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Electrochemical Cell

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Electrochemical Cell

In this article, we will go over electrochemical cells, what they are, and some of their applications. Electrochemical cells are very crucial for the development of many different industrial materials and reagents. They can also be used for the determination of thermodynamic constants for reactions, which is why electrochemistry is such a crucial part of physical chemistry.

  • We'll first cover the definition and types of electrochemical cells.
  • We'll then go over the features of electrochemical cells, with a diagram.
  • We'll then look at various applications of electrochemical cells.
  • We'll find the standard cell potential and also calculate Gibbs free energy and the equilibrium constant.
  • We'll then cover how to predict the direction of redox.

Definition of Electrochemical Cell

Electrochemical cells are the main sites for electrochemical reactions to take place. So what are they exactly?

Electrochemical cells provide the means to control redox reactions. They can be divided into voltaic and electrolytic cells.

The main concept of electrochemical cells is that they allow a redox reaction to be split, in order to control it. In redox reactions, the processes of oxidation and reduction occur simultaneously. This means that splitting these two processes apart can be used for specific chemical needs. By splitting the reaction, you can control the flow of electrons between the oxidation and reduction half-reactions.

The flow of electrons in an electrochemical cell will be through a circuit, and it will be in the form of an electrical current.

Electrochemical cells are complete circuits, which means that even though they take apart the given redox reaction, they are connected at two points: the external circuit and the salt bridge. The external circuit will allow for the transfer of electrons, while the salt bridge will facilitate the mobility of the anions of the reaction. This way the reaction forms a circuit and is able to proceed.

Below we will talk about the definition of each electrochemical cell.

Types of Electrochemical Cells

Here we will discuss the two types of general electrochemical cells: voltaic and electrolytic. More importantly, we will focus on how they differ from each other, and how they were developed for different purposes and chemical needs.

Voltaic (Galvanic) Cell

A voltaic cell is an electrochemical cell which facilitates a spontaneous reaction.

A spontaneous redox reaction is a reaction that can thermodynamically proceed without requiring additional energy to be placed into the system.

These types of reactions will cause energy to be released. By creating a voltaic cell, you can monitor the energy through a voltmeter, as electrons will flow in the external circuit creating electricity.

Voltaic cells have two half-cells, each of which facilitate a single half-reaction, be it oxidation or reduction. You will see a diagram of this in the next section. The two half cells are connected by a salt bridge to promote the mobility of anions through the solutions, completing the circuit. This is opposed to how electrolytic cells are comprised.

Electrolytic Cell

Electrolytic cells usually don't have half-cells, but rather are performed in a single reaction compartment, such as a single beaker. This is because the reaction we are trying to perform is non-spontaneous, so mixing the reagents will not result in a reaction.

In electrolysis, the reaction you are trying to perform is non-spontaneous, meaning that you have to put energy into the system to make the reaction proceed. Applying a current to the reaction through electrodes will cause oxidation at one electrode and reduction at the other electrode. A current, being a stream of electrons, will supply energy and shift the equilibrium of the reaction to one side.

Electrochemical Cell Diagram

Here we will go through and represent a diagram of an electrochemical cell, specifically a voltaic (galvanic) cell.

Diagram. Electrochemical Cells. StudySmarterA voltaic electrochemical cell diagram depicting a Copper-Zinc cell. Source: glossary.periodni.com

Above you will see the diagram of an electrochemical cell depicting the reaction of Zinc with Copper Sulphate. Here Zinc is oxidised, since it loses electrons, while Copper is reduced, since it gains electrons.

Below the diagram, you will notice the half-reactions for each half-cell. These will tell you what reaction is occurring at each electrode. The electrodes are labelled above to state which one is the anode and which one if the cathode. Additionally, below the diagram you will find the cell notation for the reaction.

The electrochemical cell notation gives you insight on the type of reactants involved in the cell, how the cell is constructed, as well as which half-reaction undergoes oxidation and which reduction. This information can tell you in which direction the flow of electrons is going.

In the next section, we will talk about the different features of electrochemical cells.

Features of Electrochemical Cells

Electrochemical cells are composed of many different components, as seen in the diagram above. Here, we will discuss the main components of electrochemical cells. These are often the same in voltaic and electrolytic cells.

Electrodes

There will be two electrodes in each electrochemical reaction. Each electrode will function to carry out a specific half-reaction. These will be either oxidation or reduction.

The electrodes can be either made from a metal that will participate in the reaction, or they can be inert. Inert electrodes do not participate chemically in the reaction, as they will be made of either graphite or platinum.

Connectors: External Circuit and Salt Bridge

In an electrochemical cell, be it voltaic or electrolytic, there will be a need for an external circuit where the current can be carried. The flow of electrons generated in the reaction will be transferred through this circuit.

On the other hand, the flow of anions will be facilitated by the salt bridge. This is usually an external piece of equipment that is porous and can support the flow of anions but not the cations. Additionally, this can be either an external tube or a thin membrane separating different parts of the same beaker.

