Chemical reactions are happening all around you every day, from...
Chemistry1,813 views·Updated 28 Aug 2026·36 pagesComplete AQA GCSE Chemistry Paper 2 Revision Notes
Stefany@stef_mvp
1 / 10
1
of 10
Rate of Reaction Basics
Ever wondered why some reactions happen instantly whilst others take ages? The rate of reaction tells you exactly how fast a chemical change occurs. You can measure it by tracking either how quickly products form or how fast reactants disappear over time.
Collision theory explains why reactions happen at all. Particles must crash into each other with enough energy to actually react - this minimum energy needed is called the activation energy. Think of it like trying to break through a brick wall - you need enough force to make it happen.
Most reactions start fast because there are loads of particles bumping into each other. As the reaction continues, fewer reactant particles remain, so collisions become less frequent and the reaction slows down. Eventually, one reactant runs out completely and the reaction stops.
Quick Tip: Remember that particles need both collision AND sufficient energy to react successfully.
2
of 10
Measuring Mass Loss
One clever way to track reaction speed involves watching mass disappear as gas escapes. When calcium carbonate reacts with hydrochloric acid, carbon dioxide gas bubbles away, making the reaction mixture lighter over time.
You'll place the whole setup on a balance and record the mass every few seconds. Cotton wool stops acid from spitting out (safety first!), but still lets gas escape. The faster the mass decreases, the quicker your reaction is happening.
This method works brilliantly because digital balances are incredibly accurate. However, there's one downside - the gas escapes straight into the air around you, which isn't ideal in a classroom setting.
Exam Hint: Always explain that mass decreases because gas escapes, not because matter disappears!
3
of 10
Gas Syringe Method
Gas syringes give you a more precise way to measure reaction rates by directly capturing the gas produced. When magnesium reacts with hydrochloric acid, hydrogen gas pushes the syringe plunger out, showing you exactly how much gas forms.
The method is straightforward: weigh your solid reactant, add it to acid in a flask, then connect the gas syringe and start timing. Record the gas volume every 10 seconds to track the reaction's progress.
Gas syringes beat measuring cylinders for accuracy because they have much better resolution - you can read smaller volume changes. Just watch out for vigorous reactions that might blow the plunger right off!
Safety Note: Always ensure the gas syringe is properly connected before starting the reaction.
4
of 10
Inverted Measuring Cylinder
This classic method uses an upside-down measuring cylinder filled with water to collect gas. As hydrogen bubbles through the delivery tube, it displaces water and you can measure exactly how much gas forms.
The setup needs careful attention to detail. The bung must seal tightly to prevent gas escaping, and the delivery tube shouldn't touch the acid (otherwise acid might travel up the tube). Once everything's connected, wait until bubbling stops completely.
This technique works well for reactions that produce a steady stream of gas. You can repeat the experiment multiple times with the same mass of magnesium to check your results are reliable.
Top Tip: Fill the measuring cylinder completely with water before inverting it - any air bubbles will mess up your measurements.
5
of 10
Disappearing Cross Method
Some reactions create products that change how clearly you can see through a solution. When sodium thiosulfate reacts with hydrochloric acid, solid sulfur forms, making the mixture increasingly cloudy until you can't see through it.
Place a cross under your reaction flask and time how long it takes to disappear completely. This method works perfectly for investigating how concentration affects reaction rate - just change the concentration of sodium thiosulfate whilst keeping everything else constant.
Your control variables include the concentration and volume of hydrochloric acid, plus the volume of sodium thiosulfate solution. The dependent variable is the time taken for the cross to vanish. Want to investigate temperature effects? Just heat your reactants in a water bath first.
Remember: The faster the cross disappears, the quicker the reaction rate!
6
of 10
Factors Affecting Reaction Rate
Five main factors control how fast chemical reactions happen, and understanding them helps you predict and control reaction speeds. Concentration matters because more particles in the same space means more frequent collisions and faster reactions.
