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# 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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- pisgahchemistLv 72 years agoFavorite Answer
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

- hcbiochemLv 72 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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