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Lithium

## INTRODUCTION: 
Can you imagine your life without batteries? Look around you. Nearly every other appliance that we see runs on batteries. Maybe it's your alarm clock or the remote for your television. The discovery of batteries has made our lives a lot easier. The smartphones we carry around with us or the laptops we use for our work all use some kind of battery. They are the reasons why we can carry these devices wherever we go without worrying about plugging them into a socket every time we wish to use them. 

Even our cars and bikes use batteries. Regardless of what type of battery we use, whether lithium-ion batteries or nickel-metal hydride batteries, they all serve the same purpose: to store electrical energy. Every single battery has a voltage marking, also known as standard cell potentials, that tells us how much energy a battery can hold. 

![Different-types-of-battery](//images.ctfassets.net/4yflszkpcwkt/1n768wOzRho6Cp2A80wDwC/2dd081c8465368ec88205c1de9e8754d/different-types-of-battery.jpg)
[Source](http://www.electronicsandyou.com/what-is-battery-types-of-battery-how-battery-works.html)

### CALCULATING STANDARD CELL POTENTIALS 

While determining the action voltage (pressure through an electrical circuit that pushes charged electrons) of a single electrode is difficult, we may give one a value of zero and use this as a baseline. The standard hydrogen electrode (SHE) is the electrode designated the zero value . The SHE comprises 1 atm hydrogen gas bubbling through a 1 M HCl solution at ambient temperature. The electrode is made of platinum, which itself is relatively inert. 

![CALCULATING STANDARD CELL POTENTIALS ](//images.ctfassets.net/4yflszkpcwkt/7FSK8vQhWdxjGL8mjH0U2m/00d5cfdfbe4b65b7e57bdff4356afcfc/CNX_Chem_17_03_SHE.jpg)
[Source](https://courses.lumenlearning.com/suny-albany-chemistry/chapter/standard-reduction-potentials/)

Standard cell potentials (SRP) may be computed by subtracting the standard anode reduction potential from the standard cathode reduction potential. 

![Standard cell potential formula](//images.ctfassets.net/4yflszkpcwkt/TlVseepQx8cPl5zptkPRu/e0546ef5a353bcccb0cd540d527912ca/Standard_cell_potential_formula.png)

The standard reduction potential of every element is already determined, and we can use this data while calculating the standard cell potential. The table below shows the SRP of different elements. There are many other uses of this data like finding out which element can act as an oxidizing agent or a reducing agent in a reaction.

![Standard-Electrode-Potential](//images.ctfassets.net/4yflszkpcwkt/5OyGeHOXJAIXJQyRHJotKZ/50562c743790e404d457ea831739e387/Standard-Electrode-Potential.jpg)
[Source](https://phas.ubc.ca/~jaymib/PhysicsConcepts.html)

### OXIDIZING AND REDUCING AGENTS 

There are several types of oxidizing agents and reducing agents. The standard reduction potentials may be thought of as a ranking of compounds based on their ability to oxidize and reduce. Compounds with high oxidation levels or high electronegativity that acquire electrons in the redox process are strong oxidizing agents. 

The reactants in the SRP table below H+ are greater oxidants than H+, whereas those above it are weaker.

## CONCLUSION:

- The standard cell potential is the voltage evaluated against a standard hydrogen electrode assuming standard circumstances. 
- Any electrochemical cell must be made up of two half-cells to work. 
- Standard cell potentials may be computed by subtracting the standard anode reduction potential from the standard cathode reduction potential. 

### FAQs:  
__1. How do you calculate the standard cell potential?__

Subtract the standard reduction potential for the reaction at the anode out from the standard reduction potential for the electrochemical process at the cathode. It gives us the standard reduction potential of the cell. Since oxidation is the inverse of reduction, the negative sign is required. 

__2. What is electrode potential?__

The potential of an electrode is defined as the potential of a unit in which the electrode in question serves as the cathode, and the standard hydrogen electrode serves as the anode. The anode is constantly oxidized, whereas the cathode is indeed reduced. 

__3.  How do you calculate standard cell potential from Delta G?__

The Gibbs free energy in a galvanic cell is linked to the potential by ΔG°cell = −nFE°cell.
If E°cell > 0, then the reaction is feasible. 

__4. What does electrode potential depend on?__

The oxidation potential is the propensity of an electrode to shed electrons, whereas the reduction potential is the capacity of an electrode to receive electrons. The potential of electrodes is determined by the concentration of metal ions and the temperature. 

*We hope you enjoyed studying this lesson and learned something cool about __How to calculate standard cell potential?__! Join our Discord community to get any questions you may have answered and to engage with other students just like you! Don't forget to download our App to experience our fun, VR classrooms - we promise, it makes studying much more fun!* 😎

## SOURCES: 
1. Calculating Standard Cell Potentials. https://www.ck12.org/c/chemistry/calculating-standard-cell-potentials/lesson/Calculating-Standard-Cell-Potentials-CHEM/. Accessed 27 Jan 2022.   
2. Oxidising and reducing agents. https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Supplemental_Modules_(Analytical_Chemistry)/Electrochemistry/Redox_Chemistry/Comparing_Strengths_of_Oxidants_and_Reductants. Accessed 27 Jan 2022.  
3. Calculating Standard Cell Potentials. https://courses.lumenlearning.com/suny-albany-chemistry/chapter/standard-reduction-potentials/.  Accessed 27 Jan 2022.  


