Electrochemical cells and fuel cells are game-changers in energy conversion. They turn chemical energy into electrical power through redox reactions, with electrons moving between electrodes. The magic happens thanks to the Gibbs free energy and cell potential .
Fuel cells take this concept further, offering clean power for various applications. From hydrogen-powered cars to natural gas-fueled power plants, these devices are reshaping our energy landscape. Their efficiency depends on factors like temperature, pressure, and catalysts.
Electrochemical Cells
Principles of electrochemical cells
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Convert chemical energy into electrical energy through redox reactions
Involve transfer of electrons between species
Oxidation releases electrons at anode (zinc electrode)
Reduction accepts electrons at cathode (copper electrode)
Gibbs free energy (Δ G \Delta G Δ G ) determines spontaneity and maximum electrical work
Negative Δ G \Delta G Δ G indicates spontaneous reaction and positive electrical work (galvanic cell )
Positive Δ G \Delta G Δ G indicates non-spontaneous reaction and negative electrical work (electrolytic cell )
Relationship between Δ G \Delta G Δ G and cell potential (E c e l l E_{cell} E ce ll ) given by Δ G = − n F E c e l l \Delta G = -nFE_{cell} Δ G = − n F E ce ll
n n n is number of electrons transferred per mole of reaction
F F F is Faraday's constant (96,485 C/mol)
EMF calculation using Nernst equation
Relates cell potential (E c e l l E_{cell} E ce ll ) to standard cell potential (E c e l l ∘ E_{cell}^{\circ} E ce ll ∘ ) and concentrations of reactants and products
Nernst equation E c e l l = E c e l l ∘ − R T n F ln Q E_{cell} = E_{cell}^{\circ} - \frac{RT}{nF} \ln Q E ce ll = E ce ll ∘ − n F RT ln Q
R R R is universal gas constant (8.314 J/mol·K)
T T T is absolute temperature (K)
Q Q Q is reaction quotient, ratio of product concentrations to reactant concentrations raised to stoichiometric coefficients
Standard cell potential (E c e l l ∘ E_{cell}^{\circ} E ce ll ∘ ) determined by difference between standard reduction potentials of half-reactions
E c e l l ∘ = E c a t h o d e ∘ − E a n o d e ∘ E_{cell}^{\circ} = E_{cathode}^{\circ} - E_{anode}^{\circ} E ce ll ∘ = E c a t h o d e ∘ − E an o d e ∘
Standard reduction potentials listed in reference tables for various half-reactions (hydrogen electrode , silver chloride electrode )
Fuel Cells
Fuel cell types and applications
Electrochemical devices convert chemical energy of fuels directly into electrical energy
Common types
Proton exchange membrane fuel cells (PEMFCs)
Use hydrogen as fuel and oxygen as oxidant
Applications in transportation (vehicles) and portable power (laptops)
Solid oxide fuel cells (SOFCs)
Use hydrocarbons (natural gas) or hydrogen as fuel and oxygen as oxidant
Applications in stationary power generation (power plants)
Molten carbonate fuel cells (MCFCs)
Use hydrocarbons as fuel and oxygen as oxidant
Applications in large-scale power generation (industrial facilities)
Consist of anode, cathode, and electrolyte
Fuel oxidized at anode, releasing electrons
Oxidant reduced at cathode, accepting electrons
Electrolyte allows transfer of ions between electrodes (proton exchange membrane, solid oxide, molten carbonate)
Thermodynamics of fuel cell reactions
Efficiency determined by ratio of electrical energy output to chemical energy input
Efficiency = E l e c t r i c a l e n e r g y o u t p u t C h e m i c a l e n e r g y i n p u t \frac{Electrical \: energy \: output}{Chemical \: energy \: input} C h e mi c a l e n er g y in p u t El ec t r i c a l e n er g y o u tp u t
Thermodynamic efficiency limited by Gibbs free energy change of reaction
Maximum thermodynamic efficiency = Δ G Δ H \frac{\Delta G}{\Delta H} Δ H Δ G
Δ H \Delta H Δ H is enthalpy change of reaction
Factors affecting efficiency
Operating temperature
Higher temperatures improve efficiency by increasing reaction rates and reducing activation losses
Pressure
Higher pressures increase efficiency by improving mass transport and reducing concentration losses
Catalyst
Effective catalysts (platinum) reduce activation energy and improve reaction kinetics
Fuel and oxidant composition
Impurities in fuel or oxidant reduce efficiency by causing side reactions or poisoning catalyst