CHEMISTRY COMMUNITY

Jacob_Eberson_2D

A greater temperature means more collisions and an increased rate of reaction.

Jacob_Eberson_2D

if the surroundings are doing work on the system, it is positive

Jacob_Eberson_2D

it won't be in the reaction, as it is separate and lowers activation energy

Jacob_Eberson_2D

yes, it lowers activation energy for the reaction regardless of direction

Jacob_Eberson_2D

catalysts lower activation energy of the reaction

Jacob_Eberson_2D

kJ/mol or J/mol

Jacob_Eberson_2D

catalysts are not consumed

Jacob_Eberson_2D

it would be linear with a positive slope (k)

Jacob_Eberson_2D

the reactants in the rate law are those in the slow step

Jacob_Eberson_2D

yes, you can match/cancel out units in the rate constant with units in the rate law

Jacob_Eberson_2D

the equation is 1 / (k*[A]initial)

Jacob_Eberson_2D

termolecular would be for third order reactions

Jacob_Eberson_2D

the final is on material from the entire quarter

Jacob_Eberson_2D

i don't think it matters as long as it's consistent throughout all the calculations and everything. I usually use seconds.

Jacob_Eberson_2D

we probably just have to recognize what the order of the reaction is based on a graph (how they look/axis variables)

Jacob_Eberson_2D

the first equation is for zero order reactions, and the second is for first order

Jacob_Eberson_2D

for zero order, the [A] vs time graph is linear with a slope of -k. first order reactions have linear graphs for ln[A] vs time. second order reactions have a linear graph for 1/[A] vs time.

Jacob_Eberson_2D

yes they are always positive as it comes from the concentration value which is always positive

Jacob_Eberson_2D

it is -k in both the zero and first order reactions, and for second order it is positive k

Jacob_Eberson_2D

when the y-axis is ln[A] it's linear for the 1st order, and when it's [A] vs time the graph is exponential

Jacob_Eberson_2D

it's usually in seconds but it depends on the problem

Jacob_Eberson_2D

an ln[A] vs time graph with a first order reaction has a -k slope.

Jacob_Eberson_2D

ln(2)=0.693

Jacob_Eberson_2D

if you graph ln([A]) vs time, the slope is -k

Jacob_Eberson_2D

a spontaneous reaction is one that is thermodynamically favorable, regardless of the speed/rate of the reaction

Jacob_Eberson_2D

Joelle Tran 1K wrote:Watching this video helped me:

https://www.youtube.com/watch?v=1g-vDSWYins

Thank you! this was really helpful

Jacob_Eberson_2D

the rate law for zero order is A=-kt+A0, which has the same format as the linear equation y=mx+b (with -k as the slope)

Jacob_Eberson_2D

kinetics is about the rate of the reaction, while thermodynamics is more about a reaction's spontaneity

Jacob_Eberson_2D

catalysts reduce the activation energy no matter the direction of the reaction which increases the rate

Jacob_Eberson_2D

a negative rate would be saying that you are forming more reactants not using them

Jacob_Eberson_2D

kinetics is talking about the rate of the reaction, versus thermodynamics which is talking about the spontaneity

Jacob_Eberson_2D

good, I took 14 ae and not taking be was a good call

Jacob_Eberson_2D

for first order reactions the half life is equal to 0.693/k

Jacob_Eberson_2D

Catalysts make the reaction faster by decreasing the activation energy required for the reaction to happen.

Jacob_Eberson_2D

Marleena wrote:I thought all of the values given are state functions. Did anyone else get this?

. yes, I was a little hesitant about temperature but I think that they are all state functions.

Jacob_Eberson_2D

In highschool I had to do a project on this! I made pancakes and explained it like a chemical process, as well as talking about what chemical processes were happening. It was actually super cool and helped me to understand the chemistry topics more than anything else.

Jacob_Eberson_2D

Those multicolor sour worms are really good and sour patch watermelon!

Jacob_Eberson_2D

The outline problems and the ones on achieve were super helpful for me.

Jacob_Eberson_2D

The most important thing that I have been doing is getting my work done in different places (library/lounge/outside). Changing up where I work has helped it feel less monotonous for sure!

Jacob_Eberson_2D

The Getty is super close and they have a ton of art! The view of the city is also amazing and they have a pretty cool garden. It was only like a 5 minute uber so definitely check it out!

Jacob_Eberson_2D

My favorites are the dried mango slices and the trail mix

Jacob_Eberson_2D

I've tried both, and I don't think there's a huge difference in how well I take in the info in person versus online. Usually I decide based on how busy I am on a certain day / if I had time to eat lunch already.

Jacob_Eberson_2D

I like doing the achieve questions and then finding similar questions online and trying to complete those too, and I have found that it has helped me to be a lot quicker at solving the problems.

Jacob_Eberson_2D

Srikar_Chintala_1E wrote:I love listening to The Weeknd or Giveon.

. Yeah what he said !!!

Jacob_Eberson_2D

I started taking my online classes (recorded and zoom) in random places on campus so that I wasn't just in my room at my desk or in the lounge. It's definitely helped it feel less monotonous and the action of walking to "class" or wherever definitely helped it feel like less of a chore.

Jacob_Eberson_2D

Diddy Riese ( ice cream/cookies )is always good if you can catch it when there's no line. Also, there is a little coffee shop called Upside Down that has good coffee and is a good place to do work.

Jacob_Eberson_2D

If you play sports check out the intermural fields there's usually people there midday playing soccer/football.

Jacob_Eberson_2D

Yoga! And walking/running through the neighborhoods surrounding campus is cool because all the houses are huge!

Jacob_Eberson_2D

Thank you so much, this was awesome! This was so inspiring.

Jacob_Eberson_2D

I really like UpsideDown in Westwood its pretty close (sorta by in-n-out) and its donation based so you pay however much you want to. There's wifi and the coffee is pretty good too!

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