Why chemical reactions don't always reach a final destination
In short: Most people think reactions go from start to finish, but many are actually two-way streets. This video explains how chemicals can move back and forth simultaneously until they reach a state of perfect balance.
The core concept is dynamic equilibrium: a state where the forward and backward reaction rates become exactly equal. Because these reactions happen at the same speed, the concentrations of reactants and products stay constant over time. However, this balance requires a closed system to ensure no substances can enter or leave.
The video also explores 'position,' which describes whether equilibrium favors the reactants (left) or products (right). It covers how external factors like temperature can shift this position. For instance, if a forward reaction is endothermic, its reverse must be exothermic, meaning heat plays a critical role in determining where the balance sits.
Opens the Intellect+ feed with this card first. Swipe up for the next one.
Sources
- Summary by Intellect · source: GCSE Chemistry - Reversible Reactions & Dynamic Equilibrium (2027/28 exams)
To cite this card, link to https://intellectplus.co.uk/app/science-gcse-chemistry-reversible-reactions-dynamic-equilibrium-2027.
How we source, check and correct cards: Editorial standards.
General information, not professional advice. Spotted an error? Flag the card or see corrections and complaints.
Intellect Plus is a visual educational discovery platform for exploring fascinating facts and ideas. Brain Food, Not Brain Rot. What is Intellect Plus?
Related
More in Chemistry · More in Science · Latest · A–Z · All topics
