14.2 Rate Laws 

This man deserves a Noble Prize, I swear. Genius

You are an great communicator. Keep up the good work. You made this really confusing topic from my class and textbook easy to understand.

They didn’t laugh at your jokes enough smh, I would’ve been like “AHHAHAHA” You’re a great professor, I’ve been stuck on these forever but I finally understand it for my test next week. Thank youuuu Back to binge watching, all your vids

I watched these videos 3 years ago for AP chemistry and I'm back again... this time for general chemistry in college. Thank you Chad! Your content is always quality and reliable :)

So happy I found your videos! You're such a good teacher!

The battery and starter analogy was spot on for explaining this. Thank you.

thank you so much for this. I was gonna cry cos im studying for my finals and NONE OF THE VIDEOS made sense until i came across this one. thank you so so so much

Hello Chad, I have some questions I was hoping you can answer. When comparing trials/experiments, you said (around 11:40) that you need to compare the one where only one of the reactants have changed, so that if the reaction rate changes, you know what was responsible for the change. That makes total sense. What doesn't make sense is in your table around 12:00, you compared trial 2 and 3 for NO. Then at 13:56 you compared trials 1 and 2 for Cl2. My questions are: 1) Why can't you compare the first trial and the third for NO and the Cl2? Why specifically 2 and 3 for NO and 1 and 2 for Cl2? 2) In trial 2, the concentration of Cl2 changed to 0.2 while NO stayed the same at 0.1. You can only change one concentration at a time in each trial, and the first row at the top is the numbers for the original before you changed anything. So why did you change the concentration of both NO and Cl2 in the 3rd trial? Both are now 0.2 moles/L. Since you already changed the concentration of Cl2 in trial 2, for trial 3, shouldn't the concentration now be 0.2 for NO and back to 0.1 for Cl2? Thanks in advance.

Far and away the best vid for rate law I've seen

Love your videos! They've been super helpful during chemistry 2 in college.

This helps me and my friends alot. Thank you for your great lecture as you've made it easy for us to understand. definitely will recommend your channel to my coursemates !

Professor how good teacher u r!It is my fortune that I was recommended to watch ur videos,they r incredible and priceless!Thankssssssssss😁😇

Extremely helpful! Thank you!

Your videos are the first I have found online that I truly understand, better than Khan academy and everything. You just make it make sense. Thank you so much :)

Chad, you are a legend! Thank you very much.

Wooow love the examples you give!!!

You explained this SO well

You really make this easy. (: Thanks a lot.

What a smart teacher wowww

What a great way of teaching!!!!! I wish I was in his class

thank you!!! :)

Hey, I really want to know why the concentrations of reacting substances must be multiplied and even raised to some powers. Please enlighten me about this.

wish I found you sooner! google needs to put you front page

This is the all syllabus in entrance too

The way he explains things!! 🙌🏽🙌🏽🙌🏽 HALLELUJAH! I’m actually gonna graduate

should we know anything about 4th order reaction ?

thank you for breaking everything down, i'm retaking chem 2 after 15 years and it's been a struggle

How you calculate this? For a particular reaction, the hydroxide ion is one of the reactants. Doubling the concentration of the hydroxide ion, while holding all other concentrations constant, changes the rate of reaction from 0.002 to 0.008. What is the order with respect to the hydroxide ion?

So sir it means order of reaction depend on the sum of stochiometric coefficient of the product in the reaction

I know it's been years since you posted this video and I never did chemical kinetics so please bare with me. When you calculated the order of reaction from the experimental data, you took the "k" to be the same for the two experiments (and k/k = 1). My question is how did you know that both experiments had the same "k"? I understand that the concentration of one of the reactants is constant between the two experiments, but I don't get how the "k"s remain the same. Apologies if I'm not seeing something obvious here.

Great

You’re awesome

GOAT 🐐🐐

The native people will enjoy your lectures but most of the words are out of our range can you please slow down your speed

Look like criminal