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anonymous

  • one year ago

Question 34

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  1. anonymous
    • one year ago
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  2. anonymous
    • one year ago
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    @aaronq

  3. Disco619
    • one year ago
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    Is there an Answer key from which the answer can be confirmed?

  4. anonymous
    • one year ago
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    in an organic synthesis 60% yield of product is achieved. which of these conversions are consistent with this information 1) 74 g of butan-2-ol -> 44.64 g of butanone 2)74 g of butan-1-ol -> 54.56 g of butanoic acid 3) 74 g of 2-methylpropane-1-ol -> 54.56 g of 2-methylpropanoic acid

  5. anonymous
    • one year ago
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    Another question ^

  6. Disco619
    • one year ago
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    According to me, the answer is 2. After 2 minutes, the sulfuric acid has produced more gas than ethanoic acid.

  7. anonymous
    • one year ago
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    Yes for 34 all are correct

  8. Disco619
    • one year ago
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    Ok so we can choose more than 1 option?

  9. Disco619
    • one year ago
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    The answer is 1. 74 g of butan-2-ol -> 44.64 g of butanone

  10. anonymous
    • one year ago
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    Yeah the options are A. 1, 2 and 3 B. 1 and 2 C. 2 and 3 D. 1 only

  11. Disco619
    • one year ago
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    Oh okay, then it's A.

  12. anonymous
    • one year ago
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    Same goes for the second question A all three are correct

  13. Disco619
    • one year ago
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    Sulfuric Acid is a stronger acid than Ethanoic Acid which is a weak acid. A Strong Acid fully dissociates Hydrogen ions in a solution, a weak Acid partially dissociates (gives out Hydrogen ions). More dissociation of Hydrogen ions would mean more amount of gas (hydrogen gas) released in the reaction, and the faster it would be released as the concentration of Hydrogen ions is greater.

  14. Disco619
    • one year ago
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    I wouldn't know about the second question cause that's the first time i'm facing that kind of a situation in Chemistry. Hopefully you understood the first Question's answer!

  15. Disco619
    • one year ago
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    Sulfuric Acid would also be at a higher temperature because, both reactions being exothermic (release heat, i.e heat 'exit'), the Stronger Acid would be more hotter as the energy/heat released in bond formation would be greater as Greater number of bonds are being made, as it's concentration is greater.

  16. anonymous
    • one year ago
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    Oh alright

  17. anonymous
    • one year ago
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    But Sulphuric acid's concentration is same as ethanoic acid.

  18. Disco619
    • one year ago
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    Yes, the MOLECULES concentration is same. But the amount of Hydrogen ions Sulfuric Acid 'donates' to the solution is Greater than Ethanoic Acid. Sulfuric Acid donates almost ALL of it's Hydrogen ions, whereas Ethanoic acid donates partially.

  19. anonymous
    • one year ago
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    Ohhhh i got it now

  20. anonymous
    • one year ago
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    So how about second question?

  21. Disco619
    • one year ago
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    For example. The Circles represent the 'MOLECULES' of the acid, and the Circles with 'X' in them are the ones that 'donate' hydrogen ions. |dw:1433717182050:dw| Hope you got it now!

  22. anonymous
    • one year ago
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    Ahaha Nice nice i got it now thanks so much

  23. Disco619
    • one year ago
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    I don't really know about the Second question, I can't say because I just used this: \[\frac{ 60 }{ 100 } \times 74 = 44. 4\] The good ol' math way, but if all are correct then I wouldn't know, this might have a Chemistry side to it.

  24. Disco619
    • one year ago
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    Maybe it's that it's not EXACTLY 60% yield, as NOTHING can be perfect in Science except Theoretically speaking. The Theoretical Yield must be 44.4g, but Experimental yield can differ by a little.

  25. anonymous
    • one year ago
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    I used the same method i got an A in olevels maths :v but alevel maths dissapointed me gave the exams recently not went good sigh.

  26. Disco619
    • one year ago
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    Hahaha Nice Nice! I JUST got done with my O'Levels. Gave the CIEs a week or two ago. I was very very very bad at Chemistry, I hated it, but I got to know this teacher and man (maybe you're a girl ahah), he made me fall in love with Chemistry in so little time. I'm still trying to perfect it.

  27. Disco619
    • one year ago
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    I've failed Maths since 6th grade lol, i'm really bad at it, you have no idea. But the CIEs went pretty good it's hard for even me to believe >.>

  28. anonymous
    • one year ago
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    Dua kero meray bhi achay ho jaen.

  29. anonymous
    • one year ago
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    I just freaked you out a little right??

