Exothermic and Endothermic Reactions Energy profile.pptx
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The document discusses exothermic and endothermic chemical reactions. Exothermic reactions release energy to the surroundings during the reaction, usually feeling hot. Endothermic reactions absorb energy from the surroundings, usually feeling cold. A reaction is exothermic if more energy is released during bond making than used during bond breaking, and endothermic if more energy is used in bond breaking than released in bond making. Energy diagrams show exothermic reactions releasing energy overall while endothermic reactions require energy input overall.
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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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Chemical reactions can be classified as either exothermic or endothermic based on whether energy is released or absorbed during the reaction. In an exothermic reaction, more energy is released from bond formation in the products than is required to break bonds in the reactants, resulting in a net release of energy. In an endothermic reaction, more energy is required to break bonds in the reactants than is released in bond formation in the products, resulting in a net absorption of energy. Common examples of exothermic reactions include combustion and yeast reactions, while photosynthesis and dissolving acid in water are typically endothermic.
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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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Chapter 7Energy and Metabolism© Cengage Learning 2015.docx
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SOLOMON • MARTIN • MARTIN • BERG
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Cells obtain energy in many forms, and have mechanisms that convert energy from one form to another
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The potential chemical energy released by cellular respiration is converted to kinetic energy in the muscles, which do the work of drawing the bow. The potential energy stored in the drawn bow is transformed into kinetic energy as the bowstring pushes the arrow toward its target.
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Passive vs. Active transport.mp4.downloadPassive vs. Active tra.docx
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Chapter 7:
Energy and Metabolism
© Cengage Learning 2015
SOLOMON • MARTIN • MARTIN • BERG
BIOLOGY
tenth edition
1
Energy Conversion
Cells obtain energy in many forms, and have mechanisms that convert energy from one form to another
Radiant energy is the ultimate source of energy for life
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© Cengage Learning 2015
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Matter: anything that has mass and takes up space
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Expressed in units of work (kilojoules, kJ) or units of heat energy (kilocalories, kcal)
1 kcal = 4.184 kJ
© Cengage Learning 2015
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Potential energy: capacity to do work as a result of position or state
Kinetic energy: energy of motion is used, work is performed
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© Cengage Learning 2015
Figure 7-1 Potential versus kinetic energy
The potential chemical energy released by cellular respiration is converted to kinetic energy in the muscles, which do the work of drawing the bow. The potential energy stored in the drawn bow is transformed into kinetic energy as the bowstring pushes the arrow toward its target.
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Organisms Carry Out Conversions Between Potential/Kinetic Energy
Most actions involve a series of energy transformations that occur as kinetic energy is converted to potential energy – or potential energy to kinetic energy
Chemical energy: potential energy stored in chemical bonds
Example: Chemical energy of food molecules is converted to mechanical energy in muscle cells
© Cengage Learning 2015
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Thermodynamics governs all activities of the universe, from cells to stars
Biological systems are open systems that exchange energy with their surroundings
Closed
system
Closed
system
Surroundings
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© Cengage Learning 2015
Figure 7-2 Closed and open systems
A closed system does not exchange energy with its surroundings.
(b) An open system exchanges energy with its surroundings.
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Energy cannot be created or destroyed
Energy can be transferred or converted from one form to another, including conversions between matter and energy
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Organisms must capture energy from the environment and transform it to a form that can be used for biological work
© Cengage Learning 2015
The Second Law of Thermodynamics
When energy is converted from one form to another, some usable energy (energy available to do work) is converted into heat that disperses in.
Passive vs. Active transport.mp4.downloadPassive vs. Active tra
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Passive vs. Active transport.mp4.download/Info.plist
__MACOSX/Passive vs. Active transport.mp4.download/._Info.plist
Chapter 7:
Energy and Metabolism
© Cengage Learning 2015
SOLOMON • MARTIN • MARTIN • BERG
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tenth edition
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Expressed in units of work (kilojoules, kJ) or units of heat energy (kilocalories, kcal)
1 kcal = 4.184 kJ
© Cengage Learning 2015
Potential Energy and Kinetic Energy
Potential energy: capacity to do work as a result of position or state
Kinetic energy: energy of motion is used, work is performed
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© Cengage Learning 2015
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The potential chemical energy released by cellular respiration is converted to kinetic energy in the muscles, which do the work of drawing the bow. The potential energy stored in the drawn bow is transformed into kinetic energy as the bowstring pushes the arrow toward its target.
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Organisms Carry Out Conversions Between Potential/Kinetic Energy
Most actions involve a series of energy transformations that occur as kinetic energy is converted to potential energy – or potential energy to kinetic energy
Chemical energy: potential energy stored in chemical bonds
Example: Chemical energy of food molecules is converted to mechanical energy in muscle cells
© Cengage Learning 2015
7.2 The Laws of Thermodynamics
Thermodynamics governs all activities of the universe, from cells to stars
Biological systems are open systems that exchange energy with their surroundings
Closed
system
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system
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© Cengage Learning 2015
Figure 7-2 Closed and open systems
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The First Law of Thermodynamics
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Chapter 7Energy and Metabolism© Cengage Learning 2015.docx
Chapter 7:
Energy and Metabolism
© Cengage Learning 2015
SOLOMON • MARTIN • MARTIN • BERG
BIOLOGY
tenth edition
1
Energy Conversion
Cells obtain energy in many forms, and have mechanisms that convert energy from one form to another
Radiant energy is the ultimate source of energy for life
Photosynthetic organisms capture about 0.02% of the sun’s energy that reaches Earth, and convert it to chemical energy in bonds of organic molecules
© Cengage Learning 2015
7.1 Biological Work
Matter: anything that has mass and takes up space
Energy: the capacity to do work (change in state or motion of matter)
Expressed in units of work (kilojoules, kJ) or units of heat energy (kilocalories, kcal)
1 kcal = 4.184 kJ
© Cengage Learning 2015
Potential Energy and Kinetic Energy
Potential energy: capacity to do work as a result of position or state
Kinetic energy: energy of motion is used, work is performed
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Energy of position
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Energy of motion
© Cengage Learning 2015
Figure 7-1 Potential versus kinetic energy
The potential chemical energy released by cellular respiration is converted to kinetic energy in the muscles, which do the work of drawing the bow. The potential energy stored in the drawn bow is transformed into kinetic energy as the bowstring pushes the arrow toward its target.
4
Organisms Carry Out Conversions Between Potential/Kinetic Energy
Most actions involve a series of energy transformations that occur as kinetic energy is converted to potential energy – or potential energy to kinetic energy
Chemical energy: potential energy stored in chemical bonds
Example: Chemical energy of food molecules is converted to mechanical energy in muscle cells
© Cengage Learning 2015
7.2 The Laws of Thermodynamics
Thermodynamics governs all activities of the universe, from cells to stars
Biological systems are open systems that exchange energy with their surroundings
Closed
system
Closed
system
Surroundings
Surroundings
© Cengage Learning 2015
Figure 7-2 Closed and open systems
A closed system does not exchange energy with its surroundings.
(b) An open system exchanges energy with its surroundings.
6
The First Law of Thermodynamics
Energy cannot be created or destroyed
Energy can be transferred or converted from one form to another, including conversions between matter and energy
The energy of any system plus its surroundings is constant
Organisms must capture energy from the environment and transform it to a form that can be used for biological work
© Cengage Learning 2015
The Second Law of Thermodynamics
When energy is converted from one form to another, some usable energy (energy available to do work) is converted into heat that disperses into the surroundings
As a result, the amount of usable energy available to do work in the universe decreases over time
Heat: the kinetic energy of randomly moving particles
© Cengage Learning 2015
Entropy
The measure of the disorder or randomness of energy
Organized, usable energy ...
Chapter 8(1)
This document provides an overview of metabolism and energy transformations in living systems. It discusses:
1) Metabolism transforms matter and energy through chemical reactions in organisms, subject to the laws of thermodynamics. Metabolic pathways involve a series of enzyme-catalyzed reactions that transform starting molecules into products.
2) Catabolic pathways break down molecules and release energy, while anabolic pathways consume energy to build molecules.
3) Energy can take different forms like kinetic, heat, potential, and chemical. The laws of thermodynamics state that energy cannot be created or destroyed, and entropy increases in closed systems.
4) Metabolism creates order from disorder by building complex molecules, but increases
Chapter 8(1)
This document provides an overview of metabolism and energy transformations in living systems. It discusses:
1) Metabolism transforms matter and energy through chemical reactions in organisms, subject to the laws of thermodynamics. Metabolic pathways involve sequences of enzyme-catalyzed reactions that transform starting molecules into products.
2) Catabolic pathways break down molecules and release energy, while anabolic pathways consume energy to build molecules.
3) Energy can take different forms but is conserved according to the first law of thermodynamics. The second law states that entropy increases as energy is transferred or transformed.
4) Metabolism decreases entropy locally by building biological structures but increases the universe's entropy, with energy entering
Passive vs. Active transport.mp4.downloadPassive vs. Active tra.docx
Passive vs. Active transport.mp4.download/Passive vs. Active transport.mp4
__MACOSX/Passive vs. Active transport.mp4.download/._Passive vs. Active transport.mp4
Passive vs. Active transport.mp4.download/Info.plist
__MACOSX/Passive vs. Active transport.mp4.download/._Info.plist
Chapter 7:
Energy and Metabolism
© Cengage Learning 2015
SOLOMON • MARTIN • MARTIN • BERG
BIOLOGY
tenth edition
1
Energy Conversion
Cells obtain energy in many forms, and have mechanisms that convert energy from one form to another
Radiant energy is the ultimate source of energy for life
Photosynthetic organisms capture about 0.02% of the sun’s energy that reaches Earth, and convert it to chemical energy in bonds of organic molecules
© Cengage Learning 2015
7.1 Biological Work
Matter: anything that has mass and takes up space
Energy: the capacity to do work (change in state or motion of matter)
Expressed in units of work (kilojoules, kJ) or units of heat energy (kilocalories, kcal)
1 kcal = 4.184 kJ
© Cengage Learning 2015
Potential Energy and Kinetic Energy
Potential energy: capacity to do work as a result of position or state
Kinetic energy: energy of motion is used, work is performed
POTENTIAL
Energy of position
KINETIC
Energy of motion
© Cengage Learning 2015
Figure 7-1 Potential versus kinetic energy
The potential chemical energy released by cellular respiration is converted to kinetic energy in the muscles, which do the work of drawing the bow. The potential energy stored in the drawn bow is transformed into kinetic energy as the bowstring pushes the arrow toward its target.
4
Organisms Carry Out Conversions Between Potential/Kinetic Energy
Most actions involve a series of energy transformations that occur as kinetic energy is converted to potential energy – or potential energy to kinetic energy
Chemical energy: potential energy stored in chemical bonds
Example: Chemical energy of food molecules is converted to mechanical energy in muscle cells
© Cengage Learning 2015
7.2 The Laws of Thermodynamics
Thermodynamics governs all activities of the universe, from cells to stars
Biological systems are open systems that exchange energy with their surroundings
Closed
system
Closed
system
Surroundings
Surroundings
© Cengage Learning 2015
Figure 7-2 Closed and open systems
A closed system does not exchange energy with its surroundings.
(b) An open system exchanges energy with its surroundings.
6
The First Law of Thermodynamics
Energy cannot be created or destroyed
Energy can be transferred or converted from one form to another, including conversions between matter and energy
The energy of any system plus its surroundings is constant
Organisms must capture energy from the environment and transform it to a form that can be used for biological work
© Cengage Learning 2015
The Second Law of Thermodynamics
When energy is converted from one form to another, some usable energy (energy available to do work) is converted into heat that disperses in.
Passive vs. Active transport.mp4.downloadPassive vs. Active tra
Passive vs. Active transport.mp4.download/Passive vs. Active transport.mp4
__MACOSX/Passive vs. Active transport.mp4.download/._Passive vs. Active transport.mp4
Passive vs. Active transport.mp4.download/Info.plist
__MACOSX/Passive vs. Active transport.mp4.download/._Info.plist
Chapter 7:
Energy and Metabolism
© Cengage Learning 2015
SOLOMON • MARTIN • MARTIN • BERG
BIOLOGY
tenth edition
1
Energy Conversion
Cells obtain energy in many forms, and have mechanisms that convert energy from one form to another
Radiant energy is the ultimate source of energy for life
Photosynthetic organisms capture about 0.02% of the sun’s energy that reaches Earth, and convert it to chemical energy in bonds of organic molecules
© Cengage Learning 2015
7.1 Biological Work
Matter: anything that has mass and takes up space
Energy: the capacity to do work (change in state or motion of matter)
Expressed in units of work (kilojoules, kJ) or units of heat energy (kilocalories, kcal)
1 kcal = 4.184 kJ
© Cengage Learning 2015
Potential Energy and Kinetic Energy
Potential energy: capacity to do work as a result of position or state
Kinetic energy: energy of motion is used, work is performed
POTENTIAL
Energy of position
KINETIC
Energy of motion
© Cengage Learning 2015
Figure 7-1 Potential versus kinetic energy
The potential chemical energy released by cellular respiration is converted to kinetic energy in the muscles, which do the work of drawing the bow. The potential energy stored in the drawn bow is transformed into kinetic energy as the bowstring pushes the arrow toward its target.
4
Organisms Carry Out Conversions Between Potential/Kinetic Energy
Most actions involve a series of energy transformations that occur as kinetic energy is converted to potential energy – or potential energy to kinetic energy
Chemical energy: potential energy stored in chemical bonds
Example: Chemical energy of food molecules is converted to mechanical energy in muscle cells
© Cengage Learning 2015
7.2 The Laws of Thermodynamics
Thermodynamics governs all activities of the universe, from cells to stars
Biological systems are open systems that exchange energy with their surroundings
Closed
system
Closed
system
Surroundings
Surroundings
© Cengage Learning 2015
Figure 7-2 Closed and open systems
A closed system does not exchange energy with its surroundings.
(b) An open system exchanges energy with its surroundings.
6
The First Law of Thermodynamics
Energy cannot be created or destroyed
Energy can be transferred or converted from one form to another, including conversions between matter and energy
The energy of any system plus its surroundings is constant
Organisms must capture energy from the environment and transform it to a form that can be used for biological work
© Cengage Learning 2015
The Second Law of Thermodynamics
When energy is converted from one form to another, some usable energy (energy available to do work) is converted into heat that disperses in ...
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2. Endothermic reactions absorb heat energy from their surroundings, causing a decrease in temperature. Dissolving salts in water is an example of an endothermic process.
3. Whether a reaction is exothermic or endothermic depends on whether more energy is released or absorbed during bond breaking and forming. Exothermic reactions release more energy than they absorb.
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5. chemical energetics
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1. Enthalpy change (ΔH) describes the energy stored in or released by a chemical reaction. Exothermic reactions (negative ΔH) release energy while endothermic reactions (positive ΔH) absorb energy.
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4. Gibbs
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Ch06 lecture
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chemistry GCSE chapter 6 Chemical Energetics.pptx
Chemical Energetics, Energy changes in reaction ,Exothermic and Endothermic reaction
Reaction profile ,Activation energy Bond and energy change
bond energy calculation
G-10 IG-CHEMICAL ENERGETICS 1 ..pptx
This document discusses chemical energetics and exothermic and endothermic reactions. It defines key terms like exothermic, endothermic, potential energy, and activation energy. Examples of exothermic reactions given are combustion reactions and neutralization which release heat. Burning fuels like methane and hydrogen are also exothermic. Endothermic reactions absorb heat from their surroundings. The document explains that bond breaking requires energy and is endothermic, while bond formation releases energy and is exothermic. Whether a reaction is exothermic or endothermic depends on the strength of bonds broken versus those formed. It concludes with questions for exercises.
Chemistry- exothermic reactions and properties
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- 1. Key Points ● When a chemical reaction happens, energy is transferred to or from the surroundings. ● When energy is transferred to the surroundings, this is called an exothermic reaction and usually feels hot. ● When energy is taken in from the surroundings, this is called an endothermic reaction and usually feel cold. 1
- 2. Exothermic or endothermic? ● If a reaction is exothermic overall, then more energy has been released during bond making than has been used for bond breaking. ● If a reaction is endothermic overall, then more energy has been used during bond breaking than has been released during bond making. 2
- 3. Energy level diagram – Exothermic reaction 3 Energy (kJ) Reactants Products Reaction time Ea Overall energy change = −ve
- 4. 4 Energy (kJ) Reactants Products Reaction time Ea Overall energy change = −ve Energy is being used to break the bonds in the reactants Energy level diagram – Exothermic reaction
- 5. 5 Energy (kJ) Reactants Products Reaction time Ea Overall energy change = −ve New bonds are formed here and energy is released Energy level diagram – Exothermic reaction
- 6. Energy level diagram – Exothermic reaction 6 Energy (kJ) Reactants Products Reaction time Ea More energy is released in bond making than is required for bond breaking, so this reaction is exothermic overall
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- 11. Energy level diagram – Endothermic reaction 11 Energy (kJ) Reactants Products Reaction time Ea Overall energy change = +ve Energy is being used to break the bonds in the reactants
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