@Frigidcold He’s talking about k, the rate constant, not K, the equilibrium constant.
@Xurian - My AP class didn’t even prepare me for the AP 
Honestly, this year was pretty much just a repeat of honors chemistry. I had a really great teacher last year who taught us a lot of tricks and mnemonics, which definitely came into use on yesterday’s subject test. There were a lot of tricks on the test yesterday, and I’m not sure how someone without a strong honors chemistry foundation/AP Chem knowledge would have gotten those questions right.
For the people talking about electrolysis. The cathode always is where reduction occurs and the anode is where oxidation occurs. Because electrolysis is reversing the motion of electrons, the cathode and anode switch. Hope that helps. 
Can someone help on 37? What’s wrong with C?
How does k the rate constant get affected by temperature exactly? Like temperature increase results in what happening to k? Or does it depend on exo/endo?
The surface area of the reactants also affects the rate constant!!
@dsi441 The answer is still temperature, sorry for the capitalization, thought it was assumed from the question.
@ambitious98 I don’t think it does… Surface area affects rate, but not rate constant k unless I’m mistaken
temperature/pressure/surface area affect the rate since more collisions occur
if rate increases, concentration would not increase so k would have to change
rate=k*[x][y]
@stemscholar it doesnt affect k directly, it affects rate which in turn affects k since it doesnt change the concentration
@Frigidcold But it’s not just temperature that affects the rate constant. Anything that affects the rate of reaction will change the rate constant.
In an electrolytic cell, we have to account for the cell-potential of water. Correct?
i never have @Centry
@Centry Yes, but generally it doesn’t matter.
it’s the Arrhenius equation @stemscholar
source: http://www.chemguide.co.uk/physical/basicrates/arrhenius.html
Increasing surface area definitely does NOT change the rate constant…you can’t change k unless you change the temperature.
The rate a crushed pill dissolves increases when it’s crushed because there’s more exposure to the solvent. This isn’t synonymous with the solubility of the pill; it just dissolves faster.
@chemistryguy123 If you’re talking about 2014 mc, you don’t know what the equilibrium constant is, so not a very reasonable answer.
@Zeppelin7 I’ve got a bad feeling that it will be buffers and titrations
@glasshours wrong. Increasing SA increases the amount of collisions, increasing the rate. Since increasing SA does not affect concentration, k would have to change if rate changes
I just found out we can’t use a calculator on the MC like a week ago, my mental math skills are pretty bad and I’m worried about it for test! Does anyone know how much math is on here and how easy/hard it is?
its more concepts.