Problem: For the reversible reactionA(g) ⇌ B(g) Which K value would indicate that there is more B than A at equilibrium?A. K = 9x10-9B. K = 0.2C. K = 9000D. K = 9x109

FREE Expert Solution

The equilibrium constant expression is written as:

$K=\frac{products}{reactants}$

$K = \frac{[B]}{[A]}$

For this problem, the expression should look as follows:

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Problem Details

For the reversible reaction

A(g) ⇌ B(g) 

Which K value would indicate that there is more B than A at equilibrium?

A. K = 9x10-9

B. K = 0.2

C. K = 9000

D. K = 9x109

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