Question

For the reversible reaction. A(g) = B(g). which K values would indicate that there is more B then A at equilibrium? a)K=7x10^-9. b)K=4000. c)K=0.2. d)K=1x10^6

Answer 1

Answer is both (b) and (d).

Explanation;

Equilibrium constant is written as a ratio between concentrations of products and reactants.

The equilibrium reaction is

A(g) ⇄ B(g)

Hence, the equilibrium constant can be expressed as

K = [B(g)] / [A(g)]

If there is more B, then A should be less. Hence, K value would be more than 1.

Hence, according to the given choices, K = 4000 and K = 1 x 10⁶ can be taken as correct answers.

Answer 2

Well, K values is usually gotten from dividing products with reactant

K   =    B  / A

So if you want to find indications that B is more than A, you should find the answer in which the K is the highest

The answer would be D. K = 1 x 10^6

Hope this helps