Given the following reactions: Ag^{+} + NH_3 | vedclass

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(A) The overall reaction for the formation of $[Ag(NH_3)_2]^+$ is the sum of the two given steps: $Ag^{+} + 2NH_3 \rightleftharpoons [Ag(NH_3)_2]^+$ T

Vedclass · Accepted Answer

$1.088 	imes 10^7$

Vedclass · Answer

(A) The overall reaction for the formation of $[Ag(NH_3)_2]^+$ is the sum of the two given steps: $Ag^{+} + 2NH_3 ightleftharpoons [Ag(NH_3)_2]^+$ The overall equilibrium constant $(K_{overall})$ or formation constant $(K_f)$ is the product of the equilibrium constants of the individual steps: $K_f = K_1 	imes K_2$ $K_f = (1.6 	imes 10^3) 	imes (6.8 	imes 10^3)$ $K_f = 10.88 	imes 10^6 = 1.088 	imes 10^7$

Given the following reactions:
$Ag^{+} + NH_3 \rightleftharpoons [Ag(NH_3)]^+ ; K_1 = 1.6 \times 10^3$
$[Ag(NH_3)]^+ + NH_3 \rightleftharpoons [Ag(NH_3)_2]^+ ; K_2 = 6.8 \times 10^3$
What is the formation constant for $[Ag(NH_3)_2]^+$?

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Given the following reactions: $Ag^{+} + NH_3 \rightleftharpoons [Ag(NH_3)]^+ ; K_1 = 1.6 \times 10^3$ $[Ag(NH_3)]^+ + NH_3 \rightleftharpoons [Ag(NH_3)_2]^+ ; K_2 = 6.8 \times 10^3$ What is the formation constant for $[Ag(NH_3)_2]^+$?