C6 notes

Rate of Reaction

Describes how rapidly the reactants are consumed or the product is formed.

Collision Theory

Explains why different reactions occur at different rates and suggests ways to change the rate of a reaction.

Successful Collisions

Collisions between particles that have enough energy to break bonds and result in a reaction.

Activation Energy

The minimum amount of energy required for particles to collide and react.

Kinetic Energy and Rate of Reaction

Higher kinetic energy of particles leads to more frequent collisions with sufficient energy, increasing the rate of reaction.

Temperature and Rate of Reaction

Increasing temperature increases the kinetic energy of particles, resulting in more frequent and harder collisions.

Concentration and Rate of Reaction

Higher concentration increases the number of reactant particles in a given volume, leading to more successful collisions.

Surface Area to Volume Ratio

Higher surface area to volume ratio in solids increases the rate of reaction by facilitating more frequent collisions.

Effect of Pressure on Gases

Increasing pressure increases the number of gas particles in a volume, leading to more frequent successful collisions.

Catalyst

Substances that speed up the rate of reaction without being chemically altered or used up in the process.

Enzymes

Biological catalysts made from proteins that can function at lower temperatures.

Core Practical: Gas Measurement

Investigates the effects of changing conditions on reaction rates by measuring the production of gas.

Core Practical Equation

CaCO3 + 2HCl → CaCl2 + H2O + CO2, measuring the volume of CO2 produced over time.

Core Practical: Color Change

Measures how long it takes for a solution's color to change, indicating the rate of reaction.

Rate Graphs

Graphs that plot product/reactant against time to measure the rate of reactions.

Gradient of Rate Graph

The steepness of the line on a rate graph indicates the speed of the reaction; steeper lines signify faster rates.