Chemical reactions either release energy to the surroundings (exothermic) or...
Chemistry108 views·Updated 19 Aug 2026·8 pagesAQA Chemistry Higher Energy Changes Notes - Triple Science C4
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1 / 8
1
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Energy Changes in Chemical Reactions
Ever wondered why some reactions make things hot whilst others make them cold? Exothermic reactions transfer energy from the reacting molecules to the surroundings, making the temperature increase. Think of burning wood - it releases loads of energy as heat and light.
You'll also see exothermic reactions in oxidation reactions and neutralisation (when acids and alkalis react). These reactions are dead useful in real life - hand warmers and self-heating food cans both use exothermic reactions to generate heat on demand.
Energy profile diagrams show how energy changes during a reaction. For exothermic reactions, the products have less energy than the reactants because energy has been transferred out to the surroundings. The difference between reactant and product energy levels tells you exactly how much energy was released.
💡 Quick Tip: In exams, you might need to label energy profile diagrams showing the energy change - remember that exothermic reactions slope downwards from reactants to products.
2
of 8
Endothermic Reactions and Energy Profiles
Endothermic reactions do the opposite - they take in energy from the surroundings, making the temperature decrease. Thermal decomposition is a classic example where compounds break down when heated, absorbing energy in the process.
On energy profile diagrams for endothermic reactions, the products sit higher than the reactants because energy has been absorbed from the surroundings. The difference between these energy levels shows how much energy the reaction took in.
Both reaction types still need to get over the same hurdle though - they rise to a peak before dropping (or rising) to the products. This peak represents the activation energy, which we'll explore more in the next section.
💡 Memory Trick: Endothermic = Energy IN (temperature drops), Exothermic = Energy EXits (temperature rises).
3
of 8
Activation Energy - The Energy Barrier
Here's something crucial: reactions can only happen when particles collide with enough energy. Activation energy is the minimum amount of energy particles need to react when they smash into each other.
Both exothermic and endothermic reactions have activation energy - it's the energy barrier they must overcome to get started. On energy profile diagrams, activation energy is measured from the reactants up to the peak of the curve.
Think of it like pushing a boulder over a hill - you need enough energy to get it to the top (activation energy) before it can roll down the other side (the reaction happens). Without sufficient activation energy, particles just bounce off each other without reacting.
💡 Exam Alert: You might be asked to mark activation energy on energy profile diagrams - it's always from reactants to the peak, regardless of whether the reaction is exothermic or endothermic.
4
of 8
Energy Change Values and Diagrams
When chemists write about energy changes, they use positive and negative values to show the direction of energy transfer. Exothermic reactions show negative energy changes because energy transfers out from the chemicals to the surroundings.
Endothermic reactions show positive energy changes because energy has been gained from the surroundings. This sign convention helps you quickly identify reaction types from data.
In exam questions, you'll often see energy profile diagrams with labels like A (progress of reaction), B (activation energy), and C (products). Make sure you can identify these key features and explain what each part represents.
💡 Sign Success: Negative = energy leaves (exothermic), Positive = energy enters (endothermic).
5
of 8
Bond Breaking and Bond Making
Every chemical reaction involves breaking existing bonds (which requires energy) and making new bonds (which releases energy). Breaking bonds is always endothermic, whilst making bonds is always exothermic.
Each type of chemical bond has a specific bond energy value - this tells you exactly how much energy is needed to break that bond. For example, breaking an H-H bond requires +436 kJ, whilst making an H-Cl bond releases -431 kJ.
To work out if a reaction is overall exothermic or endothermic, you calculate the total energy needed to break bonds, then subtract the total energy released when making new bonds. If the answer is negative, the reaction is exothermic; if positive, it's endothermic.
💡 Calculation Tip: Energy required to break bonds - Energy released making bonds = Overall energy change. Negative result = exothermic reaction.
6
of 8
RP4: Investigating Temperature Changes
Required Practical 4 investigates temperature changes in the exothermic neutralisation reaction between hydrochloric acid and sodium hydroxide. You'll add increasing volumes of alkali to acid and measure the maximum temperature reached.
The method involves measuring 30cm³ of hydrochloric acid in a polystyrene cup, then adding 5cm³ of sodium hydroxide solution. Use a thermometer to stir and measure the highest temperature reached after the reaction.
