Chemsheets AS006 (Electron arrangement)

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Presentation transcript:

Chemsheets AS006 (Electron arrangement) 08/05/2018 Adapted from: www.CHEMSHEETS.co.uk ELECTROCHEMISTRY Cells and batteries © www.chemsheets.co.uk A2 046 20-Jul-12

Non-rechargeable (primary) cells – Zinc-carbon -0.80 V Zn(NH3)22+ + 2 e- ⇌ Zn + 2 NH3 +0.70 V 2 MnO2 + 2 H+ + 2 e- ⇌ Mn2O3 + H2O Standard cell Short life Determine: a) cell emf b) overall reaction during discharge

Non-rechargeable (primary) cells – alkaline -0.76 V Zn2+ + 2 e- ⇌ Zn +0.84 V MnO2 + H2O + e- ⇌ MnO(OH) + OH- Determine: a) cell emf b) overall reaction during discharge Longer life

Non-rechargeable (primary) cells – lithium Very long life High voltage Determine: a) cell emf b) overall reaction during discharge

Rechargeable (secondary) cells In non-rechargeable (primary) cells, the chemicals are used up so the voltage drops In rechargeable (secondary) cells the reactions are reversible – they are reversed by applying an external current. It is important that the products from the forward reaction stick to the electrodes and are not dispersed into the electrolyte.

Rechargeable (secondary) cells – Li ion +0.60 V Li+ + CoO2 + e- ⇌ LiCoO2 -3.00 V Li+ + e- ⇌ Li Rechargeable Most common rechargeable cell Determine: a) cell emf b) overall reaction during discharge c) overall reaction during re-charge

Rechargeable (secondary) cells – lead-acid +1.68 V PbO2 + 3 H+ + HSO4- + 2 e- ⇌ PbSO4 + 2 H2O -0.36 V PbSO4 + H+ + 2 e- ⇌ Pb + HSO4- Determine: a) cell emf b) overall reaction during discharge c) overall reaction during re-charge Used in sealed car batteries (6 cells giving about 12 V overall)

Rechargeable (secondary) cells – nickel-cadmium +0.52 V NiO(OH) + 2 H2O + 2 e- ⇌ Ni(OH)2 + 2 OH- -0.88 V Cd(OH)2 + 2 e- ⇌ Cd + 2 OH- Determine: a) cell emf b) overall reaction during discharge c) overall reaction during re-charge

FUEL CELLS High efficiency (more efficient than burning hydrogen) How is H2 made? Input of H2/O2 to replenish so no need to recharge +0.40 V O2 + 2 H2O + 4 e- ⇌ 4 OH- -0.83 V 2 H2O + 2 e- ⇌ H2 + 2 OH- Determine: a) cell emf b) overall reaction

From wikipedia (public domain)

Pros & cons of cells + portable source of electricity Pros & cons of non-rechargeable cells + cheap, small – waste issues Pros & cons of rechargeable cells + less waste, cheaper in long run – still some waste issues Pros & cons of fuel cells + water is only product – most H2 is made using fossil fuels, fuels cells expensive