Additional Accessories

Other components which are crucial for electrochemical cells include the storage compartment of the reaction, which can be either a single beaker, as seen in electrolysis reactions, or two beakers, which act as half cells for the redox reaction.

Additionally, another component which deals with the flow of electrons is necessary. This regulatory equipment for electricity can be either in the form of a voltage meter, for voltaic cells, or a battery (or other power source) for electrolytic cells. These components directly monitor and modulate the flow of electrons in the electrochemical cell.

Applications of Electrochemical Cells

Here we will discuss the main applications of electrochemical cells, which concern calculating the standard cell potential and other thermodynamic values of electrochemical reactions.

Standard Cell Potential

So what is cell potential?

Standard cell potential refers to the voltage produced by the voltaic electrochemical cell.

So there are two ways which can be used to find the standard cell potential for a reaction.

  1. Perform the reaction and read the voltage meter.
  2. Calculate the standard cell potential from standard electrode potentials.

Here, we will focus on how to calculate the standard cell potential by combining two standard electrode potentials.

Standard electrode potentials are measured by performing the electrochemical reaction connecting the given half cell to a standard hydrogen electrode. This will give you either a positive or a negative voltage reading which you can use for calculations with other electrode potentials, as they are all relative to the standard hydrogen electrode potential. This means that you can "zero out" the standard hydrogen electrode to perform these calculations.

You can find information on different standard electrode potentials in a table such as this one (you can probably find one at the end of your chemistry textbook):

Electrochemical Cells Standard electrode potentials StudySmarter OriginalsTable of standard electrode potentials. Source: inspiritvr.com

Above you can see all the different voltage values for different electrode potentials.

To calculate the standard electrode potential of an electrochemical cell, use the following formula:

E0cell = E0red - E0oxid

Here we will calculate the standard cell potential for the Copper and Zinc cell.

We know that the electrode values for the standard electrode potentials for the reduction of Cu is +0.34, while for the oxidation of Zn it's -(-0.76).

Remember to flip the sign when going from oxidation to reduction, as the reaction is reversed (from the state in which it is written in the table).

Thus:

E0cell = + 0.34 - (-0.76)

E0cell = + 1.0988 volts

Other Thermodynamic Factors

The standard cell potential is related to other thermodynamic aspects, such as Gibbs free energy, the equilibrium constant, and entropy.

Gibbs Free Energy

Gibbs free energy (ΔG) determine the amount of energy in the system. This is the energy that can be put to work.

Take a look at the following equation:

ΔG = nFEcell

This equation joins the parameters of Gibbs free energy with the cell potential. Through this equation, you can calculate Gibbs free energy just by knowing the cell potential of a reaction, or the other way round.

This is because the other components in the equation are constants: "n" is the number of electrons involved in the reaction, while "F" is Faraday's Constant (= 96,485 C/mol).

Equilibrium Constant

The equilibrium constant (K) gives us the ratio of the products to the reactants.

We can use the equilibrium constant to monitor the redox reaction.

Take a look at the following equation:

ΔG0 = RTlnK

Thus:

nFE0cell = RTlnK

Hence:

E0cell = (RTlnK) / (nF)

Through this equation, you can find the equilibrium constant by knowing the standard cell potential or the other way round. This is because the other values in the formula are constants: "T" being the temperature in K, and "R" being the gas constant (= 8.314 joule kelvin−1 mole−1).

Predicting Redox Direction

Predicting the redox direction, or in other words the direction of electron flow, depends on the electrodes and the reactions they facilitate.

So, we know that in a redox reaction there will be oxidation and reduction occurring simultaneously. The electrodes split those two processes apart.

The reduction will occur at the cathode, while oxidation will occur at the anode. One you have figured out which electrode is the cathode and which one is the anode, predicting the direction of electron flow should be easy.

Electrons will flow from the anode to the cathode.

Electrochemical Cells - Key takeaways

  • Electrochemical cells facilitate redox reactions.
  • They can be electrolytic or voltaic cells.
  • Electrochemical cells contain 2 electrodes connected by an external circuit and a salt bridge.
  • You can use electrochemical cells to measure the standard cell potential.
  • By knowing the standard cell potential, you can measure the Gibbs free energy and equilibrium constant.
  • We can also predict the flow of electrons (anode to cathode).

Frequently Asked Questions about Electrochemical Cell

An electrochemical cell facilitates the control of a redox reaction. By splitting the processes of oxidation and reduction, an electrochemical cell can control the flow of electrons.

There are two types of cells. Voltaic (galvanic) cells allow spontaneous redox reactions to take place, while electrolytic cells put in electrical energy to facilitate a reaction. 

One application of an electrochemical cell would be to measure the standard cell potential, which can then be used to calculate other thermodynamic constants.

The most common features include the presence of a salt bridge, and two electrodes connected by an external circuit.

Electrochemical cells are able to provide thermodynamic insights on reactions, and they can also be used to manufacture reagents. 

Final Electrochemical Cell Quiz

Question

What is an electrochemical cell?

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Answer

Electrochemical cells are devices that turn chemical energy into electrical energy through redox reactions that involve the transfer of electrons.

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Question

What is a battery?

