Exothermic and endothermic
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Fossil fuels such as petroleum formed from the remains of ancient plants and animals that lived hundreds of millions of years ago. When these organisms died, their remains were buried underground over time by layers of sediment. Through the application of heat, pressure, and microbial activity, the buried organic matter was converted into petroleum and other fossil fuels over millions of years.
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This document discusses endothermic and exothermic reactions. It provides examples of exothermic reactions like combustion and cellular respiration which release energy. Exothermic reactions are illustrated as having energy released by the reactants. Endothermic reactions like photosynthesis and cold packs absorb energy, shown as energy being absorbed by the reactants. Both reaction types are accompanied by temperature changes or energy transfers that allow identification of whether energy is released or absorbed in a chemical reaction.
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This document discusses chemical reactions and properties of matter. It defines physical and chemical properties, and explains that a chemical change produces new substances while a physical change does not. It also outlines how to identify chemical reactions through observation of properties like color change, gas production, or precipitate formation. The document then explains how to write and balance chemical equations, and categorizes three main types of chemical reactions: synthesis, decomposition, and replacement. Finally, it discusses factors that affect the rate of chemical reactions like surface area, temperature, concentration, and catalysts.
17.1 17.2 lecture slides
Thermochemistry is the study of energy changes that occur during chemical reactions and changes in state. Heat is energy that transfers from one object to another due to a temperature difference. In an endothermic process, the system gains heat from its surroundings, while in an exothermic process the system loses heat to its surroundings. Calorimetry allows for the precise measurement of heat flow during chemical and physical processes using an insulated calorimeter. The enthalpy change of a reaction, measured in kilojoules, can be determined from calorimetry experiments and represented in a thermochemical equation.
2.1 Chemical Formulas and Equations
This document discusses chemical reactions and equations. It explains that chemical reactions involve substances changing partners to form new substances, while conserving mass. Chemical equations are used to represent these reactions, showing the reactants, products, and phase changes. The document also discusses how energy is often either released or absorbed during chemical reactions, depending on whether the bonds in the products are more or less stable than the reactants. Key terms like endothermic and exothermic are introduced to describe reactions that absorb or release thermal energy.
Ppt chemical reactions
This document defines and describes chemical reactions. It explains that in a chemical reaction, atoms rearrange to form new compounds, with old bonds breaking and new bonds forming. Chemical reactions can be represented by chemical equations that show the reactants and products. Reactions can be exothermic, releasing energy, or endothermic, absorbing energy. They can also vary in reaction rate. The document also covers the law of conservation of matter, balancing chemical equations, and the main types of chemical reactions: synthesis, decomposition, single replacement, double replacement, and combustion reactions.
1406 ch 4 energy and enzymes blank sp 2018
This document discusses energy and chemical reactions in living cells. It covers:
1) Two main forms of energy - kinetic and potential - and how sunlight provides kinetic energy for photosynthesis which produces chemical potential energy in sugars.
2) Chemical reactions in cells, including exergonic reactions which release energy and endergonic reactions which require energy input.
3) How ATP is used to transfer energy from exergonic reactions to drive endergonic reactions and cellular tasks.
Chapter 3 Chemical Reactions
Chemical reactions involve the rearrangement of atoms. There are two main types of chemical changes - synthesis reactions which combine simpler substances into more complex ones, and decomposition reactions which break down a substance into simpler parts. Chemical equations are used to represent chemical reactions, and must obey the law of conservation of mass by being balanced. Reactions can release or absorb energy depending on whether the bonds in the products are stronger or weaker than the bonds in the reactants. Living things and industry rely on exothermic and endothermic chemical processes.
Definitions and MCQs of Ninth Class Chemistry (chemical energetics)
This document defines key terms related to chemical energetics and thermodynamics. It discusses exothermic and endothermic reactions, heat of formation, standard heat of formation, and enthalpy. It also provides multiple choice questions to test understanding of these concepts, such as identifying whether photosynthesis is an exothermic or endothermic reaction.
Endo and exo rections experiments
This document summarizes endothermic and exothermic reactions. It defines physical and chemical changes, noting indicators of chemical changes like temperature change, odor change, formation of precipitates, and sometimes color change. Exothermic reactions release energy to the surroundings, lowering their temperature, while endothermic reactions absorb energy from the surroundings, raising their temperature. Examples of exothermic reactions given are combustion, evaporation of water, and the mixing of sodium and chlorine to form table salt. Examples of endothermic reactions include cold packs and melting ice. The document also discusses activation energy, cellular respiration, photosynthesis, and conduction of two experiments on exothermic reactions involving citric acid/baking soda and steel wool
Energy From The Atom
There are three main ways that energy can be released from atoms: radioactivity, chemical reactions, and the excitation of electrons. Radioactivity occurs when unstable atomic nuclei decay by emitting particles like alpha or beta rays. Chemical reactions release energy when chemical bonds are broken and formed. Electron excitation occurs when electrons absorb energy and jump to higher energy levels, releasing energy as light when they fall back down.