Pressure works similarly for gases - squashing gas molecules together increases collision frequency. Surface area is crucial for solid reactants because breaking them into smaller pieces exposes more surface for reactions to occur on.
Temperature has the biggest impact because it makes particles move faster and hit each other harder. More collisions happen, and more of them have enough energy to overcome the activation energy. Catalysts speed things up by providing an alternative pathway with lower activation energy.
Exam Focus: Learn to explain each factor using collision theory - examiners love this connection!
7
of 10
Reversible Reactions and Equilibrium
Some reactions can go both ways - products can turn back into reactants under the right conditions. Dynamic equilibrium occurs when the forward and reverse reactions happen at exactly the same rate in a closed system.
A brilliant example is copper sulfate changing between its hydrated (blue) and anhydrous (white) forms. Heat drives water off (blue to white), whilst adding water reverses this (white to blue). If a reaction is exothermic in one direction, it's always endothermic in the reverse direction.
Ammonium chloride shows this beautifully - heating the white solid produces colourless gases, but cooling makes them recombine into the white solid again. The key is that equilibrium only happens when nothing can escape from your reaction vessel.
Key Point: Dynamic equilibrium means reactions are still happening - they're just balanced perfectly!
8
of 10
Le Chatelier's Principle
Le Chatelier's Principle predicts how equilibrium systems respond to changes - they always try to counteract whatever you do to them. It's like a chemical balancing act that automatically adjusts to maintain stability.
Temperature changes shift equilibrium towards the endothermic direction when heated, or the exothermic direction when cooled. Pressure changes in gas reactions favour the side with fewer molecules when increased, or more molecules when decreased.
Concentration changes trigger the system to use up excess reactants or make more products to restore balance. Interestingly, catalysts don't shift equilibrium position at all - they speed up both forward and reverse reactions equally.
Memory Trick: Think of equilibrium as a stubborn system that always fights back against changes!
9
of 10
Crude Oil and Alkanes
Crude oil formed millions of years ago from ancient plankton buried in mud - it's basically fossilised sea life! This finite resource contains thousands of different hydrocarbons (molecules made only of hydrogen and carbon atoms).
Alkanes are the simplest hydrocarbons with the general formula CnH2n+2. They're saturated because all carbon atoms are connected by single bonds. You need to know methane (CH4), ethane (C2H6), propane (C3H8), and butane (C4H10).
Fractional distillation separates crude oil by heating it until everything evaporates, then cooling different fractions at different temperatures. Heavy molecules condense first (bottom of the column), whilst light molecules rise higher before condensing. This works because different sized molecules have different boiling points.
Quick Fact: Longer hydrocarbon chains are more viscous, less volatile, less flammable, and have higher boiling points!
10
of 10
Hydrocarbon Fuels and Cracking
Different fractions from crude oil become fuels for different purposes - LPG for camping stoves, petrol for cars, diesel for lorries, kerosene for aircraft, and heavy fuel oil for ships. Each fraction has properties perfectly suited to its use.
Combustion of hydrocarbons releases energy that powers our world. Complete combustion produces carbon dioxide and water, but incomplete combustion also creates dangerous carbon monoxide. The equation is simple: hydrocarbon + oxygen → carbon dioxide + water.
Cracking breaks down long, less useful hydrocarbon chains into shorter, more valuable ones. This thermal decomposition reaction uses high temperatures and catalysts (like aluminium oxide) to split large molecules. The products include both alkanes and alkenes, giving us more useful fuels and chemicals.
Industrial Importance: Cracking helps match supply with demand - we need more petrol than crude oil naturally provides!
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Chemistry1,813 views·Updated 28 Aug 2026·36 pagesComplete AQA GCSE Chemistry Paper 2 Revision Notes
Stefany@stef_mvp
Chemical reactions are happening all around you every day, from the fuel in cars to the food you digest. Understanding how fast these reactions happen and what affects their speed is crucial for everything from industrial processes to your GCSE...