The standard cell potential is the potential difference between cathode and anode.


Calculating Standard Cell Potentials Study Guide

## INTRODUCTION

We always keep a special check over the battery percentage of our phones! We rely on rechargeable batteries to operate our smartphones, desktop computers, and other portable electrical gadgets. What do we do when the battery dies?  
Batteries use a chemical process to produce electrical power, but this process slows down. You must invert the reaction to replenish the battery. This requires electric power, and you must charge the battery by plugging it in. The battery functions as an electrolytic cell while charging itself.

### ELECTROLYTIC CELLS

To define electrolytic cells, we need first to understand electrolysis. Electrolysis is a method that entails passing an electric current through a liquid containing ions, causing the compounds inside to disintegrate. This is used to isolate the metal from metallic elements, segregate other chemical substances (such as water) and electroplate metals, and recharge batteries. A complete circuit is essential to maintain an electrolytic process; we need to be able to draw electricity from the cell continually.

An electrolytic cell's cathode and anode are connected to a power source. These two stable electrodes and a fluid electrolyte solution are found in every electrolytic cell. The electrolyte solution conducts electricity since dissolved ions can move freely in the solution.

### WHAT HAPPENS INSIDE AN ELECTROLYTIC CELL?

Let’s have a look at the electrolytic cell diagram:

![Electrolytic-cells](//images.ctfassets.net/4yflszkpcwkt/51cHtu6MOfYxoKTPthlRjh/a1d3af301f8f8a4ca3ba19e5eef2f492/Electrolytic-cells-2-3-300x228.png)
[Source](https://www.online-sciences.com/chemistry/electrolytic-cells-structure-importance-and-difference-between-electrolytic-cell-galvanic-cell/)

The battery initially offers an electrical energy source by forcing electrons onto the cathode, which makes it negatively charged. The anode is also positively charged because electrons are taken out of it. An oxidation-reduction reaction is triggered as a result of this. An oxidation reaction happens at the anode, generating electrons drawn to the positive anode. Simultaneously, a reduction process occurs at the cathode, which consumes the electrons accumulated on the cathode. These reactions can be written as : 

Oxidation half of the reaction: A- --> e- A-
Reduction half of the reaction: B e- --> B

The end outcome of each of these processes is that two ions become neutral atoms (A or B). This is achieved by the battery's electrical energy, which transfers electrons from the anode to the cathode. 

## CONCLUSION

- Running electric current through a conductive solution or molten salt causes a chemical reaction called electrolysis. 
- A cell made up of electrolytes and electrodes used to drive a non-spontaneous redox reaction is called an electrolytic cell. 
- The two reactions in an electrolytic cell are: 

             Oxidation A- --> e- A-

             Reduction B e- --> B

### FAQs:

__1. How do electrons flow in an electrolytic cell?__

Electrons pass from the anode to the cathode through an external circuit in an electrolytic cell.

__2. Why do electrolytic cells require a battery?__

Electrolytic cells require an external electron source, such as a DC battery, because they involve non-spontaneous processes.

__3. How does charge travel in an electrolytic cell?__

The negatively charged electrons flow from cathode to anode in an electrolytic cell. 

*We hope you enjoyed studying this lesson and learned something cool about __Electrolytic Cells__! Join our Discord community to get any questions you may have answered and to engage with other students just like you! Don't forget to download our app to experience our fun VR classrooms - we promise it makes studying much more fun!* 😎

## SOURCES:
1. Electrolysis: https://www.sciencedirect.com/topics/earth-and-planetary-sciences/electrolysis. Accessed 24 Feb 2022.
2. Electrolytic Cells: https://www.ck12.org/c/chemistry/electrolytic-cells/lesson/Electrolytic-Cells-CHEM/. Accessed 24 Feb 2022.


Electrolytic cells convert electrical energy into chemical energy.

 Electrolytic Cells Study Guide

## INTRODUCTION 

What would our life be like if we didn't have batteries? Take a lookout. Almost every other appliance we see is powered by batteries. Maybe it's your television remote or your alarm clock. The invention of batteries has greatly simplified our lives. The batteries in the cell phones we carry with us or the computers we use for work are the reason we can take these gadgets with us everywhere we go without having to worry about plugging them in every time we want to use them. Even our automobiles and motorcycles run on batteries. Now let’s know about, what is in a battery and the battery’s working.

![Batteries](//images.ctfassets.net/4yflszkpcwkt/2b4xU8tYAfjqiHDhIxHpDe/bab0e53ead0989afe368325b785e8d0a/Batteries.jpg)
[Source](https://en.wikipedia.org/wiki/Electric_battery)

### WHAT IS A BATTERY?

- A battery comprises electrochemical cells that store chemical energy before converting it to electricity.
- The dry cell and the lead storage battery are two variants of the fundamental voltaic cell.