Power Notes: Physical vs. Chemical
Today's science lesson will cover:
1. Physical vs chemical changes through notes and worksheets
2. Identifying volume through a lab
3. Test #2 on learning points from Oct 20-21 including notes and binder check
4. Basic particles that make up substances and how this determines if a change is physical or chemical
5. Signs that a chemical reaction may be occurring and examples of physical and chemical properties
6. The difference between endothermic and exothermic reactions
Chapter17 Section01 Edit
- The document discusses heat transfer and energy transformations, explaining that heat always flows from warmer objects to cooler ones. It defines endothermic processes as those that absorb heat from surroundings and exothermic processes as those that release heat.
- Specific heat is introduced as the amount of heat needed to raise 1g of a substance by 1°C, and heat capacity as the amount of heat needed to change an object's temperature by 1°C. Water is noted to release a lot of heat as it cools.
February 25
The document provides an agenda and lesson plan for a chemistry class on the topic of conservation of mass. The agenda includes a warm-up, setting up notes, a candle demonstration, a conservation of mass activity, and finishing with notes and answering focus questions. The demonstration shows how atoms are conserved in a chemical reaction by rearranging to form new substances, as seen in the burning of a candle. Students then do a hands-on modeling activity and learn that the atoms in the reactants are the source of the atoms in the products.
Exothermic and Endothermic Reactions.ppt
The document discusses exothermic and endothermic chemical reactions. Exothermic reactions release heat energy and cause an increase in temperature, while endothermic reactions absorb heat energy and cause a decrease in temperature. All chemical reactions require activation energy to break existing bonds between atoms before new bonds can form, releasing or absorbing energy. Catalysts can lower the activation energy needed for a reaction to occur, speeding up the reaction.
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Definitions and MCQs of Ninth Class Chemistry (chemical energetics)
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Solution concentration
This document discusses different units for expressing concentration of solutions, including percent, parts per hundred (pph), and parts per million (ppm). It provides an example of calculating the concentration in percent by mass of a solution containing 25 g of sucrose dissolved in 175 g of water.
Digestion acids
Acids have a pH between 1 and 7, with stronger acids having a lower pH. They are able to break down chemicals into smaller parts through chemical reactions. Our bodies use acid in digestion to break down food. Hydrochloric acid in the stomach has a very low pH of 2.0 and helps break down food, though the stomach is lined with mucus to protect it from this strong acid. Heartburn occurs when stomach acid rises into the esophagus, and is often treated by neutralizing the acid with products containing calcium carbonate like TUMS.
Acids & bases
Acids have H+ ions dissolved and are corrosive to metals, with a sour taste and pH below 7. Bases have OH- ions dissolved, feel soapy or slippery, have a bitter taste, and pH above 7. The pH scale measures if a substance is acidic, basic, or neutral, with 0-7 being acidic, 7 being neutral, and 7-14 being basic. A change of one pH unit is a 10 times difference in acidity or basicity, so a pH of 2 is 100 times more acidic than a pH of 4. Water that is too acidic or basic can harm fish development, increase toxic metals, or dissolve organic materials like skin and scales. Drinking water should have a
Reaction rates
The document discusses chemical reactions and factors that affect their rates. It explains that reactions can be exothermic, releasing energy, or endothermic, absorbing energy. All reactions require a minimum amount of energy called the activation energy to initiate the rearrangement of reactants into products. The rate of reactions can be increased by raising the temperature, increasing the concentration or surface area of reactants, using catalysts to lower the activation energy, or through mechanical means like stirring. An experiment is described that shows reaction rates increase as particle size decreases due to greater surface area exposure.
Covalent bonding
Covalent bonds form between two atoms that share a pair of electrons. To draw covalent bonds, determine the number of valence electrons for each atom and draw them as dots singly or in pairs. Electrons spread out first before pairing up. Covalent bonds are then drawn as lines between atoms to show how the valence electrons are shared to form molecules such as H2 and CH4.
Major molecule properties
The four major molecules in food are carbohydrates, fats, proteins, and water. Carbohydrates provide the body's main source of energy and are found in grains, rice, bread and other foods. Fats also provide energy and are important for health, though eaten in excess they are stored in the body. Proteins are made of amino acids and are essential for many processes in the body. Finally, water makes up 70% of the body and is necessary for transport and chemical reactions.
