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Samenvatting Reacties en Evenwichten $3.88   Add to cart

Summary

Samenvatting Reacties en Evenwichten

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Een samenvatting van de totaal te leren stof voor reacties en evenwichten

Preview 1 out of 11  pages

  • No
  • Hoofdstuk 8, 12, 13 en 16
  • November 5, 2015
  • 11
  • 2015/2016
  • Summary

2  reviews

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By: Stijnnnn • 3 year ago

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By: AnnaRitzen • 6 year ago

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Reacties
en
evenwichten


Hoofdstuk
12



!!"#!$#%&'%($
Reactiesnelheid =
!!"#$


Voorbeeld:
2 N2O2 ↔ 4 NO2 + O2
[!!] ![!"#$]
r = !" → O2 = -0,5
!!
(0,5 → 1:2)
!"#$%&#  !""#  !"  !"#$
• Getal bepalen: !"#$%&#  !"  !"  !"#$
- (min) bij reactant → verdwijnt

Reactiesnelheid is afhankelijk van:
• Begin concentratie
• Temperatuur
• Aanwezigheid van katalysator

r = k [A]m[B]n
→ totale reactieorde= m+n
• 0e orde: snelheid afhankelijk van k

Voorbeeld reactieorde bepalen:
Gegeven is: Concentratie N O Reactiesnelheid r
2 5
0,020 M 3,4 x 10-5 M/s
0,050 M 8,5 x 10-5 M/s
r = 3,4 x 10-5 = k[0,020]m
r = 8,5 x 10-5 = k[0,050]m
→ beide delingen resulteren in 2,5, dit betekent een 1e orde reactie (m=1)

− Reactiemechanisme: volgorde van reactiestappen van reactant naar product
− Elementaire reactie: kan niet meer opgesplitst worden in meerdere producten

Nulde orde reactie:
• Snelheid onafhankelijk van de concentratie
• r=k
• [A]t = -kt + [A]o
• plot A vs tijd (k = -helling)

Eerste orde reactie:
• Snelheid afhankelijk van één reactant
• r = k[A]
• ln[A]t = -kt + ln[A]o
• plot ln(A) vs tijd (k = -helling)
!,!"#
• t1/2 = ! → constant

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