Many students in my weekly JC1 GCE A-Level H2 Chemistry Tuition Classes in Singapore told me that they are struggling to understand the concepts regarding Redox Reactions. This is usually taught in JC1 Topic 1: Mole Concepts & Stoichiometry in their Junior College’s lectures and tutorial classes. They seems lost and don’t even know how to start when looking at a Redox Reactions question.

Many of them have approached their JC teacher or recommended H2 Chemistry tutor but still not able to solve redox reactions question confidently.

So, before you work on another Redox Reactions question, do go through the following:

**4 steps on How to Solve Redox Reactions**

**1. Describe and explain redox processes in terms of electron transfer and/or of changes in oxidation number (oxidation state)**

Reduction and Oxidation processes may be defined in terms of electron transfer and/or changes in oxidation number (oxidation state).

- Reduction: A process whereby a substance gains electrons, resulting in a decrease in oxidation number
- Oxidation: A process whereby a substance loses electrons. resulting in an increase in oxidation number
- Reducing Agent (Reductant): A substance that gives electrons to another, itself being oxidised in the process
- Oxidising Agent (Oxidant): A substance that takes in electrons from another, itself being reduced in the process

Next, you would need to understand that in a redox reaction, there is a transfer of electrons from the reducing agent (who loses electrons and is being oxidised) to the oxidising agent (who gains electrons and is being reduced).

**2. Construct redox equations using the relevant half-equations**

For most examination questions, the full redox equation is not given directly in the question. So, students would need to be able to come out with it. This is only possible if you are able to work out the half-equations (both the oxidation half and the reduction half) on your own.

From there, you would need to combine the oxidation half equation and the reduction half equation to form the full redox equation. Do note that half equations will always contain electrons in it while full redox equations will not have any electrons since they have been cancelled out.

I have blogged about these previously and if you have missed out on these earlier videos, you can watch them via the links below:

- 10 Steps Strategy to Balance Redox Equations in Acidic Medium
- 13 Steps Strategy to Balance Redox Equations in Alkaline Medium

**3. Perform calculations, using the mole concepts, involving redox reactions**

What you have learned previously in *Mole Concepts* or *Mole Calculations* will come into good use here. You will usually be required to calculate terms involving *Mole*, *Volume* and *Molar Concentration*.

You must also be aware that the * number of moles of electrons lost by the reducing agent must be equal to the number of electrons gained by the oxidising agent*.

In another word, to solve such questions, you need to determine the * mole of electrons that are being transferred*.

**4. Deduce stoichiometric relationships from calculations such as those in (3) above**

From there, you will have to * deduce the stoichiometric relationships* to solve the question using the balanced equation.

Click on the following link below to see how i apply the 4 steps to solve a Redox Reaction. Enjoy watching!

4 Steps to Solve Redox Reactions in JC A-Level H2 Chemistry

Length of video: 5.35 minutes

I hope you find the content easy for your understanding and if you have any questions, leave me a comment below. Feel free to share this blog post with your friends and learn proper Chemistry Concepts together.

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### Related Articles:

- 10 Steps Strategy to Balance Redox Equations in Acidic Medium Video
- 13 Steps Strategy to Balance Redox Equations in Alkaline Medium Video
- Mole Calculation Question in Atoms, Molecules & Stoichiometry
- Organic Chemistry: Determining the Oxidation State (Number) of Carbon in Organic Compounds
- Chemical Energetics: Definitions of Standard Enthalpy Changes of Reactions

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