You'll repeat this experiment increasing the sodium hydroxide volume by 5cm³ each time up to 40cm³. The polystyrene cup and plastic lid are crucial because polystyrene is a good thermal insulator that reduces heat loss, giving more accurate temperature measurements.
💡 Safety First: Always wear safety goggles when working with acids and alkalis, and handle glassware carefully to avoid spills.
7
of 8
RP4: Results and Graph Analysis
When you plot your results, you'll see the maximum temperature initially increases as you add more sodium hydroxide. This happens because more particles are available to react with the hydrochloric acid, releasing more energy in this exothermic reaction.
However, the temperature reaches a peak then starts decreasing. This occurs because there's now so much sodium hydroxide that there isn't enough hydrochloric acid left to react with it all - you've reached the limiting reactant situation.
The temperature actually drops after this point because you're adding greater volumes of solution, so the same amount of energy released gets spread out over a larger volume. This dilution effect reduces the temperature rise you can measure.
💡 Graph Pattern: Temperature rises to a peak (complete neutralisation), then falls due to dilution - this creates a characteristic mountain shape.
8
of 8
RP4: Equipment Choices and Heat Loss
The polystyrene cup with plastic lid isn't just random equipment choice - it's specifically designed to minimise heat loss during your temperature measurements. Polystyrene acts as a thermal insulator, reducing heat loss through the sides and bottom of the container.
The plastic lid prevents heat escaping to the air above the reaction mixture. Without these precautions, you'd lose heat to the surroundings and get inaccurate, lower temperature readings.
This practical demonstrates how important it is to consider heat transfer when measuring energy changes in reactions. Any heat lost to the surroundings won't be detected by your thermometer, leading to underestimated energy changes.
💡 Exam Favourite: Questions often ask why we use polystyrene cups and lids - always mention thermal insulation and reducing heat loss for accurate measurements.
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Chemistry108 views·Updated 19 Aug 2026·8 pagesAQA Chemistry Higher Energy Changes Notes - Triple Science C4
🎀 𝒈𝒓𝒂𝒄𝒆 🎀@grace.xxcharlotte08
Chemical reactions either release energy to the surroundings (exothermic) or absorb energy from them (endothermic). Understanding these energy changes is crucial for predicting how reactions behave and helps explain everything from hand warmers to why certain reactions need heating to...
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Energy Changes in Chemical Reactions
Ever wondered why some reactions make things hot whilst others make them cold? Exothermic reactions transfer energy from the reacting molecules to the surroundings, making the temperature increase. Think of burning wood - it releases loads of energy as heat and light.
You'll also see exothermic reactions in oxidation reactions and neutralisation (when acids and alkalis react). These reactions are dead useful in real life - hand warmers and self-heating food cans both use exothermic reactions to generate heat on demand.
Energy profile diagrams show how energy changes during a reaction. For exothermic reactions, the products have less energy than the reactants because energy has been transferred out to the surroundings. The difference between reactant and product energy levels tells you exactly how much energy was released.
💡 Quick Tip: In exams, you might need to label energy profile diagrams showing the energy change - remember that exothermic reactions slope downwards from reactants to products.
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Endothermic Reactions and Energy Profiles
Endothermic reactions do the opposite - they take in energy from the surroundings, making the temperature decrease. Thermal decomposition is a classic example where compounds break down when heated, absorbing energy in the process.
On energy profile diagrams for endothermic reactions, the products sit higher than the reactants because energy has been absorbed from the surroundings. The difference between these energy levels shows how much energy the reaction took in.
Both reaction types still need to get over the same hurdle though - they rise to a peak before dropping (or rising) to the products. This peak represents the activation energy, which we'll explore more in the next section.
💡 Memory Trick: Endothermic = Energy IN (temperature drops), Exothermic = Energy EXits (temperature rises).
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Activation Energy - The Energy Barrier
Here's something crucial: reactions can only happen when particles collide with enough energy. Activation energy is the minimum amount of energy particles need to react when they smash into each other.
Both exothermic and endothermic reactions have activation energy - it's the energy barrier they must overcome to get started. On energy profile diagrams, activation energy is measured from the reactants up to the peak of the curve.
