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Samenvatting Hoofdstuk 18 Accu's en brandstofcellen Scheikunde Chemie Overal 6vwo R68,95   Add to cart

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Samenvatting Hoofdstuk 18 Accu's en brandstofcellen Scheikunde Chemie Overal 6vwo

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Hoofdstuk over accu's en brandstofcellen, Elektrochemische cel en brandstofcel, zowel de werking als een voorbeeld. Fossiele brandstoffen en energietransitie. Paragraaf 1 tot en met 4

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  • February 7, 2023
  • 4
  • 2021/2022
  • Summary
  • Secondary school
  • 6
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Samenvatting scheikunde hoofdstuk 18

Elektrochemische cel
Daniell cel

Eén reactievat wordt ook wel een
halfcel genoemd.

Kant waar elektroden vrij komen =
negatieve elektrode/ minpool

Kant waar elektroden worden
opgenomen = positieve elektrode

Zn = Red: Zn  Zn2+ + 2e-
Cu = ox: Cu2+ + 2e-  Cu

Of Red: Cu  Cu2+ + 2e-
Ox: Zn2+ + 2e-  Zn
Eén van de twee reageert maar! Sterkste RED en sterkte OX reageren.
Bovenste = sterkste dus deze reactie vindt plaats.

Richting: van zink naar koper. Zink staat elektronen af koper neemt elektronen op. Zink
negatieve pool en koper positieve pool.

Meer Zn2+ dan gaat Cl- uit de zoutbrug naar de oplossing zn2+ toe.
In een oplossing moet + en – lading gelijk zijn.

Elektrolyt = zoutoplossing

Wat kun je met deze cel?
Voorloper van de batterij. In serie schakelen levert hoeveelheid groter volt op.

Bronspanning (binas 48)
Standaardelektrodepotentiaal V0
0 (nul) bij waterstof. De recht + of -.

Δ V 0=V 0 OX −V 0 RED
Bronspanning voorbeeld van opstelling afbeelding.
Δ V 0=0,34−−0,76=1,10 V
= ideale situatie bij omstandigheden:
- P = P0
- T = 298 K (25 graden)

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