Home

Chemistry

Redox and cells

Energy storage cells and hydrogen fuel cells

Energy storage cells and hydrogen fuel cells

Videos

Summary

Exercises

Select Lesson

Exam Board

Select an option

Practical skills

The scientific method

How to plan experiments

Improving repeatability and reproducibility

Presenting results using tables and graphs

Analysing results: anomalies and correlation

Evaluating experiments

Modern analytical techniques II

NMR spectroscopy

Proton NMR spectroscopy

Chromatography

Combining analytical techniques

Organic chemistry III

Benzene: structure and combustion

Electrophilic substitution

Friedel-Crafts reactions

Phenols

Aliphatic and aromatic amines

Reactions of amines

Forming amides

Condensation polymers

Amino acids and zwitterions

Grignard reagents

Synthetic routes

Practical techniques

Percentage composition and combustion analysis

Organic chemistry II

Optical isomers and chirality

Aldehydes and ketones

Carboxylic acids: properties and reactions

Esters: formation, properties and uses

Acyl chlorides: formation and reactions

Kinetics II

Measuring rates of reaction

Determining reaction orders

The initial rates method

Rate equations and the rate constant

The rate determining step

Halogenoalkane reaction mechanisms

Activation energy and the Arrhenius equation

Transition metals

Transition metals: electron configuration and oxidation number

Complex ions: formation, shape and isomerism

Colours of inorganic ions and complexes

Chromium and its reactions

Ligand substitution reactions

Transition metals as catalysts

Redox II

Electrochemical cells and redox

Electrode potentials and calculations

The electrochemical series

Energy storage cells and hydrogen fuel cells

Redox titrations

Energetics II

Lattice enthalpies and Born-Haber cycles

Polarisation and the Pauling scale

Enthalpy change in solution

Entropy and calculating entropy change

Gibbs free energy change

Acid-base equilibria

Acids and bases

pH calculations

The ionic product of water

pH curves and indicators

Buffer solutions and calculations

Equilibrium II

The equilibrium constant

Partial pressure and gas equilibria

Le Chatelier's principle and equilibrium constants

Equilibrium I

Reversible reactions

Le Chatelier's principle

Kinetics I

Collision theory and rates of reaction

Calculating the rate of reaction

Catalysts and the Maxwell-Boltzmann distribution

Energetics I

Enthalpy changes and reaction profiles

Standard enthalpy changes

Hess's Law and enthalpy cycles

Calculating bond enthalpies

Modern analytical techniques I

Mass spectrometry

IR spectroscopy

Organic chemistry I

Basic concepts of organic chemistry

Organic reactions and mechanisms

Structural isomerism

Alkanes and free radical substitution

Fractional distillation of crude oil

Fuels: combustion and emissions

Alkenes: bonding and reactivity

Stereoisomerism

Reactions of alkenes

Addition polymerisation

Halogenoalkanes and their reactions

Alcohol: classification and reactions

Oxidation of alcohols

Organic techniques

Formulae, equations and amounts of substances

The mole and Avogadro's constant

Calculations involving gases

Empirical and molecular formulae

Balancing equations

Acid-base titrations

Calculating uncertainty and errors

Atom economy and percentage yield

Inorganic chemistry and the periodic table

Group 2: ionisation energy and properties

Thermal stability of nitrates and carbonates

Chemical properties of Group 7

Reactions with halogens

Halide ion reactions

Testing for ions

Redox I

Calculating oxidation numbers

Oxidation, reduction and redox reactions

Bonding and structure

Ionic bonding

Covalent bonding

Shapes of molecules

Giant covalent and metallic structures

Electronegativity and polarisation

Intermolecular forces: types and examples

Hydrogen bonding

Solubility

Predicting structures and properties

Atomic structure and the periodic table

The atom: history, structure and isotopes

Relative masses and mass spectrometry

Electronic structure: shells and orbitals

Atomic emission spectra

Ionisation energies

Ionisation energy trends

Periodicity

Explainer Video

Tutor: Sophie

Summary

​​Energy storage cells and hydrogen fuel cells

​​In a nutshell

The cell potential of energy storage cells can be calculated using the electrode potentials. Lithium batteries are rechargeable and are commonly seen in phones and laptops. Hydrogen fuel cells can produce electricity by reacting hydrogen and oxygen to form water under acidic or alkaline conditions. 



