Most Common Chemistry Final Exam Question: Limiting Reactants Review
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- Опубліковано 20 сер 2024
- This Chemistry review covers a common final exam question/ topic. We'll go over how to find the limiting reactant, excess reactant, theoretical yield, percent yield, actual yield and how to find the amount of excess left over.
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I haven't even finished chem 1 but I went from exam 1- 65% 2nd -80% to the 3rd 92% because of your videos ❤ as soon as I can i will be visiting your patreon
I'm going to bust my butt to do well on the final
What I should’ve done now I have a 59 and need to do well on the final so watching this and writing facts down to study till then
My Chemistry 101 final is on Wednesday (it's Monday...) and I only had like three days to prepare for it so binging your youtube channel has been a bigger help than my own professor. I'm finally understanding all these concepts without spending like four hours on one topic!
Thank you SO much for including practice problems you're the reason I might not fail.
You are so welcome!!
Exactly the same situation here, but today is the final, in 30min. Wooo i love chem…
Still managed to get a C in my chem 1 final. I would've fluked the course if not for your videos! Will make a comeback on chem 2!!
Why take chem 2? Is it part of your major I thought you only need one science lab
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@@btw3344 do biology majors need to take the ACS final for chem. Im in biology but still take chem courses and apparently we do. Can we opt out or something?
I have a chemistry final exam tomorrow for Gen Chem 1. I didn't know stoichiometry or limiting reactant, however, from watching your videos, I not understand both! a MASSIVE thank you! I feel way more confident going into my exam and I am definitely going to keep watching your videos!
How did it go?
Amazing how your videos taught me all the chemistry I know and am loving the smile that stays on my face when I write chemistry exams/tests. THANK YOU!!!!!!!!!!
thank you mrs melissa, i hope i can boost my chem from 70% to 100% on the final exam and get over with it
I have a final today and this cleared SO MUCH for me omggg 😭 thank you Melissa! 💗
I have my gen chem 1 final tomorrow morning and your videos have been super helpful thank you!!!
Update: I just took my final and this helped me so much!!
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My professor hasn't taught a class since the pandemic, so you're saving me! I hope to at least get a C. She yeeted stuff from the hw so she wouldn't have to grade it but it'll be on the final.
Thank you for this Melissa!😍 I now slightly understand stoichiometry👏
my finals are less than a week and ur videos are saving me, thanks a lot
There is an easier way of working out the limiting reactant. Just find the moles of both reactants and use the molar ratio to compare both reactants. The reactant with fewer moles is gonna be your limiting reactant.
Yep that works too, I just like getting to the grams because most questions ask for the theoretical yield and students forget how to get there. So I like showing you one way that answers two questions.
Melissa Maribel Ahh I understand. However wouldn’t finding the limiting reactant by moles be more effective as you exclude the other reactant for the second part of the question.
Both are effective, if you prefer stopping at moles then do that. The important part is that you understand how to get there 👍
I’ve watched all most every video on youtube for this and still not completely understanding it THANK YOU my test is today hopefully I pass !!!!
hope you're test went well. Writing mine tomorrow. All the best for the future
Theoretical yield is the quantity of a product obtained from the complete conversion of the limiting reactant in a chemical reaction. It is the amount of product resulting from a perfect (theoretical) chemical reaction, and thus not the same as the amount you'll actually get from a reaction in the lab. Theoretical yield is commonly expressed in terms of grams or moles.
In contrast to theoretical yield, the actual yield is the amount of product actually produced by a reaction. Actual yield is usually a smaller quantity because few chemical reactions proceed with 100% efficiency because of loss recovering the product and because other reactions may be occurring that reduce the product. Sometimes an actual yield is more than a theoretical yield, possibly because of a secondary reaction that yields additional product or because the recovered product contains impurities.
This is AMAZING! Thank you so much Melissa😊
This really took a long time for me to understand the limiting reactants and finding each yield and excess reactants to percentages lol but thank you so much this really helped me greatly.
you're a teaching genius
Aw thanks!
Thank you soooo much
love this channel
Knowing what percent yield actually is solidifed my faith in chemistry
You’re amazing ! God Bless you!!!
Thanks Michelle 😊💕
I LOVE YOU THANK YOU FOR SAVING ME IN CHEM!!!
So helpful thank you for all that you do!
When I did this on my own for some reason my brain said find the molar mass of 2Fe because on the product side the coefficient was 2.. its like throwing me off a bit and i don't understand why
You are amazing!!!
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my final is tomorrow lol goodluck to all!
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Thanks mam
I have exams in August 😥😥😥i have never been so good in che 110 I really need ur help Madam and this videos is so helping
How did you get 163g Fe2O3 for the used? I keep getting 653g
So if you start with finding Fe instead of CO2 the first time you would have to continue finding Fe in the second one?
So...is percentage yield accuracy, how close you were to achieving the perfect scenario or compound?
Edit: Nevermind, asked too soon.
What if it says mixed with ? the wording is tripping me up because I don't know if I have to add the two given numbers in grams and then set the problem up or am I still solving for one?
In the reaction given below, 35.2 g of bromine (Br2) is MIXED with 23.1 g of phosphorus (P) to produce phosphorus tribromide (PBr3).
What are the limiting reactant and the theoretical yield, in grams, of phosphorus tribromide?
OH my god i really thought i was going to wing it because i could not save my life doing these problems. I understand it a little bit more and i think I'm buying the notes chem 2 if i pass
I am so much inspired by you mam
Thank you!
Someone please help would appreciate
If magnessium burns in the air to form magnessium oxide accordingly to the following balanced equation
2 Mg +O2->2Mg
If the percentage yield of this reaction is only 80% calculate the mass of magnessium that needs to be burned to produce 30g of magnessium oxide
Hey there, did you still need help with this question?
@@melissamaribel yes please i would appreciate ♡
@@melissamaribel please
You are a given the percent yield of 80% and the actual yield of 30 g MgO
1)Start with finding the theoretical yield by plugging the percent yield and actual yield into the percent yield formula shown at 23:29.
2) After you found your theoretical yield of MgO you will work your way back to grams of Mg.
So you'll go from grams of MgO to mol MgO to mol Mg to grams of Mg and you are done.
Make sense?
@@melissamaribel thanks i truly understand 😄 thanks melissa you are a star 🙆🙌
how do you know what product to choose from if u have 2 of em
I am not sure why, but on the conversion os CO to Fe, why is the grams of Fe only 55.85g? In the reactants it is 2Fe, so why was the molar mass not done 2Fe, only 1Fe? Is it because that is just converting it back to grams? So the Fe is only one because that is the conversion done?
The rest totally helped me. Before, I didn't even know where to start. This clarifies limiting reactant problems so much.
For molar mass it's only 1 mole of that element or that compound, so for Fe we are not looking at the mole to mole ratio or the balanced equation instead we only want 1 mole of Fe = molar mass of just 1 Fe.
@@melissamaribel Thanks!
Can you please explain how you got 116.8g
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Thanks!
Hi sorry this is unrelated but in regards to chemistry if we wanted to investigate the affect of concentration of rate reaction how will we do so with: HCL and Antacid in this case we have to do a prac where we need to put our results in a graph where we vary the concentrations of the HCL from 0.1 m 0.5 m 1m but maintain the antacid so far I have plotted just the times of when the reaction is done but I don’t know how to record the rest in order to make a graph?
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