GCSE Chemistry Revision "Cells and Batteries" (Triple)

GCSE workbooks www.amazon.co....
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In this video, we learn how cells and batteries use a chemical reaction to produce electricity. We look at how the reactivities of the metals affect the potential difference produced and we learn the difference between rechargeable and non-rechargeable batteries.
This video is based on the AQA spec. If you are following a different exam board then you should check your specification. The Amazon link above is an affiliate link. This provides a small commission which helps to support freesciencelessons. The cost remains the same to you. If you prefer not to use this, you can search Amazon for the Freesciencelessons workbooks.
Image credits:
Duracell 9V battery. commons.wikime... (Ashley Pomeroy)
Several batteries (By BateriaR14.jpg: User:Julo derivative work: Palu (BateriaR14.jpg) [Public domain], via Wikimedia Commons)
Five AA batteries (By Cyberpunk - Own work, CC0, commons.wikime...)
Duracell rechargeable (By Dmitry G (Own work) [CC BY-SA 3.0 (creativecommons...) or GFDL (www.gnu.org/cop...)], via Wikimedia Commons)

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At 1:22 you say a chemical reaction is happening. What between?

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There are two reactions taking place: one between the electrolyte and the positive electrode, and one between the electrolyte and the negative electrode.

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Why does the current move in that direction?

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You don't need to memorise it. The information that you need will be given.

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Why do electrolytes have to be a solution of only IONIC compounds.

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Ionic compounds conduct electricity in aqueous solution. Covalent compounds do not.

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Hi. If you look in the playlist "Quantitative Chemistry", you will find all the videos on the mole.

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No it's the solution or liquid that electrolysis takes place in. It's not a catalyst.

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Very useful video but what do you mean when you say “we can reverse the chemical reactions when we apply an electrical current” on the rechargeable cell/battery? What does that do and how does it work? Thank you

[@Freesciencelessons]

A cell consists of a chemical reaction, in which an electrical current is generated. If we instead APPLY an electrical current, we can make the same chemical reaction go backwards (ie reverse). This means that we can recharge a spent battery (as long as it's rechargeable as we cannot recharge a normal battery).

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hi, why have you included tin and lead in the reactivity series at 2:13. In the reactivity series comment section, you said that the reactivity series you covered is the only one that comes up in the specification... so do we need to know the positions of tin and lead?

[@Freesciencelessons]

Hi, no you don't need to know those. I put them in because it nicely illustrates the idea that the potential difference depends on the difference in reactivity between the two metals.

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this is triple - and yet they're making us learn this as combined

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Hello, how does the electrolyte affect the voltage?

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The more concentrated the electrolyte is, the more voltage it produces

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do we need to know the reactivity series off by heart?

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The best cell uses electrodes with the largest difference in standard reduction potential.

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do we need to know what rechargeable batteries are made of?

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No not for AQA. Just that the chemical reaction can be reversed if you put an electrical current through.

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Does the rechargeable battery work because the current allows heat to be transferred to the reactants to allow the endothermic reaction to take place, resulting in the products which would then become the reactants of the exothermic reaction when the battery is removed?

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Is it essentially electrolysis that is producing the electricity, because the electrolyte can be an ionic compound? And when the reaction stops, is it due to a limiting factor?

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