Energy storage cells

Batteries are energy storage cells, which work in a similar way to electrochemical cells. The cell potential of energy storage cells and overall reaction can be determined, if you know the half equations and their electrode potentials. 


Example

The Ni/ZnNi/ZnNi/Zn battery has a Ni(OH)2Ni(OH)_2Ni(OH)2​ cathode, a ZnZnZn anode and a KOHKOHKOH electrolyte solution. 

location

half equation

Voltage

Anode
​Zn(OH)2+2e−⇋Zn+2OH−Zn(OH)_2+2e^-\leftrightharpoons Zn+2OH^-Zn(OH)2​+2e−⇋Zn+2OH−​​
​−1.24 V-1.24\ V−1.24 V​​
Cathode
​NiO(OH)+H2O+e−⇋Ni(OH)2+OH−NiO(OH)+H_2O+e^-\leftrightharpoons Ni(OH)_2+OH^-NiO(OH)+H2​O+e−⇋Ni(OH)2​+OH−​​
​+0.49 V+0.49\ V+0.49 V​​
Overall
​2NiO(OH)+Zn+2H2O→2Ni(OH)2+Zn(OH)22NiO(OH)+Zn+2H_2O\rightarrow 2Ni(OH)_2+Zn(OH)_22NiO(OH)+Zn+2H2​O→2Ni(OH)2​+Zn(OH)2​​​
​+1.73 V+1.73\ V+1.73 V​​


To determine the overall reaction from the half equations, you can determine that both equations have electrons and OH−OH^-OH− ions so they must be either side of the reaction to balance out. The cathode half equation must be doubled so each equation has 2e−2e^-2e− and  2OH−2OH^-2OH− to give you:


​2NiO(OH)+2H2O+2e−⇋2Ni(OH)2+2OH−2NiO(OH)+2H_2O+2e^-\leftrightharpoons2Ni(OH)_2+2OH^-2NiO(OH)+2H2​O+2e−⇋2Ni(OH)2​+2OH−


At the anode, ZnZnZn must lose electrons so oxidation can occur so the half equation will start with ZnZnZn to give:


Zn+2OH−→Zn(OH)2+2e−Zn+2OH^-\rightarrow Zn(OH)_2+2e^-Zn+2OH−→Zn(OH)2​+2e−


This can now be combined with the cathode to give you the overall equation:


2NiO(OH)+Zn+2H2O→2Ni(OH)2+Zn(OH)22NiO(OH)+Zn+2H_2O\rightarrow 2Ni(OH)_2+Zn(OH)_22NiO(OH)+Zn+2H2​O→2Ni(OH)2​+Zn(OH)2​​​


To work out cell potential which is given as +1.73 V+1.73\ V+1.73 V, the following equation must be used:


Ecell=E(reduction)θ−E(oxidation)θE_{cell}=E^\theta_{(reduction)}-E^\theta_{(oxidation)}Ecell​=E(reduction)θ​−E(oxidation)θ​​​

​Ecell=0.49−(−1.24)E_{cell}=0.49-(-1.24)Ecell​=0.49−(−1.24)​​

​Ecell=0.49+1.24E_{cell}=0.49+1.24Ecell​=0.49+1.24​​

​Ecell=+1.73 VE_{cell}=+1.73\ VEcell​=+1.73 V​​



Lithium batteries

Rechargeable lithium cells are used in mobile phones and laptops to provide energy.  As lithium batteries have reversible reactions, they are recharged by supplying a current which forces the electrons to flow in the reverse direction. 


Lithium batteries are initially expensive but they have longer lifetimes and can be reused, so are cheaper in the long-term. Lithium is flammable and reactive, so the batteries have a risk of catching fire if the device overheats. Toxic chemicals are used to produce many energy storage cells so they must be disposed of correctly.



Hydrogen fuel cells

Fuel cells are different to other energy storage cells as the chemicals are stored outside of the cell,  whereas for most cells the chemicals will be within the cell in the electrodes. One of the most common fuel cell is the alkaline hydrogen-oxygen fuel cell which can be used as a source of power for electric vehicles. 