Think of it like pushing a boulder over a hill - you need enough energy to get it to the top (activation energy) before it can roll down the other side (the reaction happens). Without sufficient activation energy, particles just bounce off each other without reacting.
💡 Exam Alert: You might be asked to mark activation energy on energy profile diagrams - it's always from reactants to the peak, regardless of whether the reaction is exothermic or endothermic.
4
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Energy Change Values and Diagrams
When chemists write about energy changes, they use positive and negative values to show the direction of energy transfer. Exothermic reactions show negative energy changes because energy transfers out from the chemicals to the surroundings.
Endothermic reactions show positive energy changes because energy has been gained from the surroundings. This sign convention helps you quickly identify reaction types from data.
In exam questions, you'll often see energy profile diagrams with labels like A (progress of reaction), B (activation energy), and C (products). Make sure you can identify these key features and explain what each part represents.
💡 Sign Success: Negative = energy leaves (exothermic), Positive = energy enters (endothermic).
5
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Bond Breaking and Bond Making
Every chemical reaction involves breaking existing bonds (which requires energy) and making new bonds (which releases energy). Breaking bonds is always endothermic, whilst making bonds is always exothermic.
Each type of chemical bond has a specific bond energy value - this tells you exactly how much energy is needed to break that bond. For example, breaking an H-H bond requires +436 kJ, whilst making an H-Cl bond releases -431 kJ.
To work out if a reaction is overall exothermic or endothermic, you calculate the total energy needed to break bonds, then subtract the total energy released when making new bonds. If the answer is negative, the reaction is exothermic; if positive, it's endothermic.
💡 Calculation Tip: Energy required to break bonds - Energy released making bonds = Overall energy change. Negative result = exothermic reaction.
6
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RP4: Investigating Temperature Changes
Required Practical 4 investigates temperature changes in the exothermic neutralisation reaction between hydrochloric acid and sodium hydroxide. You'll add increasing volumes of alkali to acid and measure the maximum temperature reached.
The method involves measuring 30cm³ of hydrochloric acid in a polystyrene cup, then adding 5cm³ of sodium hydroxide solution. Use a thermometer to stir and measure the highest temperature reached after the reaction.
You'll repeat this experiment increasing the sodium hydroxide volume by 5cm³ each time up to 40cm³. The polystyrene cup and plastic lid are crucial because polystyrene is a good thermal insulator that reduces heat loss, giving more accurate temperature measurements.
💡 Safety First: Always wear safety goggles when working with acids and alkalis, and handle glassware carefully to avoid spills.
7
of 8Sign up to see the content. It's free!
- Access to all documents
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By signing up you accept Terms of Service and Privacy Policy
RP4: Results and Graph Analysis
When you plot your results, you'll see the maximum temperature initially increases as you add more sodium hydroxide. This happens because more particles are available to react with the hydrochloric acid, releasing more energy in this exothermic reaction.
However, the temperature reaches a peak then starts decreasing. This occurs because there's now so much sodium hydroxide that there isn't enough hydrochloric acid left to react with it all - you've reached the limiting reactant situation.
The temperature actually drops after this point because you're adding greater volumes of solution, so the same amount of energy released gets spread out over a larger volume. This dilution effect reduces the temperature rise you can measure.
💡 Graph Pattern: Temperature rises to a peak (complete neutralisation), then falls due to dilution - this creates a characteristic mountain shape.
8
of 8Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
By signing up you accept Terms of Service and Privacy Policy
RP4: Equipment Choices and Heat Loss
The polystyrene cup with plastic lid isn't just random equipment choice - it's specifically designed to minimise heat loss during your temperature measurements. Polystyrene acts as a thermal insulator, reducing heat loss through the sides and bottom of the container.
The plastic lid prevents heat escaping to the air above the reaction mixture. Without these precautions, you'd lose heat to the surroundings and get inaccurate, lower temperature readings.
This practical demonstrates how important it is to consider heat transfer when measuring energy changes in reactions. Any heat lost to the surroundings won't be detected by your thermometer, leading to underestimated energy changes.
💡 Exam Favourite: Questions often ask why we use polystyrene cups and lids - always mention thermal insulation and reducing heat loss for accurate measurements.
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.
That's right! Enjoy free access to study content, connect with fellow students, and get instant help – all at your fingertips.
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