I'm so sorry to bother you guys again! Stuck on two other questions:

1. In the following equilibrium: NaCl(s) Na+(aq) + Cl–(aq),
would adding more NaCl(s) increase the Cl-(aq) concentration? Explain why.
My thoughts:
I thought that it wouldn't increased the Cl- concentration because a saturated solid means that the maximum amount of NaCl can be dissolved is present, meaning that it cannot dissolve any further to create Cl- ions.

2. Considering only the NO2-N2O4 equilibrium and assuming the NO2-N2O4 reaction attains equilibrium in smog, predict whether you would expect the sky of Los Angeles to appear "dirtier" on a day when the temperature is l00 ˚F, or on a 65 ˚F day (assume the same total amount of NO2-N2O4 is in the air on both days). Justify your answer.
My thoughts: This is an exothermic reaction. Heating this would shift the equilibrium to the left, to absorb the heat. The heating or temperature increase generates a higher concentration of NO2, which is a darker brown. This means that on days of higher temperature (like 100 degree F) that the sky will appear "dirtier."

I like most of your explanation for #1 but I would change slightly to note that equilibrium means there is at least 1 molecule of NaCl(solid) present. Then

adding more solid NaCl only means more solid NaCl is sitting in the bottom of the flask but no more dissolves. Fit that into what you have written.

2. See here.http://chemed.chem.purdue.edu/demos/main_pages/21.1.html

1. In the given equilibrium: NaCl(s) ⇌ Na+(aq) + Cl–(aq), adding more NaCl(s) would not increase the Cl–(aq) concentration. This is because the system is at equilibrium, which means that the forward and reverse reactions are occurring at equal rates. Adding more NaCl(s) will disturb the equilibrium and cause the system to try to restore it. According to Le Chatelier's principle, when you add more of a reactant, the system shifts in the direction that consumes the excess. In this case, adding more NaCl(s) would shift the equilibrium towards the right, consuming more NaCl(s) to form more Na+(aq) and Cl–(aq). As a result, the concentration of NaCl(s) would decrease, but the concentrations of Na+(aq) and Cl–(aq) would increase to restore the equilibrium. Therefore, adding more NaCl(s) would not directly increase the Cl–(aq) concentration.

2. In the NO2-N2O4 equilibrium, the reaction is represented as: 2NO2(g) ⇌ N2O4(g). When the temperature increases, it causes the equilibrium to shift in the exothermic direction (to the left) in order to absorb the excess heat. This is because the forward reaction is exothermic, meaning it releases heat, while the reverse reaction is endothermic, meaning it absorbs heat.

Based on the information provided, we can conclude that Los Angeles would appear "dirtier" on a day when the temperature is 100 ˚F compared to a day when the temperature is 65 ˚F. This is because at higher temperatures, the equilibrium shifts to the left, favoring the formation of more NO2(g), which is a darker brown color. Therefore, with a higher concentration of NO2(g), the sky would appear "dirtier" on a hotter day.