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Rate of Reaction Basics
Ever wondered why some reactions happen instantly whilst others take ages? The rate of reaction tells you exactly how fast a chemical change occurs. You can measure it by tracking either how quickly products form or how fast reactants disappear over time.
Collision theory explains why reactions happen at all. Particles must crash into each other with enough energy to actually react - this minimum energy needed is called the activation energy. Think of it like trying to break through a brick wall - you need enough force to make it happen.
Most reactions start fast because there are loads of particles bumping into each other. As the reaction continues, fewer reactant particles remain, so collisions become less frequent and the reaction slows down. Eventually, one reactant runs out completely and the reaction stops.
Quick Tip: Remember that particles need both collision AND sufficient energy to react successfully.
2
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Measuring Mass Loss
One clever way to track reaction speed involves watching mass disappear as gas escapes. When calcium carbonate reacts with hydrochloric acid, carbon dioxide gas bubbles away, making the reaction mixture lighter over time.
You'll place the whole setup on a balance and record the mass every few seconds. Cotton wool stops acid from spitting out (safety first!), but still lets gas escape. The faster the mass decreases, the quicker your reaction is happening.
This method works brilliantly because digital balances are incredibly accurate. However, there's one downside - the gas escapes straight into the air around you, which isn't ideal in a classroom setting.
Exam Hint: Always explain that mass decreases because gas escapes, not because matter disappears!
3
of 10Sign up to see the content. It's free!
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Gas Syringe Method
Gas syringes give you a more precise way to measure reaction rates by directly capturing the gas produced. When magnesium reacts with hydrochloric acid, hydrogen gas pushes the syringe plunger out, showing you exactly how much gas forms.
The method is straightforward: weigh your solid reactant, add it to acid in a flask, then connect the gas syringe and start timing. Record the gas volume every 10 seconds to track the reaction's progress.
Gas syringes beat measuring cylinders for accuracy because they have much better resolution - you can read smaller volume changes. Just watch out for vigorous reactions that might blow the plunger right off!
Safety Note: Always ensure the gas syringe is properly connected before starting the reaction.
4
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Inverted Measuring Cylinder
This classic method uses an upside-down measuring cylinder filled with water to collect gas. As hydrogen bubbles through the delivery tube, it displaces water and you can measure exactly how much gas forms.
The setup needs careful attention to detail. The bung must seal tightly to prevent gas escaping, and the delivery tube shouldn't touch the acid (otherwise acid might travel up the tube). Once everything's connected, wait until bubbling stops completely.
This technique works well for reactions that produce a steady stream of gas. You can repeat the experiment multiple times with the same mass of magnesium to check your results are reliable.
Top Tip: Fill the measuring cylinder completely with water before inverting it - any air bubbles will mess up your measurements.
5
of 10Sign up to see the content. It's free!
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Disappearing Cross Method
Some reactions create products that change how clearly you can see through a solution. When sodium thiosulfate reacts with hydrochloric acid, solid sulfur forms, making the mixture increasingly cloudy until you can't see through it.
Place a cross under your reaction flask and time how long it takes to disappear completely. This method works perfectly for investigating how concentration affects reaction rate - just change the concentration of sodium thiosulfate whilst keeping everything else constant.
Your control variables include the concentration and volume of hydrochloric acid, plus the volume of sodium thiosulfate solution. The dependent variable is the time taken for the cross to vanish. Want to investigate temperature effects? Just heat your reactants in a water bath first.
Remember: The faster the cross disappears, the quicker the reaction rate!
6
of 10Sign up to see the content. It's free!
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Factors Affecting Reaction Rate
Five main factors control how fast chemical reactions happen, and understanding them helps you predict and control reaction speeds. Concentration matters because more particles in the same space means more frequent collisions and faster reactions.
