Consider the following equilibrium: Ag+(aq) 2 NH3(aq) [Ag(NH3)2]\"(aq) AH =-15 k

Question

Consider the following equilibrium: Ag+(aq) 2 NH3(aq) [Ag(NH3)2]"(aq) AH =-15 kJ + - How does each of the following situations affect the position of the equilibrium? 1. Dissolving AgNO, in the solution. (Remember that metal nitrates are fully soluble in water 2. and will dissociate upon dissolving: M,(NO3)y(s) xMn+(aq) + yNO3"(aq).) Bubbling NH, (g) into the solution. (Remember that NH, gas is soluble in water.) Heating the solution. . Dissolving NaCl in the solution, given the following information: AgClo Ag'(a) + Cl(aq Ke 1.8 x 1010

Explanation / Answer

Solution :-

Ag^+(aq) + 2NH3(aq) ----- > [Ag(NH3)2]^+                     Delta H = -15 kJ

1)Dissolving AgNO3in the solution= When the AgNO3 is dissolved in the solution then it will give Ag+ ions so it increases the concentration of the reactant side therefore the equilibrium will shift to the right side to form more complex.

2) Bubbling NH3 causes the increase in the concetration of the NH3 so this means increasing the reactant concentration so equilibrium will shift to the right side.

3)Heating the solution will cause the equilibrium so shift to the left side because the reaction is exothermic so increasing temperature will shift equilibrium to left side.

4) Dissolving the NaCl in the solution gives the Cl- ions these ions combine with Ag+ to form solid AgCl so the reaction will shift to the left side because the addition of the NaCl causes the decrease in the concentration of the Ag+

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