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Reacties en evenwichten Samenvatting 2024 Applied Science $9.90
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Reacties en evenwichten Samenvatting 2024 Applied Science
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  • Course
  • Reacties en evenwichten
  • Institution
  • Fontys Hogeschool (Fontys)
  • Book
  • Chemistry, Global Edition

In deze samenvatting komen alle onderwerpen aan bod voor het tentamen van het vak reacties en evenwichten op de fontys opleiding applied science.

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Document information

  • No
  • Hoofdstuk 14
  • October 29, 2024
  • 17
  • 2024/2025
  • Summary

Subjects

  • reacties en evenwichten
  • reaction rate
  • reaction law
  • 2024
  • reaction order
  • ideale gaswet
  • osmotische druk
  • chemische energie
  • enthalpie
  • hesss wet
  • evenwichtsconstante
  • principe van le chatelier
  • oplosbaarheid
  • e

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Reacties en evenwichten 2024
14.1 Reaction rates
De reaction rate is de toename van de concentratie van een product per tijdseenheid of de afname
van de concentratie van een reactant per tijdseenheid.

𝑣𝑒𝑟𝑎𝑛𝑑𝑒𝑟𝑖𝑛𝑔 𝑖𝑛 𝑐𝑜𝑛𝑐𝑒𝑛𝑡𝑟𝑎𝑡𝑖𝑒 ∆[𝐴]
𝑅𝑎𝑡𝑒 = =
𝑣𝑒𝑟𝑎𝑛𝑑𝑒𝑟𝑖𝑛𝑔 𝑡𝑖𝑗𝑑 ∆𝑡

Voorbeeld:
2 N2O5 (g) → 4 NO2 (g) + O2 (g)




∆[𝑂2 ] 0.0049 𝑀 − 0.0040 𝑀
𝑅𝑎𝑡𝑒 𝑣𝑎𝑛 𝑂2 = = = 9.0 × 10−6 𝑀/𝑠
∆𝑡 400 𝑠 − 300 𝑠

∆[𝑁𝑂2 ] 0.0197 𝑀 − 0.0160 𝑀
𝑅𝑎𝑡𝑒 𝑣𝑎𝑛 𝑁𝑂2 = = = 3.7 × 10−5 𝑀/𝑠
∆𝑡 400 𝑠 − 300 𝑠

Wanneer O2 en NO2 worden gevormd, verdwijnt N2O5.
De reaction rate is gedefinieerd als een positieve waarde en daarom moet er altijd een min (-) teken
worden geïntroduceerd wanneer de rate wordt berekend van een reactant.

−∆[𝑁2 𝑂5 ] −(0.0101 𝑀 − 0.0120 𝑀)
𝑅𝑎𝑡𝑒 𝑣𝑎𝑛 𝑁2 𝑂5 = = = 1.9 × 10−5 𝑀/𝑠
∆𝑡 400 𝑠 − 300 𝑠




1

,Voor de algemene reactie:
aA + bB → cC + dD

Geldt de volgende algemene reaction rate:
1 ∆[𝐴] 1 ∆[𝐵] 1 ∆[𝐶] 1 ∆[𝐷]
𝑅𝑎𝑡𝑒 = − =− = =
𝑎 ∆𝑡 𝑏 ∆𝑡 𝑐 ∆𝑡 𝑑 ∆𝑡

Voorbeeld:
2 N2O5 (g) → 4 NO2 (g) + O2 (g)

1 ∆[𝑁2 𝑂5 ] 1 ∆[𝑁𝑂2 ] ∆[𝑂2 ]
𝑅𝑎𝑡𝑒 = − = =
2 ∆𝑡 4 ∆𝑡 ∆𝑡

14.2 Rate laws and reaction order
Algemene reactie:
aA + bB → producten

Rate law:
Rate = k[A]m[B]n

- Wanneer m = -1
→ [A]-1 of 1/[A]
→ wanneer [A] verdubbeld, dan neemt de rate af met een factor 2.
- Wanneer m = 0
→ [A]0 = 1
- Wanneer m = 1
→ [A]1 of [A]
→ wanneer [A] verdubbeld, dan verdubbeld de rate ook.
- Wanneer m = 2
→ [A]2
→ wanneer [A] verdubbeld, dan neemt de rate toe met een factor 4.




2

, 14.3 Method of initial rates: experimental determination of a rate law
Een methode om de waarden van de exponenten in een rate law te bepalen (the method of initial
rates).

Voorbeeld:
2 NO(g) + O2(g) → 2 NO2(g)




Experiment 1 en 2:
[NO] verdubbeld; [O2] is constant; reaction rate neemt toe met een factor 4 (0,096/0,024 = 4). Dit
betekent dat m = 2, oftewel [NO]2

Experiment 1 en 3:
[NO] is constant; [O2] verdubbeld; reaction rate neemt toe met een factor 2 (0,048/0,024 = 2). Dit
betekent n = 1, oftewel [O2]

Rate = k[NO]2[O2], hieruit kan k berekend worden:

𝑟𝑎𝑡𝑒 0.024 𝑀/𝑠
𝑘= = = 7.1𝑥103 𝑀−1 𝑠 −1
[𝑁𝑂] [𝑂2 ] (0.015 𝑀)2 (0.015 𝑀)
2




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