IGCSE 11.1.1
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Exothermic reactions release energy as heat to the surroundings and can occur spontaneously or explosively. Examples include combustion, respiration, and reactions of metals with acids. Endothermic reactions absorb energy from the surroundings and cause cooling. Reversible reactions are exothermic in one direction as they release heat, but are endothermic in the reverse direction as they absorb the same amount of heat.
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Displacement reaction
this is a ppt made bby Hima Mohammed
well, made this when I was in 7th grade.
subject : chemistry
hope you ll like it
enjoy..
good luck
let me know wat d u think about this powerpoint presntation
SINGLE DISPLACEMENT REACTION
A single displacement reaction occurs when a more reactive element replaces a less reactive element in a compound. To determine if a single displacement reaction will occur, one checks the activity series to see if the replacing element is more reactive than the element being replaced. If so, the products of the reaction are determined by distributing the elements between the reactants and products. The overall balanced chemical equation is obtained by combining the distributed elements.
IGCSE 11.1.5
The document discusses endothermic reactions. It states that endothermic reactions absorb thermal energy, causing a decrease in temperature. Examples of endothermic reactions given include thermal decomposition of calcium carbonate in a blast furnace, photosynthesis, some types of electrolysis, and the melting of sherbet.
Energy and change
This document discusses endothermic and exothermic reactions. Endothermic reactions absorb energy from their surroundings in the form of heat. Examples include melting ice and dissolving salts in water. Exothermic reactions release energy, usually as heat, warming their surroundings. Examples are combustion reactions and the neutralization of acids and bases. The heat of reaction, ΔH, indicates whether a reaction is endothermic (ΔH positive) or exothermic (ΔH negative). Bond breaking requires energy while bond formation releases energy.
Enthalpy Change
The document discusses enthalpy changes and exothermic and endothermic reactions. It defines exothermic reactions as reactions where heat energy is released to the surroundings, giving a negative enthalpy change. Endothermic reactions absorb heat from the surroundings, having a positive enthalpy change. Bond breaking requires energy and is endothermic, while bond forming releases energy and is exothermic. Whether a reaction is exothermic or endothermic depends on if more energy is released or absorbed during bond breaking and forming.
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The document discusses enthalpy changes and exothermic and endothermic reactions. It defines exothermic reactions as reactions where heat energy is given out to the surroundings, while endothermic reactions absorb heat from the surroundings. Whether a reaction is exothermic or endothermic depends on whether more energy is released or absorbed during bond breaking and forming. The enthalpy change, ∆H, is negative for exothermic reactions and positive for endothermic reactions. Examples of each type of reaction are provided.
Enthalpy change
This document summarizes different types of enthalpy changes in chemical reactions. It defines exothermic reactions as releasing energy to the surroundings and endothermic reactions as absorbing energy from the surroundings. Enthalpy change is the energy exchange between a reaction and its surroundings at constant pressure. The document explains how to calculate enthalpy change and represents reaction pathways using enthalpy profile diagrams to show enthalpy changes for exothermic and endothermic reactions. It also defines standard enthalpy changes of combustion, neutralization, solution, and hydration of salts.
Decomposition reaction
This document discusses decomposition reactions, where a single compound breaks down into simpler substances. Examples given include lead nitrate decomposing into lead oxide, oxygen, and nitrogen dioxide when heated. Blue copper sulfate pentahydrate also decomposes when heated, forming white copper sulfate and water vapor. Electrolysis and exposure to sunlight are provided as other means for decomposition reactions to occur, such as water decomposing into hydrogen and oxygen during electrolysis or silver chloride decomposing into silver and chlorine in the presence of light.
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Displacement reaction
this is a ppt made bby Hima Mohammed
well, made this when I was in 7th grade.
subject : chemistry
hope you ll like it
enjoy..
good luck
let me know wat d u think about this powerpoint presntation
SINGLE DISPLACEMENT REACTION
A single displacement reaction occurs when a more reactive element replaces a less reactive element in a compound. To determine if a single displacement reaction will occur, one checks the activity series to see if the replacing element is more reactive than the element being replaced. If so, the products of the reaction are determined by distributing the elements between the reactants and products. The overall balanced chemical equation is obtained by combining the distributed elements.
IGCSE 11.1.5
The document discusses endothermic reactions. It states that endothermic reactions absorb thermal energy, causing a decrease in temperature. Examples of endothermic reactions given include thermal decomposition of calcium carbonate in a blast furnace, photosynthesis, some types of electrolysis, and the melting of sherbet.
