given the reaction: agcl(s) +2nh3 (aq) <--> ag (nh3)2 +(aq) + cl^- (aq). if more ammonia, nh3 is added to the system at equilibrium the a) amount of agcl increases b) system cannot achieve equilibrium c) rate of the forward reaction decreases d) concentration of cl^- decreases e) concentration of ag (nh3)2 + (aq) increases. explain
To determine the effect of adding more ammonia (NH3) to the system at equilibrium, let's analyze the given reaction:
AgCl(s) + 2NH3(aq) ⇌ [Ag(NH3)2]+(aq) + Cl^-(aq)
When more NH3 is added to the system, it increases the concentration of NH3, which will disrupt the equilibrium. To understand the impact on the system, we need to consider Le Chatelier's principle.
Le Chatelier's principle states that if a stress is applied to a system at equilibrium, the system will adjust in order to minimize that stress and restore equilibrium.
In this case, adding more NH3 to the system increases its concentration, so it will be considered a stress on the equilibrium. Now, let's examine each option:
a) The amount of AgCl (silver chloride) does not change because AgCl is in the solid state and is not affected by changes in concentration.
b) The system can still achieve equilibrium by adjusting the concentrations of the other species.
c) The rate of the forward reaction does not decrease due to increased ammonia concentration. In fact, the rate of the forward reaction may initially increase due to the increased concentration of NH3.
d) The concentration of Cl^- (chloride ion) does not change because it is a spectator ion. It does not participate in the reaction and remains in solution. Therefore, the concentration of Cl^- remains constant.
e) The concentration of [Ag(NH3)2]+ (silver diammine ion) increases. This is because the increased NH3 concentration shifts the equilibrium towards the products, leading to the formation of more [Ag(NH3)2]+ ions.
Therefore, the correct answer is e) the concentration of [Ag(NH3)2]+ (aq) increases.
When more ammonia (NH3) is added to the system at equilibrium, the equilibrium will shift to the right in order to counteract the change. Let's examine the possible effects of this change on each answer choice:
a) The amount of AgCl increases: No, adding more NH3 does not directly affect the amount of AgCl. The addition of NH3 primarily affects the formation of Ag(NH3)2+ and Cl-.
b) The system cannot achieve equilibrium: No, the system will still achieve equilibrium, but the position of the equilibrium will shift to the right due to the addition of NH3.
c) The rate of the forward reaction decreases: No, the rate of the forward reaction is related to the concentration of reactants (AgCl and NH3) and not influenced by the addition of more NH3.
d) The concentration of Cl- decreases: Yes, adding more NH3 will lead to the formation of more Ag(NH3)2+ ion and Cl- ion. This means that the concentration of Cl- will decrease.
e) The concentration of Ag(NH3)2+ increases: Yes, adding more NH3 will shift the equilibrium to the right, favoring the formation of Ag(NH3)2+ ion. This will lead to an increase in the concentration of Ag(NH3)2+.
Therefore, the correct answers are d) The concentration of Cl- decreases and e) The concentration of Ag(NH3)2+ increases.
You need to locate the caps key on your computer and learn to use it. CO, Co, and co are three different meanings based on the caps key.
Le Chatelier's Principle tells us that a system at equilibrium will try to undo what we've done to it. Adding more NH3 means the system will shift so as to use up the added NH3. That means it will shift to the right.