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ne”> 5.ne”> 5. Equilibrium constants a) [Cd(H2O)6]2+ + en ⇔ [Cd(en)(H2O)4]2+ + 2 H2O log K = 5.84 b) [Cd(H2O)6]2+ + 2 NH3 ⇔ [Cd(NH3)2(H2O)4]2+ + 2 H2O log K = 4.95 The equilibrium constant for reaction a is approximately 10-fold greater than that of reaction b. Please rationalize this difference and explain the underlying effect in terms of the enthalpic and entropic changes of the reaction.constants a) [Cd(H2O)6]2+ + en ⇔ [Cd(en)(H2O)4]2+ + 2 H2O log K = 5.84 b) [Cd(H2O)6]2+ + 2 NH3 ⇔ [Cd(NH3)2(H2O)4]2+ + 2 H2O log K = 4.95 The equilibrium constant for reaction a is approximately 10-fold greater than that of reaction b. Please rationalize this difference and explain the underlying effect in terms of the enthalpic and entropic changes of the reaction.

/in /by

ne”> 5. Equilibrium

constants

a) [Cd(H2O)6]2+ + en ⇔ [Cd(en)(H2O)4]2+ + 2 H2O log K = 5.84

b) [Cd(H2O)6]2+ + 2 NH3 ⇔ [Cd(NH3)2(H2O)4]2+ + 2 H2O log K = 4.95 The equilibrium constant for reaction a is approximately 10-fold greater than that of reaction b. Please rationalize this difference and explain the underlying effect in terms of the enthalpic and entropic changes of the reaction.

 
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