  30. Disco619
    • one year ago
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    HAHAHAH OMFG XD iA iA Achay ho jayen ge, pellet DAMN! xD

  31. Disco619
    • one year ago
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    sh!t* :@

  32. anonymous
    • one year ago
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    Yeah Good morning.

  33. Disco619
    • one year ago
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    It's.. :| 4 AM, but yeh Good Morning! Goodluck though! If you need any more help (from an O'Level student lol) feel free to ask, i'll be on my way to help someone else!

  34. anonymous
    • one year ago
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    Azaan ho gae hae iss liey mein ne kaha

  35. Disco619
    • one year ago
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    Umm btw if you're in Lahore, try studying from Sir Mohammad Ali. That's the BEST Chemistry teacher you'll ever meet. EVER.

  36. Disco619
    • one year ago
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    Specially for A'Level students.

  37. anonymous
    • one year ago
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    No not in Lahore.

  38. Disco619
    • one year ago
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    Ok so I just realized the answer to Question 34 is 1 and 2.

  39. anonymous
    • one year ago
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    and 3. all three are correct

  40. Disco619
    • one year ago
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    No, not 3. I also thought 3 but I read the Question again. Only 1 and 2. If your Answer Key says all 3 are correct, i'd bet 9.9/10 that it's wrong.

  41. anonymous
    • one year ago
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    today's my exam i hope this doesn't come up :o. why cannot C be though?

  42. Disco619
    • one year ago
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    My Cousin's exam is today too, He's doing AS. I confirmed it from him. Lemme see if I can explain

  43. Disco619
    • one year ago
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    OK I forgot what that rule was named (after the scientist) which told us how to make the reactions go in forward direction (pressure, temperature, moles, concentration), if you remember, you can remind me.

  44. Disco619
    • one year ago
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    Ok I remember, it was Le Chatelier's principle.

  45. anonymous
    • one year ago
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    whats the problem in it? carboxylic acids are weak acids....

  46. anonymous
    • one year ago
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    that was easy it just slipped out of my mind

  47. anonymous
    • one year ago
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    so obviously h2so4 would give less yield

  48. anonymous
    • one year ago
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    Ann-Hybrid why its A in the markscheme then

  49. Disco619
    • one year ago
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    Anyways, the thing is. When the partially dissociated hydrogen ions in weak acid get used up and are released as Hydrogen gas, their concentration decreases in the solution, which causes the acid to release MORE Hydrogen ions. This keeps on happening till all the hydrogen ions are released from the acid and at the end, the gas would be the same amount as of Sulfuric acid, as their volume and concentration is same.

  50. anonymous
    • one year ago
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    Ann-Hybrid it's something you won't understand.

  51. anonymous
    • one year ago
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    rostella

  52. Disco619
    • one year ago
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    Get it?

  53. anonymous
    • one year ago
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    is common sense....that h2so4 would give more yeild at any point

  54. anonymous
    • one year ago
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    but ofcourse its Common sense

  55. anonymous
    • one year ago
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    Ann-Hybrid stop it now i'm trying to focus here

  56. anonymous
    • one year ago
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    kay...u focus..

  57. Disco619
    • one year ago
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    The difference is, the Sulfuric Acid reaction would be faster and more 'intense' (exothermic) as the frequency of fruitful collisions is greater due to it's concentration of Hydrogen Ions. At one time, GREATER Number of ions are released, whereas in the Organic Acid, it's weak and at one time, less number are being released and when they escape as Hydrogen gas, the decrease in concentration causes them to release more Hydrogen ions.

  58. anonymous
    • one year ago
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    I thought the same @Disco619 but just got confused when i saw the markscheme it sure is misleading

  59. Disco619
    • one year ago
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    You just have to trust yourself, I also had trouble cause Marking scheme does lower your confidence sometimes. Goodluck!

  60. anonymous
    • one year ago
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    no wait you said earlier that weak acid dissociates partially it won't give much OH ions so 3 can be correct in this way

  61. Disco619
    • one year ago
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    Not 'OH', 'H' ions.

  62. anonymous
    • one year ago
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    i get it i get it it will be used up by the end of reaction.

  63. Disco619
    • one year ago
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    Yes they DO Dissociate partially! But when the - whatever dissociated ions - in the solution escape (as H2 in this case), their concentration decreases, which causes the weak acid to dissociate MORE of it's ions. Then they get used up, more are released, they're used up and so on... Till the acid runs out of Hydrogen ions to be released (as the metal was in excess)

  64. anonymous
    • one year ago
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    oh yeah H ions

  65. anonymous
    • one year ago
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    ohh so markscheme is a lie. oh well.

  66. Disco619
    • one year ago
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    Yup!

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