Energy and change
This document discusses endothermic and exothermic reactions. Endothermic reactions absorb energy from their surroundings in the form of heat. Examples include melting ice and dissolving salts in water. Exothermic reactions release energy, usually as heat, warming their surroundings. Examples are combustion reactions and the neutralization of acids and bases. The heat of reaction, ΔH, indicates whether a reaction is endothermic (ΔH positive) or exothermic (ΔH negative). Bond breaking requires energy while bond formation releases energy.
Enthalpy Change
The document discusses enthalpy changes and exothermic and endothermic reactions. It defines exothermic reactions as reactions where heat energy is released to the surroundings, giving a negative enthalpy change. Endothermic reactions absorb heat from the surroundings, having a positive enthalpy change. Bond breaking requires energy and is endothermic, while bond forming releases energy and is exothermic. Whether a reaction is exothermic or endothermic depends on if more energy is released or absorbed during bond breaking and forming.
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This document summarizes different types of enthalpy changes in chemical reactions. It defines exothermic reactions as releasing energy to the surroundings and endothermic reactions as absorbing energy from the surroundings. Enthalpy change is the energy exchange between a reaction and its surroundings at constant pressure. The document explains how to calculate enthalpy change and represents reaction pathways using enthalpy profile diagrams to show enthalpy changes for exothermic and endothermic reactions. It also defines standard enthalpy changes of combustion, neutralization, solution, and hydration of salts.
Decomposition reaction
This document discusses decomposition reactions, where a single compound breaks down into simpler substances. Examples given include lead nitrate decomposing into lead oxide, oxygen, and nitrogen dioxide when heated. Blue copper sulfate pentahydrate also decomposes when heated, forming white copper sulfate and water vapor. Electrolysis and exposure to sunlight are provided as other means for decomposition reactions to occur, such as water decomposing into hydrogen and oxygen during electrolysis or silver chloride decomposing into silver and chlorine in the presence of light.
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Decomposition reactions occur when a compound breaks down into simpler substances like elements or other compounds. There are three main types of decomposition reactions: thermal decomposition caused by heat, photo decomposition caused by light, and electric decomposition caused by an electric current. An example of a decomposition reaction is when water breaks down into hydrogen and oxygen gases.
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1) Displacement reactions can be classified as metal-metal displacement reactions or metal-nonmetal displacement reactions.
2) In metal-metal displacement reactions, more reactive metals displace less reactive metals according to the reactivity series. For example, copper displaces iron when an iron bar is placed in copper sulfate solution.
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This document provides information on chemical reactions and equations. It defines a chemical reaction as a process that transforms one set of substances into another. It explains the different types of chemical equations like word equations, skeletal equations, and balanced equations. It also describes the different types of chemical reactions such as combination, decomposition, displacement, and redox reactions. It discusses oxidation and reduction processes and defines oxidizing and reducing agents. Examples of chemical equations are also provided.
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Chemical reactions can be either exothermic or endothermic. Exothermic reactions release energy in the form of heat, causing a temperature increase. Endothermic reactions absorb energy from their surroundings in the form of heat, causing a temperature decrease. Examples of exothermic reactions given are the neutralization of an acid with a base and burning magnesium, while examples of endothermic reactions include the thermal decomposition of limestone and dissolving salts in water. The energy changes in chemical reactions can be explained by considering the energy required to break bonds in reactants versus the energy released when new bonds form in products.
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The circuit for a door bell contains an electromagnet that pulls an armature towards it when the circuit is closed, causing a hammer to strike the bell and produce sound. The movement of the armature then breaks the circuit, allowing the hammer to return to its original position, and this sequence repeats to make the bell ring continuously whenever the door bell button is pressed.
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An electromagnet on a recycling plant conveyor belt is used to pick up and move metal cans. Electromagnets attract ferromagnetic metals like iron, nickel, and cobalt. Electromagnets have the advantage over permanent magnets in that their magnetic field can be switched on and off by controlling the electric current running through the magnet coils.
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The document presents results from an experiment investigating electromagnets. It shows that increasing the number of coils or the current in an electromagnet increases the number of drawing pins attracted. Graphs illustrate the direct relationship between the number of coils/current and the number of drawing pins attracted.
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Increasing the concentration of a substance in a reversible reaction shifts the equilibrium to decrease the concentration of that substance. For example, adding more water to a reaction producing bismuth oxychloride and hydrochloric acid from bismuth chloride and water would shift the equilibrium right, producing more products. Similarly, adding more chlorine gas to a reaction producing iodine trichloride from chlorine and iodine chloride would make the mixture appear more yellow by shifting the equilibrium to the right.
