Question

the equilibrium constant K for a certain reversible reaction is 1.32 × 10−4. Which of the following is true for the reaction? The reverse reaction is more favorable than the forward reaction. The forward reaction takes place at a much faster rate than the reverse reaction. The equilibrium reaction mixture will have a very low concentration of reactants. The equilibrium reaction mixture will have a very high concentration of products.

Answer 1

Answer:

The reverse reaction is more favourable than the forward reaction.

Explanation:

The value of equilibrium constant in this case is  $1.32 \times 10 ^-^4 (0.000132)$.  A high value of equilibrium constant indicates that the forward reaction is more favourable.  

Thus the resultant of the reaction will have higher concentration of products.  When the value of equilibrium constant is less the reverse reaction will be more favoured than the forward reaction.

Thus the resultant of the reaction will have more reactants than products. Here equilibrium constant has a very low value which favours reverse reaction.