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Answer

A collection of electrochemical cells joined together.

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Question

How many half cells do you need to create an electrochemical cell?

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Answer

2

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Question

Which of the following are required to make an electrochemical cell?

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Answer

Two electrodes

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Question

True or false? In an electrochemical cell, the electrons move from the more reactive metal to the less reactive metal.

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Answer

True

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Question

True or false? All electrochemical cells use metals as their electrodes.

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Answer

False

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Question

Zinc-carbon batteries are a type of ____.

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Answer

Non-rechargeable battery

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Question

Lithium ion batteries are a type ____.

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Answer

Rechargeable battery

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Question

Hydrogen fuel cells are a type of ____.

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Answer

Fuel cell

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Question

In electrochemical cells, oxidation occurs at the ____.

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Answer

Anode

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In electrochemical cells, reduction occurs at the ____.

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Answer

Cathode

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Question

Which of the following are true when it comes to electrochemical cells?

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Answer

The anode is the negative electrode

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Question

Give two advantages of non-rechargeable batteries.

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Answer

  • They are cheap.
  • They last a long time.

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Give two disadvantages of non-rechargeable batteries.

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Answer

  • They can only be used once.
  • They are toxic.

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Question

Give two advantages of rechargeable batteries.

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Answer

  • They can be recharged and used again.
  • They produce less waste than non-rechargeable batteries.

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Question

Give two disadvantages of rechargeable batteries.

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Answer

  • They are more expensive than non-rechargeable batteries.
  • They are more sensitive to temperature fluctuations.

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Question

Give two advantages of hydrogen fuel cells.

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Answer

  • They don't produce any toxic products.
  • They can be a carbon-free source of electricity.

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Question

Give two disadvantages of hydrogen fuel cells.

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Answer

  • The fuel is flammable and requires careful storage.
  • Hydrogen has a low energy density and takes up a lot of space.

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Question

What are the two types of electrochemical cells?

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Answer

Electrolytic and voltaic

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Question

In which direction do electrons flow between the electrodes?

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Answer

Anode to cathode

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Question

Can oxidation occur at both electrodes of the electrochemical cell?

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Answer

No

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Question

What is the abbreviation of the "electromotive force"?

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Answer

EMF

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Question

What does a voltmeter measure?

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Answer

Voltage (not volts!)

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What are the units of EMF?

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Answer

Volt (V)

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If a reaction is spontaneous, will it show a voltmeter reading?

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Answer

Yes

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What device can measure volts?

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Answer

The voltmeter

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Question

What information do you need to know if you would like to calculate the EMF of a cell?

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Answer

The standard electrode potentials of the half cells involved. 

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Question

State two constants which you can determine from knowing the EMF of a cell?

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Answer

The Gibbs free energy and the equilibrium constant. 

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Question

If a reaction produces a flow of electrons, is it electrolytic or voltaic?

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Answer

Voltaic

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What other key constants do you need to know if you want to calculate the EMF of a call from the Gibbs free energy?

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Answer

Faraday's constant and the stoichiometry of the reaction. 

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Which of the following information can the Gibbs free energy tell us about the reaction?

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Answer

Its spontaneity 

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If you know the equilibrium constant of a reaction, can you know the standard cell potential of the reaction?

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Answer

Yes

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Question

If an EMF is negative is the reaction spontaneous or not?

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Answer

Spontaneous

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Can you learn about the kinetics of the reaction just by knowing the EMF?

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Answer

No

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What is the SI unit of measurement for the electromotive force?

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The volt (v)

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Does the voltmeter influence the reaction chemically?

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Answer

No

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Question

In which directions do electrons flow between the electrodes?

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Answer

From the anode to the cathode

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How can you predict electron flow in an electrochemical cell?

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Answer

Determine which electrode is the anode and cathode, which will allow you to know that electrons flow from the anode to the cathode. 

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What are the two types of electrochemical cells?

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Answer

Voltaic and electrolytic cells

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Can you use electrochemical cells to measure the standard cell potential?

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Answer

Yes

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Question

What other thermodynamic constants can you determine if you know the standard cell potential?

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Answer

Gibbs Free energy and the equilibrium constant.

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Question

What is the relationship between the standard electrode potential and gibbs free energy?

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Answer

The relationship is defined by the following equation: ΔnFEcell

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Question

What is the relationship between the standard electrode potential and the equilibrium constant?


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Answer

The relationship is defined by the following equation: E0cell = (RTlnK) / (nF)

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What are the two ways you can determine the standard electrode potential?

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Answer

Experimentally (voltmeter reading) or by calculations. 

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Question

What is the equation for calculating the standard cell potential from standard and electrode potentials? 

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Answer

E0cell E0red - E0oxid

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Question

How is the standard electrode potential calculated?

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Answer

The electrode is compared to the standard hydrogen electrode (SHE)

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Question

What are the most important features of an electrochemical cell?

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Answer

Electrodes, Circuit, and Salt Bridge

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Question

At which electrode does oxidation occur in a voltaic cell?

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Answer

Anode

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Question

At the cathode, which redox process occurs?

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Answer

Reduction

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