/wsr/ - Worksafe Requests » Thread #1008092

[12 / 2 / ?]

60KiB, 640x360, gettyimages-484013593-640x640.jpg

Anonymous Wed 14 Apr 2021 18:26:35 No.1008092 View View Reply Original Report

Quoted By: >>1008116 >>1008131 >>1008138

Only you can help me 4chan

I need to finish this in 1:12. Please, I don't know how to answer that. Can u guys help me? > <

10 moles of SO2 and 10 moles of oxygen are passed over a V2O5 catalyst and result 8 moles of sulfuric anhydride.

What are the moles of
gas that remained unreacted, indicating limiting and excess reagent?

2. Reaction yield?

save me /wsr/ please :(

Anonymous

Anonymous Wed 14 Apr 2021 19:03:49 No.1008116 Report

Quoted By:

>>1008092
Dude i would help u but i don't know anything about chemistry the only thing i can say to you that there are boards about maths and that shit u can ask them

Anonymous

View Same Google ImgOps iqdb SauceNAO 1599337149427.jpg, 275KiB, 957x931

Anonymous Wed 14 Apr 2021 19:29:41 No.1008131 Report

Quoted By: >>1008162

>>1008092
>I need to finish this in 1:12.

not OP

not OP Wed 14 Apr 2021 19:41:15 No.1008138 Report

Quoted By: >>1008155 >>1008162 >>1008181

>>1008092
remaining moles
5 moles of O2
limiting reagent SO2
excess reagent O2
Reaction yield 80%

not OP

not OP Wed 14 Apr 2021 20:00:44 No.1008155 Report

Quoted By: >>1008181

>>1008138
i mean 6 mol O2 left over
2 SO2 + O2 -> 2 SO3

Anonymous

Anonymous Wed 14 Apr 2021 20:08:12 No.1008162 Report

Quoted By: >>1008181

>>1008138
>>1008131
I still have time lol
pls help me

bruhmomentunodostres

bruhmomentunodostres Wed 14 Apr 2021 20:30:25 No.1008181 Report

Quoted By: >>1008191 >>1008232

>>1008138
This was me
>>1008162
what more do you want?
>>1008155
plz don't use my name to correct the answer Op will think its the same guy
it is 5 moles of O2 left 10 moles of SO2 were consumed(had this not happened reaction would not have stopped) out of which only 8 moles was our yield , so 5 moles of O2 were consumed
5 moles left

Anonymous

Anonymous Wed 14 Apr 2021 20:40:40 No.1008191 Report

Quoted By: >>1008198

>>1008181
are we reading the same question bro?
from the balanced equation
2 SO2 + O2 -> 2 SO3
1 O2 molecule gets consumed for every 2 SO2 molecules consumed
8 moles SO2 were consumed to make 8 moles SO3, therefore 4 moles of O2 were consumed, 6 moles O2 are unreacted
i don't understand the reasoning here

Anonymous

Anonymous Wed 14 Apr 2021 20:58:43 No.1008198 Report

Quoted By: >>1008229 >>1008232 >>1008248

>>1008191
>are we reading the same question bro?
man I hate to do this to you

>8 moles SO2 were consumed to make 8 moles SO3
They never said 8 moles of SO2 were consumed to make 8 moles of SO3 , they said result was 8 moles of SO3 actual yield and theoretical yield are different , for the reaction to stop there must be a limiting reagent , it has to be SO2 theoretically because you have equal moles of SO2 and O2 but only half of O2 is consumed per 1 of SO2
Since SO2 is the limiting reagent all 10 moles have to have been consumed and 10 moles of SO3 were produced but we lost 2 moles of SO3 in the process

Anonymous

Anonymous Wed 14 Apr 2021 21:53:37 No.1008229 Report

Quoted By: >>1008232 >>1008248

>>1008198
>they said result was 8 moles of SO3 actual yield and theoretical yield are different , for the reaction to stop there must be a limiting reagent , it has to be SO2 theoretically because you have equal moles of SO2 and O2 but only half of O2 is consumed per 1 of SO2
yes, that's correct
>Since SO2 is the limiting reagent all 10 moles have to have been consumed and 10 moles of SO3 were produced
that would have been the theoretical yield yes, the idealized case when the reaction goes to completion, not necessarily the case in this problem or in real life

>They never said 8 moles of SO2 were consumed to make 8 moles of SO3
>but we lost 2 moles of SO3 in the process
this is the main issue i have bro, you didn't need to overcomplicate things with this. don't assume the chemist actually made 10 mol SO3, but 2 slipped through the cracks of the reactor...
if you really wanted to be realistic with the problem, whatever's left inside the reactor ultimately depends on the reaction conditions like temperature, pressure, reaction time, etc., and we don't have the specifics

just keep it simple, it's only a homework question after all
we know that there's 8 moles of SO3 by the end, so 8 moles of SO2 must have been reacted and 2 moles of SO2 are left inside
if 8 moles of SO2 were consumed, then 4 mol O2 are used up, and 6 mol O2 remain unreacted

Anonymous

Anonymous Wed 14 Apr 2021 21:59:22 No.1008232 Report

Quoted By:

>>1008229
>>1008198
>>1008181
thank you brothers. I love this community.

Anonymous

Anonymous Wed 14 Apr 2021 22:39:51 No.1008248 Report

Quoted By:

>>1008198
>for the reaction to stop there must be a limiting reagent
You forgot to counter this argument btw
>>1008229
2nd part wants reaction yield the formula for which is
(actual yield)/(theoretical yield)*100

here's a video of some1 else solving for reference
https://youtu.be/WncgeAMDNwc?t=142
this guy is solving a similar problem watch till he solves part b 5:15 .

Capcode	All Only User Posts Only Verified Posts Only Moderator Posts Only Manager Posts Only Admin Posts Only Developer Posts Only Founder Posts
Show Posts	All Only With Images Only Without Images Only Spoiler Images Only Non-Spoiler Images
Deleted Posts	All Only Deleted Posts Only Non-Deleted Posts
Ghost Posts	All Only Ghost Posts Only Non-Ghost Posts
Post Type	All Only Sticky Threads Only Opening Posts Only Reply Posts
Results	All Grouped By Threads
Order	Latest Posts First Oldest Posts First

On these archives

Your latest searches