Measuring and Controlling Reaction Rates
Understanding reaction rates is like being a chemical detective - you're measuring how quickly reactants disappear or products appear. The maths is straightforward: rate equals the quantity of substance divided by time, giving you units like g/s or cm³/s.
There are three main ways to track reactions in the lab. You can measure decreasing mass (like when gas escapes), increasing gas volume, or decreasing light passing through a solution (the classic disappearing cross experiment). Each method gives you real data about how fast your reaction is proceeding.
The secret behind all reactions lies in particle collisions. Think of it like a game of molecular snooker - particles must crash into each other with enough energy (called activation energy) to actually react. Without enough energy, they just bounce off each other uselessly.
Five key factors control how fast reactions happen: temperature, concentration, pressure (for gases), surface area, and catalysts. Master these, and you can predict and control virtually any chemical reaction.
Quick Check: Remember that smaller pieces of solid reactants mean larger surface area, which means more collisions and faster reactions!
Catalysts are absolute game-changers in chemistry. They speed up reactions without getting used up themselves, often by lowering the activation energy barrier. Industries love them because they save time, money, and energy - platinum in car exhausts and iron in ammonia production are perfect examples.