Consider the reversible reaction A ( g ) − ⇀ ↽ − B ( g ) Which K values would indicate that there is more B than A at equilibrium? K = 9 × 10 – 5 K = 0.4 K = 5000 K = 8 × 10 7

5000 and indicate that there is more B than A at equilibrium

Explanation:

For the given reaction:

where [B] and [A] represents equilibrium concentration B and A respectively. K represents equilibrium constant

More B than A at equilibrium means, [B] > [A]

So,

As, both 5000 and are greater than 1 therefore these two K values indicate that there is more B than A at equilibrium

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