2
The document discusses exothermic and endothermic reactions. It states that all reactions are exothermic in one direction, releasing heat, and endothermic in the other direction, absorbing heat. It also explains that if temperature is increased, the equilibrium will shift in the endothermic direction to decrease temperature, and if temperature is decreased, the equilibrium will shift in the exothermic direction to increase temperature. It provides the example of nitrogen dioxide and dinitrogen tetroxide, where the forward reaction is exothermic and the backward reaction is endothermic. If temperature is increased in this system, more nitrogen dioxide will be produced.
5
Catalysts speed up chemical reactions by lowering the activation energy of the reaction pathway, without being used up in the process. When added to a reversible reaction, a catalyst increases the rates of both the forward and reverse reactions equally, resulting in no change to the equilibrium position but equilibrium being reached faster. Catalysts are particularly important in industrial applications as they allow reactions to proceed more quickly.
6
Ammonia is produced industrially through the Haber process, which involves reacting nitrogen and hydrogen at high pressures and temperatures. However, the reaction is reversible and does not go to completion. To maximize yield while keeping costs low, manufacturers use a compromise of 450°C and 200 atmospheres, as extremely high pressures require expensive equipment and low temperatures slow the reaction rate. Key costs in ammonia production include raw materials, energy, equipment, wages. Yield is maximized by using a catalyst, removing ammonia as it forms, and recycling unreacted gases.
1
Le Chatelier's principle states that if a system in dynamic equilibrium experiences a change, the equilibrium will shift to counteract the change. Specifically, increasing temperature shifts equilibrium towards the endothermic direction, increasing concentration shifts equilibrium away from that substance, and increasing pressure shifts equilibrium away from the gas producing side.
IB 3.2.2.5
The melting points of elements in group 1 decrease down the group because the atomic radius increases, resulting in weaker metallic bonds and a weaker attraction between the nucleus and delocalized electrons. The melting points given for lithium, sodium, potassium, rubidium, and cesium show this decreasing trend.
IB 3.2.2.4
Electronegativity decreases down a group because the atomic radius increases and shielding increases due to electrons filling new principal energy levels, making the increased nuclear charge less significant. Therefore, iodine has a larger atomic radius and attracts electron density in a covalent bond less strongly than fluorine.
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IGCSE 11.1.1
- 1. Exothermic and endothermic reactions What are exothermic and endothermic reactions? 1 of 35 © Boardworks Ltd 2007
- 2. Exothermic and endothermic reactions What are exothermic and endothermic reactions? exothermic reactions release energy – they get hot ex = out (as in ‘exit’) thermic = relating to heat 2 of 35 © Boardworks Ltd 2007
- 3. Exothermic and endothermic reactions What are exothermic and endothermic reactions? exothermic reactions release energy – they get hot ex = out (as in ‘exit’) thermic = relating to heat endothermic reactions absorb energy – they get cold en = in (as in ‘entrance’) Most chemical reactions are exothermic. 3 of 35 © Boardworks Ltd 2007
- 4. Exothermic reactions Exothermic reactions release thermal energy (heat) into their surroundings. Exothermic reactions can occur spontaneously and some are explosive. 4 of 35 © Boardworks Ltd 2007
- 5. Exothermic reactions Exothermic reactions release thermal energy (heat) into their surroundings. Exothermic reactions can occur spontaneously and some are explosive. What are some examples? combustion respiration neutralization of acids with alkalis reactions of metals with acids the Thermit Process. 5 of 35 © Boardworks Ltd 2007
- 6. Reversible reactions and energy Reversible reactions are exothermic in one direction and endothermic in the other direction. For example: hydrated anhydrous copper sulfate copper sulfate + water CuSO4.5H2O CuSO4 + 5H2O 6 of 35 © Boardworks Ltd 2007
- 7. Reversible reactions and energy Reversible reactions are exothermic in one direction and endothermic in the other direction. For example: endothermic hydrated anhydrous copper sulfate copper sulfate + water CuSO4.5H2O CuSO4 + 5H2O 7 of 35 © Boardworks Ltd 2007
- 8. Reversible reactions and energy Reversible reactions are exothermic in one direction and endothermic in the other direction. For example: endothermic hydrated anhydrous copper sulfate copper sulfate + water CuSO4.5H2O CuSO4 + 5H2O exothermic 8 of 35 © Boardworks Ltd 2007
- 9. Reversible reactions and energy Reversible reactions are exothermic in one direction and endothermic in the other direction. For example: endothermic hydrated anhydrous copper sulfate copper sulfate + water CuSO4.5H2O CuSO4 + 5H2O exothermic The amount of energy transferred in each direction is exactly the same. 9 of 35 © Boardworks Ltd 2007