Consider the following equilibrium: Ag\'(aq) + 2NH_3(aq) = [Ag(NH_3)_2] (aq) del

Question

Consider the following equilibrium: Ag'(aq) + 2NH_3(aq) = [Ag(NH_3)_2] (aq) delta H = -15KJ How does cadi of the following situations..fleet tlic position of the equilibrium. Dissolving AgNO_3 in tlic solution. (Remember that metal nitrates are fully soluabe in water and will dissociate upon dissolving: M_3(NO_3)y (s) rightrarrow xM^n(aq) + yNO_3 (aq).) Bubbling NH_3 (g) into the solution. (Remember that NH_3 gas is soluble in water. Heating the solution. Dissolving NaCL in the solution, given the following information: AgCI_(s) Cl-(aq) K_eq = 1.8 times 10^-10

Explanation / Answer

1. More number of Ag+ ions will be produced sothat concentration of Ag + ions increases hence equilibrium shifts towards right side. i.e., formation of complex

2. Bubbling of NH3 means increasing the concentration of NH3 hence reaction shifts towards right side.

3. The given reation is exothermic since dH = -ve. So if we increase the temperature then energy of produts will become high and rection shifts backward direction

4.Since all the Ag+ is precipitate in the solution hence concentration of Ag+ ions decreases hence reaction shifts in backward direction

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