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Rates in Chemical Reactions - Coggle Diagram
Rates in Chemical Reactions
Concentration
Higher concentration = faster reaction rate – because there are more reactant particles in the same volume, leading to more frequent collisions.
More collisions = more chances for reactions – increased particle interactions raise the likelihood of successful collisions with enough energy to react.
Lower concentration = slower rate – fewer particles mean collisions happen less often.
Surface Area
Larger surface area = faster reaction – because more of the solid is exposed to react.
More exposed particles = more collisions – increasing the chances of successful reactions.
Smaller surface area = slower reaction – fewer particles are available to collide.
Surface area matters for solids – it doesn’t affect gases or liquids the same way.
Powdered solids react faster than chunks – this is a practical example of surface area affecting rate.
Catalyst
Catalysts make reactions faster – they help particles react more easily.
They work by lowering the activation energy – less energy is needed for collisions to succeed.
Catalysts are not used up – they can be used again and again.
They don’t change the amount of product – just how fast it is made.
Temperature
Higher temperature = faster reaction – particles move faster and collide more often.
Faster particles = more energetic collisions – making reactions more likely to happen.
Lower temperature = slower reaction – particles move slower and collide less often.
More collisions + more energy = faster reaction – that’s why heat speeds things up.
Temperature affects almost all reactions – hot conditions usually make reactions quicker, cold slows them down.