### DRY CELL:
- The electrolyte is immobilized as a paste in a dry cell, with barely enough moisture to permit current to pass. 
- Because it contains no loose liquid, unlike a wet cell, a dry cell may work in any direction without spilling. 
- Because of its adaptability, it's ideal for portable equipment. 
- The early wet-cell batteries, on the other hand, were often fragile glass canisters with lead rods suspended from an open top. As a result, they are required to be handled with care to avoid leakage. 
- The invention of the dry-cell battery resulted in significant improvements in battery safety and mobility.
- The zinc-carbon cell, which employs a cell known as the Leclanché cell, is a typical dry-cell battery. 
- The module is composed of an anode, which is a zinc container on the outside.
- A core carbon rod is flanked by a combination of carbon and manganese (IV) dioxide as the cathode (MnO₂). 
- The electrolyte is an ammonium chloride paste (NH₄Cl). The two electrodes are separated by fibrous material, and a brass peg in the cell's core carries electricity to the outside circuitry.
- To enable energy storage, there occur chemical reactions in a battery; the processes may be represented using balanced chemical equations that outline the electron flow. 

- The following half-reaction occurs when ammonium chloride paste is applied:

                  2NH₄(aq) + 2e −→ 2NH₃(g) + H₂(g)

- According to the following process, the manganese (IV) oxide in the cell eliminates the hydrogen generated by the ammonium chloride:

               2MnO₂(s) + H₂(g) → Mn₂O₃(s) + H₂O(l)

- At the cathode, the combined outcome of these two processes occurs. When we combine these two responses, we get:

            2NH₄(aq) + 2MnO₂(s) + 2e → Mn₂O₃(s) + 2NH₃(g) + H₂O(l)

- Finally, the half-reaction of the anode is as follows:

                          Zn(s) → Zn₂ + 2e−

- As a result, the cell's total equation is:

        Zn(s) + 2MnO₂(s) + 2NH₄(aq) → Mn₂O3(s) + H₂O(l) + Zn₂ + 2NH₃(g)

The above reaction has a potential of 1.50 V.

![Dry Cells](//images.ctfassets.net/4yflszkpcwkt/6y3MWr3VTd5Bh26PW3R8k6/edc4bfd997c69ef7f696a2bed47e7892/f-d_c3cc8ffc8f5e72ab7692b8cd107085ec466c01045355966bd1bf0348_IMAGE_THUMB_POSTCARD_TINY_IMAGE_THUMB_POSTCARD_TINY.1)
[Source](https://www.ck12.org/c/chemistry/batteries/lesson/Batteries-CHEM/)

### LEAD STORAGE BATTERY:

- Lead-acid batteries, often known as lead storage batteries, can hold a lot of charges and provide a considerable current for a small period.
- Lead-acid batteries can be recharged, which is crucial for their usage in automobiles.
- Both the positive and negative plates must become lead (II) sulphate, and the electrolyte must lose substantially of its dissolved sulfuric acid in order to discharge the stored energy.

![lead-storage-battery](//images.ctfassets.net/4yflszkpcwkt/7xDuHmlMcFRNPQ5xXDGRtQ/0b815ad26b9b043b6920a8ba75973648/lead-storage-battery.gif)
[Source](https://courses.lumenlearning.com/introchem/chapter/lead-storage-battery/)

## CONCLUSION:

- A battery is made up of electrochemical cells that store chemical energy before converting it to electricity.
- The dry cell and the lead storage battery are two variants of the fundamental voltaic cell.
- Lead storage batteries can hold a lot of charges and provide a considerable of current for a small period.

### FAQs: 

__1. What is a battery and what are its types?__

There are a few additional types of secondary batteries, but the 3 most common are: 

- Lead-acid Batteries
- Nickel-cadmium Batteries
- Lithium-ion Batteries

__2. What is the use of batteries?__

A battery is used to provide backup power during a power failure. The batteries are usually connected to electrical gadgets at home. These gadgets continue to function even if the power is out. Many clients, for example, have energy tariffs that vary depending on the time of day.

*We hope you enjoyed studying this lesson and learned something cool about __Batteries__! Join our Discord community to get any questions you may have answered and to engage with other students just like you! Don't forget to download our App to experience our fun VR classrooms - we promise, it makes studying much more fun!* 😎 

## SOURCES
1. Batteries: https://www.ck12.org/c/chemistry/batteries/lesson/Batteries-CHEM/. Accessed 16 March 2022.
2. Electric Battery: https://en.wikipedia.org/wiki/Electric_battery. Accessed 16 March 2022.
3. Batteries: https://courses.lumenlearning.com/boundless-chemistry/chapter/batteries/. Accessed 16 March 2022.


A battery comprises electrochemical cells that store chemical energy before converting it to electricity.


Batteries Study Guide

TL;DR Electrolytic Cells

TL;DR Batteries

Standard reduction potentials can be useful in determining the directionality of a reaction. Check out this cheat sheet to know more!