Chemical kinetics is all about understanding how fast reactions happen...
Chemistry44 views·Updated 5 Sept 2026·2 pagesOCR A Level Chemistry: Rates Topic Mind Map
Angelin saji@angelinsaji_urux
1
of 2
Measuring Reaction Rates and Orders
Ever wondered why some reactions happen instantly whilst others take ages? Rate experiments help us figure out exactly how concentration affects reaction speed. You'll use techniques like colorimetry to track how reactant concentrations change over time.
The initial rates method is your go-to technique for determining reaction orders. You run several experiments, changing one reactant's concentration each time whilst keeping others constant. Then you measure how fast the reaction starts - that's your initial rate.
Reaction order tells you how concentration affects rate. If doubling a reactant's concentration doubles the rate, it's first order. If it quadruples the rate, it's second order. The overall rate equation looks like: Rate = k[A]^m[B]^n, where m and n are the individual orders.
Quick Tip: Always use a tangent to the curve at time zero to find your initial rate - it's the most accurate method!
2
of 2
The Arrhenius Equation and Temperature Effects
Temperature is absolutely crucial in chemical reactions - even small increases can dramatically speed things up. The Arrhenius equation explains this perfectly: k = Ae^(-Ea/RT), where k is the rate constant and Ea is the activation energy.
Think of activation energy as the energy barrier molecules need to overcome before they can react. Higher temperatures give more molecules enough energy to clear this barrier, so more successful collisions happen per second.
The Arrhenius plot is brilliant for finding activation energy experimentally. You plot ln against 1/T to get a straight line with gradient -Ea/R. This means you can calculate exactly how much energy your reaction needs to get started.
Remember: A steeper Arrhenius plot means higher activation energy - your reaction is more sensitive to temperature changes!
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Chemistry44 views·Updated 5 Sept 2026·2 pagesOCR A Level Chemistry: Rates Topic Mind Map
Angelin saji@angelinsaji_urux
Chemical kinetics is all about understanding how fast reactions happen and what affects their speed. You'll learn to measure reaction rates, work out reaction orders, and discover how temperature dramatically influences chemical processes through the Arrhenius equation.
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Measuring Reaction Rates and Orders
Ever wondered why some reactions happen instantly whilst others take ages? Rate experiments help us figure out exactly how concentration affects reaction speed. You'll use techniques like colorimetry to track how reactant concentrations change over time.
The initial rates method is your go-to technique for determining reaction orders. You run several experiments, changing one reactant's concentration each time whilst keeping others constant. Then you measure how fast the reaction starts - that's your initial rate.
Reaction order tells you how concentration affects rate. If doubling a reactant's concentration doubles the rate, it's first order. If it quadruples the rate, it's second order. The overall rate equation looks like: Rate = k[A]^m[B]^n, where m and n are the individual orders.
Quick Tip: Always use a tangent to the curve at time zero to find your initial rate - it's the most accurate method!
2
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The Arrhenius Equation and Temperature Effects
Temperature is absolutely crucial in chemical reactions - even small increases can dramatically speed things up. The Arrhenius equation explains this perfectly: k = Ae^(-Ea/RT), where k is the rate constant and Ea is the activation energy.
Think of activation energy as the energy barrier molecules need to overcome before they can react. Higher temperatures give more molecules enough energy to clear this barrier, so more successful collisions happen per second.
The Arrhenius plot is brilliant for finding activation energy experimentally. You plot ln against 1/T to get a straight line with gradient -Ea/R. This means you can calculate exactly how much energy your reaction needs to get started.
Remember: A steeper Arrhenius plot means higher activation energy - your reaction is more sensitive to temperature changes!
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