Anonymous
Anonymous asked in Science & MathematicsChemistry · 2 years ago

Calculate K for the following reaction: 2 A ⇌ 3 D given the following K values: A ⇌ ½ B + C K1 = 85.90 3 D ⇌ B + 2 C K2 = 1.17?

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  • 2 years ago
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    Calculate K.....

    2A <==> 3D

    A <==> ½B + C .............. K1 = 85.90

    3D <==> B + 2C ............. K2 = 1.17

    B + 2C <==> 3D ............. K3 = 1/K2 = 0.855

    2A <==> B + 2C ............. K4 = 7379

    2A <==> 3D .................... K5 = K3 x K4 = 6310

    From:

    K3 x K4 = ([D]³ / ([B][C]²)) x ([B][C]² / [A]²) = [D]³ / [A]²

  • 2 years ago

    Double equation 1. When you double the equation, you square the value of K:

    2A <--> B + 2C K1 = 7379

    Flip equation 2 over. When you flip an equation, you invert K.

    B + 2C <--> 3D K2 = 0.855

    Now, when you add those two equations and simplify, you get the desired equation. When you add two equations together, you multiply their individual equilibrium constants. So:

    2A <--> 3D K3 = K1 X K2 = 6.31X10^3

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