Pressure works similarly for gases - squashing gas molecules together increases collision frequency. Surface area is crucial for solid reactants because breaking them into smaller pieces exposes more surface for reactions to occur on.
Temperature has the biggest impact because it makes particles move faster and hit each other harder. More collisions happen, and more of them have enough energy to overcome the activation energy. Catalysts speed things up by providing an alternative pathway with lower activation energy.
Exam Focus: Learn to explain each factor using collision theory - examiners love this connection!
7
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Reversible Reactions and Equilibrium
Some reactions can go both ways - products can turn back into reactants under the right conditions. Dynamic equilibrium occurs when the forward and reverse reactions happen at exactly the same rate in a closed system.
A brilliant example is copper sulfate changing between its hydrated (blue) and anhydrous (white) forms. Heat drives water off (blue to white), whilst adding water reverses this (white to blue). If a reaction is exothermic in one direction, it's always endothermic in the reverse direction.
Ammonium chloride shows this beautifully - heating the white solid produces colourless gases, but cooling makes them recombine into the white solid again. The key is that equilibrium only happens when nothing can escape from your reaction vessel.
Key Point: Dynamic equilibrium means reactions are still happening - they're just balanced perfectly!
8
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By signing up you accept Terms of Service and Privacy Policy
Le Chatelier's Principle
Le Chatelier's Principle predicts how equilibrium systems respond to changes - they always try to counteract whatever you do to them. It's like a chemical balancing act that automatically adjusts to maintain stability.
Temperature changes shift equilibrium towards the endothermic direction when heated, or the exothermic direction when cooled. Pressure changes in gas reactions favour the side with fewer molecules when increased, or more molecules when decreased.
Concentration changes trigger the system to use up excess reactants or make more products to restore balance. Interestingly, catalysts don't shift equilibrium position at all - they speed up both forward and reverse reactions equally.
Memory Trick: Think of equilibrium as a stubborn system that always fights back against changes!
9
of 10Sign up to see the content. It's free!
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Crude Oil and Alkanes
Crude oil formed millions of years ago from ancient plankton buried in mud - it's basically fossilised sea life! This finite resource contains thousands of different hydrocarbons (molecules made only of hydrogen and carbon atoms).
Alkanes are the simplest hydrocarbons with the general formula CnH2n+2. They're saturated because all carbon atoms are connected by single bonds. You need to know methane (CH4), ethane (C2H6), propane (C3H8), and butane (C4H10).
Fractional distillation separates crude oil by heating it until everything evaporates, then cooling different fractions at different temperatures. Heavy molecules condense first (bottom of the column), whilst light molecules rise higher before condensing. This works because different sized molecules have different boiling points.
Quick Fact: Longer hydrocarbon chains are more viscous, less volatile, less flammable, and have higher boiling points!
10
of 10Sign up to see the content. It's free!
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Hydrocarbon Fuels and Cracking
Different fractions from crude oil become fuels for different purposes - LPG for camping stoves, petrol for cars, diesel for lorries, kerosene for aircraft, and heavy fuel oil for ships. Each fraction has properties perfectly suited to its use.
Combustion of hydrocarbons releases energy that powers our world. Complete combustion produces carbon dioxide and water, but incomplete combustion also creates dangerous carbon monoxide. The equation is simple: hydrocarbon + oxygen → carbon dioxide + water.
Cracking breaks down long, less useful hydrocarbon chains into shorter, more valuable ones. This thermal decomposition reaction uses high temperatures and catalysts (like aluminium oxide) to split large molecules. The products include both alkanes and alkenes, giving us more useful fuels and chemicals.
Industrial Importance: Cracking helps match supply with demand - we need more petrol than crude oil naturally provides!
We thought you’d never ask...
Our AI Companion is a student-focused AI tool that offers more than just answers. Built on millions of Knowunity resources, it provides relevant information, personalised study plans, quizzes, and content directly in the chat, adapting to your individual learning journey.
You can download the app from Google Play Store and Apple App Store.
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