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Author: Subject: Theoretical Yield Ni + 2HCl yields NiCl2 + H2
blondeface03
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[*] posted on 7-3-2017 at 07:30
Theoretical Yield Ni + 2HCl yields NiCl2 + H2


Hey All,

I have the balanced equation of Ni (s) + 2 HCl (aq) -> NiCl2 (aq) + H2 (g)

A.) If 12.0 moles of HCl were reacted, how many moles of Ni would be needed such that there was no excess?

B.) What is the theoretical yield (in grams) of NiCl2 from reacting 12.0 mol HCl?

C.) If 12.0 mol of HCl was reacted and the percent yield of the reaction was 78.5%, what was the actual yield (grams) of NiCl2?

I am completely lost when it comes to theoretical yield questions.. Any help is gladly needed!

Thank-you so much!
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ficolas
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[*] posted on 7-3-2017 at 07:40


Quote:

Beginnings Schoolwork help and beginner questions (not a textbook substitute).

I dont want to be rude, but this is very very very basic, and your teacher is probably the one who should have answered this question for you.

Still, to try to be less rude, im going to give you some info.

That equation means that you need 1 mol of Ni, per each 2 mols of HCl, to form 1 mol of NiCl2 and 1 mol of H2. From that i'll let you calculate the rest.

To convert from molest to grams, you just multiply by that substance molecular weigh.

And the last question, well a 78.5% of what would be formed if the reaction went to completion, pretty sure you can figure that out!


Im not going to solve it, because by thinking by yourself you train your mind to solve more difficult things.

[Edited on 7-3-2017 by ficolas]
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blondeface03
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[*] posted on 7-3-2017 at 07:46


Hey,

I didn't realize this forum was supposed to be only for scientific geniuses- Forgive Me.

I appreciate what you did explain to me- even with the cyber attitude that came with it :)
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ficolas
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[*] posted on 7-3-2017 at 09:10


I never said it was for scientific geniused, im really inexperienced, however copypasting a question your teacher gives you is far from amateur experimentalism.

Google could have solved that faster. I am not trying to be rude at all, mainly because you are probably really young to know much, and even if you arent, still no reason to be rude.

(Yes, I am making some pre-asumptions from what you asked and the way you did, but they are probably right)


[Edited on 7-3-2017 by ficolas]
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blondeface03
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[*] posted on 7-3-2017 at 09:20


I am reaching out for help beyond just asking my teacher. I didn't realize that was a crime to you.

"They are probably right"- more snarky attitude from you... Really, Queen? Please don't bother answering any future questions I post here.

Your feedback is negative and unneeded.
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DraconicAcid
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[*] posted on 7-3-2017 at 10:01


Quote: Originally posted by blondeface03  
I am reaching out for help beyond just asking my teacher. I didn't realize that was a crime to you.

"They are probably right"- more snarky attitude from you... Really, Queen? Please don't bother answering any future questions I post here.

ficolas isn't the one being rude here.




Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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blondeface03
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[*] posted on 7-3-2017 at 10:18


Hey Geniuses-

Will someone check my answer for me, please? Everyone wants to call me out for being rude, could you at-least tell me if I'm on the right track with answering the proposed questions?

A) Just use the coefficients of the balanced equation to relate moles of one thing to moles of another:
12 mol HCl X (1 mol Ni / 2 mol HCl) = 6 mol Ni

B) Again, use the coefficients from the equation to calculate moles NiCl2 formed. Then use the molar mass of NiCl2 to convert moles to grams:
12 mol HCl X (1 mol NiCl2 / 2 mol HCl) = 6 mol NiCl2
6 mol NiCl2 X (129.6 g/mol) = 778 grams NiCl2 (THIS is the theoretical yield for this reaction)

C) The percent yield is calculated as:
% yield = (actual yield / theoretical yield) X 100.

So, substituting what you know into this gives:

78.5% = (actual yield / 778 g) X 100
0.785 = actual yield / 778
actual yield = 611 grams NiCl2

Thanks!
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DraconicAcid
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[*] posted on 7-3-2017 at 10:20


That looks correct.



Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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blondeface03
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[*] posted on 7-3-2017 at 10:25


Thanks for replying to such a "very basic" question. I appreciate it.
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Jstuyfzand
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[*] posted on 7-3-2017 at 11:23


No need to be a cunt about it, grow up.
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