At 298K, the molar equilibrium concentrations of Ag+, NH3 and [Ag(NH3)2]+ for the equilibrium Ag+(aq) + 2NH3(aq) ⇌[Ag(NH3)2]+(aq) were found to be 10-1, 10-3, and 10-1 respectively. The value Kc is

Kc = AgNH32+Ag+NH32=10-110-1×10-6=106

At 298K, the molar equilibrium concentrations of Ag+, NH3 and [Ag(NH3)2]+ for the equilibrium Ag+(aq) + 2NH3(aq) ⇌[Ag(NH3)2]+(aq) were found to be 10-1, 10-3, and 10-1 respectively. The value Kc is

Kc = AgNH32+Ag+NH32=10-110-1×10-6=106

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At 298K, the molar equilibrium concentrations of Ag⁺, NH₃ and [Ag(NH₃)₂]⁺ for the equilibrium Ag⁺_(aq) + 2NH_3(aq) $⇌$ [Ag(NH₃)₂]⁺_(aq)were found to be 10^-1, 10^-3, and 10^-1 respectively. The value K_c is

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10⁶

10^-6

5 $\times$ 10⁴

2 $\times$ 10^-3

answer is A.

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K_c = $\frac{{[Ag {({NH}_{3})}_{2}]}^{+}}{{[Ag]}^{+} {[{NH}_{3}]}^{2}}$

= $\frac{10^{- 1}}{10^{- 1} \times 10^{- 6}}$ =10⁶

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At 298K, the molar equilibrium concentrations of Ag+, NH3 and [Ag(NH3)2]+ for the equilibrium Ag+(aq) + 2NH3(aq) ⇌[Ag(NH3)2]+(aq) were found to be 10-1, 10-3, and 10-1 respectively. The value Kc is

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At 298K, the molar equilibrium concentrations of Ag⁺, NH₃ and [Ag(NH₃)₂]⁺ for the equilibrium Ag⁺_(aq) + 2NH_3(aq) $⇌$ [Ag(NH₃)₂]⁺_(aq)were found to be 10^-1, 10^-3, and 10^-1 respectively. The value K_c is