Hydrogen gas fuel is reacted with an oxidant such as oxygen gas by feeding the two gases into the cell when electricity is required. An alkaline KOHKOHKOH electrolyte is used as a source of hydroxide ions. The overall reaction is between hydrogen and oxygen to form water. 


Example
Chemistry; Redox II; KS5 Year 12; Energy storage cells and hydrogen fuel cells

location

half equation

Anode
​2H2+4OH−→4H2O+4e−2H_2+4OH^-\rightarrow 4H_2O+4e^-2H2​+4OH−→4H2​O+4e−​​
Cathode
​O2+2H2O+4e−→4OH−O_2+2H_2O+4e^-\rightarrow 4OH^-O2​+2H2​O+4e−→4OH−​​
Overall
​2H2+O2→2H2O2H_2+O_2\rightarrow 2H_2O2H2​+O2​→2H2​O​​



Generating electricity in an alkaline Hydrogen fuel cell

1.
At the anode, hydrogen is fed in and it is reacted with hydroxide ions to produce water and electrons.
2.
The anion-exchange membrane that separates the electrodes allows water and hydroxide ions to pass through, only.
3.
Electrons cannot pass through the membrane, so they pass through an external circuit from the anode to the cathode which generates an electric current.
4.
At the cathode, oxygen is fed in and it is reacted with water and electrons from the circuit, forming hydroxide ions.
5.
The hydroxide ions from the anode, can pass through the membrane to react with hydrogen at the cathode. 


Electricity can also be generated from hydrogen and oxygen gas using acidic conditions instead. A polymer electrolyte membrane (PEM) is used which only allows the flow of H+H^+H+ across. This process produces water which is the only waste product involved.


Example
Chemistry; Redox II; KS5 Year 12; Energy storage cells and hydrogen fuel cells


location

half equation

Anode
​H2→2H++2e−H_2\rightarrow 2H^++2e^-H2​→2H++2e−​​
Cathode
​12O2+2H++2e−→H2O\frac{1}{2}O_2+2H^++2e^-\rightarrow H_2O21​O2​+2H++2e−→H2​O​​
Overall
​H2+12O2→H2OH_2+\frac{1}{2}O_2\rightarrow H_2OH2​+21​O2​→H2​O​​


Generating electricity in an acidic hydrogen fuel cell

1.
Hydrogen is fed in at the anode and split into protons and electrons by the catalytic platinum electrode.
2.
The protons can pass through the PEM which forces the electrons through the electrical circuit, from the anode to the cathode, generating an electric current.
3.
Oxygen is fed in at the cathode which combines with the protons and electrons to form water.



Advantages and disadvantages of hydrogen fuel cells

Advantages

Disadvantages

Produce energy more efficiently than combustion engines which lose energy in the form of heat.

Produce less pollution and only have one waste product (water) compared to CO2CO_2CO2​ and other toxic pollutants which are produced from combustion engines.

No need to be recharged, a constant supply of oxygen and hydrogen will produce electricity. Water waste can also be reused to supply hydrogen and oxygen.
Energy is needed to produce the supply of hydrogen and oxygen which requires electricity, usually from the burning of fossil fuels. 

Hydrogen is a flammable gas so needs to be stored and transported with care.
Read more

Learn with Basics

Learn the basics with theory units and practise what you learned with exercise sets!
Length:
Electrolysis

Unit 1

Electrolysis

Chemical and fuel cells

Unit 2

Chemical and fuel cells

Jump Ahead

Score 80% to jump directly to the final unit.

Optional

Energy storage cells and hydrogen fuel cells

Unit 3

Energy storage cells and hydrogen fuel cells

Final Test

Test reviewing all units to claim a reward planet.

Create an account to complete the exercises

FAQs - Frequently Asked Questions

What is the overall reaction for a hydrogen fuel cell?

The overall reaction for a hydrogen fuel cell: Oxygen reacting with hydrogen to form water.

How are hydrogen fuel cells different to other energy storage cells?

Hydrogen fuel cells are different as they store the chemicals separately from the cell, rather than within the cell. They are fed in when electricity is required.

How are lithium batteries recharged?

Lithium batteries can be recharged as the half reactions are reversible. When a current is applied, this forces the electrons in the reverse direction and the reverse reactions occur.

©2020 - 2024 evulpo AG

Beta