Why you can never change the subscripts in a chemical equation
In short: Mastering chemical equations is about more than just moving numbers around; it is about respecting the fundamental laws of physics. This guide explains how to translate chemical reactions into balanced symbols without violating the conservation of mass.
The core principle behind balancing equations is the law of conservation of mass, which dictates that atoms cannot be created or destroyed in a chemical reaction. Consequently, every type of atom must appear in the same quantity on both the reactant and product sides of an equation.
The video demonstrates how to distinguish between word equations and symbol equations, including the specific representation of diatomic molecules like oxygen (O2). It provides a technical breakdown of the rules: you must use coefficients—the large numbers in front of molecules—to balance the equation, while never altering the subscripts, which define the identity of the substance itself. Practical examples include balancing the combustion of methane and neutralisation reactions.
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Sources
- Summary by Intellect · source: GCSE Chemistry - Balancing Equations | Writing Word & Symbol Equations (2027/28 exams)
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