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Electrolysis: Aqueous Solutions and Half Equations đŸ§Ș GCSE Chemistry Learning & Revision

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Manage episode 483873400 series 3139602
Content provided by Seneca Learning. All podcast content including episodes, graphics, and podcast descriptions are uploaded and provided directly by Seneca Learning or their podcast platform partner. If you believe someone is using your copyrighted work without your permission, you can follow the process outlined here https://player.fm/legal.

In this episode, we will discuss the electrolysis of aqueous solutions and half equations.

Predicting products during the electrolysis of aqueous solutions is complex due to water's dissociation into hydrogen and hydroxide ions.

At the positive electrode (anode), either halogens form if halide ions are present, or oxygen gas is produced otherwise.

Conversely, at the negative electrode (cathode), hydrogen gas evolves if the metal is more reactive than hydrogen, while the metal itself deposits if it's less reactive.

These electrode reactions can be represented by half-equations, illustrating the oxidation (loss of electrons) at the anode and reduction (gain of electrons) at the cathode, as exemplified by the electrolysis of lead bromide.

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167 episodes

Artwork
iconShare
 
Manage episode 483873400 series 3139602
Content provided by Seneca Learning. All podcast content including episodes, graphics, and podcast descriptions are uploaded and provided directly by Seneca Learning or their podcast platform partner. If you believe someone is using your copyrighted work without your permission, you can follow the process outlined here https://player.fm/legal.

In this episode, we will discuss the electrolysis of aqueous solutions and half equations.

Predicting products during the electrolysis of aqueous solutions is complex due to water's dissociation into hydrogen and hydroxide ions.

At the positive electrode (anode), either halogens form if halide ions are present, or oxygen gas is produced otherwise.

Conversely, at the negative electrode (cathode), hydrogen gas evolves if the metal is more reactive than hydrogen, while the metal itself deposits if it's less reactive.

These electrode reactions can be represented by half-equations, illustrating the oxidation (loss of electrons) at the anode and reduction (gain of electrons) at the cathode, as exemplified by the electrolysis of lead bromide.

Don't miss out on subscribing for more educational content tailored to help you succeed in your exams. Perfect for AQA, OCR, Edexcel, CIE and WJEC exam boards.

⁠Click here to see all of our GCSE Chemistry content!

  continue reading

167 episodes

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