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amylumey2005
20.07.2019 •
Chemistry
The reaction ag+(aq) + cl−(aq) ↔ agcl(s) has an equilibrium of 1020 (keq = 1020). if you have a beaker containing 1 liter of water with 0.1 mol of agcl(s) in it along with 10−6 m ag+(aq) and 10−15 m cl−(aq), how does the reaction shift?
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Ответ:
so, Q = [Ag]*[Cl-] and we neglected [AgCl] as it is solid
∴ Q = 10^-6 * 10^-5
= 10^-11
now we will compare the value of Q with the value of Keq:
when Q = Keq so, the system is in equilibrium
and when Q > Keq so, the reaction will go forward (shift to right) to achieve equilibrium.
and when Q< Keq so, the reaction will go left (shift to left) to achieve equilibrium.
when Q = 10^-11 and Keq = 10^20
∴Q< Keq
and the reaction will shift to left.
Ответ: