Step 1 :The equilibrium constant for the reaction \(C \rightleftharpoons D\) is given as 0.15.
Step 2 :The equilibrium constant for a reaction is the reciprocal of the equilibrium constant for the reverse reaction.
Step 3 :Therefore, the equilibrium constant for the reaction \(D \rightleftharpoons C\) should be the reciprocal of 0.15.
Step 4 :Calculate the reciprocal of 0.15 to find the equilibrium constant for the reaction \(D \rightleftharpoons C\).
Step 5 :K_reverse = 1 / 0.15 = 6.666666666666667
Step 6 :Round the result to two decimal places.
Step 7 :K_reverse = 6.67
Step 8 :Final Answer: The equilibrium constant for the reaction \(D \rightleftharpoons C\) is \(\boxed{6.67}\).