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
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."
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