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    Mass of a Molecule

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    50.0 g of N2O4 is introduced into an evacuated 2.00 Litre vessel and allowed to come to equilibrium with its decomposition product, N2O4(g) = 2 NO2(g). For this reaction Kc=0.133. Once the system has reached equilibrium, 5.00 g of NO2 additional is injected in to the vessel, and the system is allowed to equilibrate once again. Calculate the mass of NO2 in the final equilibrium mixture.

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    Solution Preview

    To view this in proper format, cut and paste it into a simple text editor like word pad.... I put in multiple spaces, but when I post this, all the spacing gets messed up... anyway... I will try using multiple (....) for spacing instead.

    First I convert grams of N2O4 to moles... ALWAYS do that!

    Moles N2O4 = 50.0 g/92.01 g/mol = 0.543 mol

    Initial concentration of N2O4 = 0.543 mol/2.00 L = 0.272 M

    And grams of NO2 to ...

    Solution Summary

    The solution provides a detailed, step-by-step calculation for the mass of a molecule in a final equilibrium mixture of a decomposed product.