia can be produced by the reaction of hydrogen gas and nitrogen gas, as shown below:

    N2(g) + 3H2(g) → 2NH3(g)

    Given that the standard free energy of formation (∆Gof) of NH3 (g) is -111 kJ/mol at 335 K, calculate the equilibrium constant, K, at this temperature.
    To express an answer in exponential notation, use E to indicate the exponent. For example, 3.0 x 103 would be written, 3.0E3.

    Part 2:
    In the previous question, you had to calculate the the standard Free Energy Change (∆Go) in order to solve for the equilibrium constant, K, for the reaction:

    N2(g) + 3H2(g) → 2NH3(g)

    This is the Free Energy measured under standard conditions, when the reaction is started with 1.0 M of each of the three gases present. Calculate the non-standard Free Energy change (∆G) at 298 K, given the following non-standard initial concentrations of the three gases (Answer in kJ).
    ∆Gfo = -16.6 kJ/mol for NH3 (g) at 298 K

    initial concentration (M)
    N2 1.0
    H2 0.09
    NH3 4.1

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    Solution Preview


    here is the answer

    Part A
    The relation between standard free energy change and equilibrium constant is
    ∆G_°=-2.303RT ...

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