The water cycle
The water cycle describes the continuous movement of water on, above, and below the surface of the Earth. Water evaporates from surfaces like oceans, lakes, and rivers and rises into the air as vapor. The vapor cools and condenses to form clouds and precipitation falls back to Earth as rain, snow, sleet, or hail, completing the cycle.
Solubility
Something dissolved in the Snake River could have caused the fish kill. Polar molecules and ionic compounds can dissolve in water due to the attractions between the water molecules and these substances. The rule is that "like dissolves like," so polar substances dissolve in polar water, while nonpolar substances do not. As temperature increases, the solubility of solids and gases generally increases and decreases, respectively, as shown by solubility curves.
Symbols & formulas
Chemical formulas have three parts: symbols, subscripts, and coefficients. Symbols represent elements with the first letter capitalized. Formulas show what elements are connected and subscripts indicate the number of each atom. Coefficients show how many copies or molecules there are and atoms are separate, not connected. Examples are given of formulas such as CO2, C12H22O11, and MgCl2 to demonstrate how to read the subscripts and coefficients.
Properties of metals and nonmetals
Metals are found on the left side of the periodic table, have properties such as luster, malleability, conductivity, and react with acids. Nonmetals are found on the right side, have properties such as being dull, brittle, not conducting electricity, and usually being gases. Metalloids are in between metals and nonmetals on the periodic table and have some properties of both.
Physical & chemical properties
This document discusses the physical and chemical properties of matter. It defines matter as anything that has mass and takes up space. Physical properties can be observed without changing the material and include characteristics like color, hardness, and melting point. Chemical properties involve a change in the material's composition through reactions with other substances, such as rusting or burning. Some examples provided assess whether various phenomena are physical or chemical properties.
Mixtures
A mixture is a combination of two or more substances that can be physically separated and where the substances retain their own properties. Mixtures can be either homogeneous, where the substances are evenly distributed throughout so it appears to be one substance, or heterogeneous, where the distinct substances can be seen separated into more than one phase. Examples of mixtures include solutions, suspensions, and alloys.
Elements & compounds
The document discusses the differences between elements and compounds. It explains that elements are pure substances made of only one type of atom, while compounds contain two or more different types of atoms that are chemically bonded together. It provides examples of common elements like carbon, oxygen, and neon, as well as examples of compounds, including water (H2O) and sodium chloride (NaCl).
Density
Density is a measurement of how much mass is contained within a given volume, calculated by dividing the mass of an object by its volume. A document provides instructions on how to calculate the density of a substance with a mass of 17.63g and volume of 43cm3, which equals 0.41 g/cm3, identifying the substance as the least dense compared to others.
Density
Density is a measurement of how much mass is contained within a given volume, calculated by dividing the mass of an object by its volume. A document provides instructions on how to calculate the density of a substance with a mass of 17.63g and volume of 43cm3, which equals 0.41 g/cm3, identifying the substance as the least dense of those listed.
Temperature & Volume
Gay-Lussac's Law states that pressure and temperature are directly related for a gas at constant volume: if temperature increases, pressure increases; if temperature decreases, pressure decreases. This is because temperature affects the kinetic energy of gas particles - higher temperature means more kinetic energy and more frequent and energetic particle collisions, resulting in higher pressure. The law can be expressed as P1/T1 = P2/T2, allowing calculations of pressure changes with temperature changes when volume is held constant and temperatures are in Kelvin.
Pressure & Volume
This document discusses the kinetic molecular theory and Boyle's law. It explains that gases are made of molecules that are far apart from each other and move randomly, colliding with the container walls. According to Boyle's law, if the volume of a container decreases, the pressure increases because the molecules collide with the walls more frequently. The document provides the formula for Boyle's law, P1V1 = P2V2, and gives examples of using it to calculate pressure and volume.
Pressure
Pressure is defined as force per unit area. It can be measured in units such as pounds per square inch, atmospheres, or pascals. Air pressure in the atmosphere is caused by gas molecules constantly colliding with surfaces and exerting force. Standard air pressure at sea level is approximately 101 kPa or 14.7 psi. Pressure calculations involve dividing the total force by the area over which that force is applied.
Matter notes
Matter comes in four forms: solids have a definite shape and volume, liquids have a definite volume but not shape, gases have no definite shape or volume, and plasmas are charged particles with no definite shape or volume. The document introduces the basic properties and states of matter, including solids, liquids, gases, plasmas, atoms, and examples of things made of plasma like flames, nebulae, and stars.
Volume notes
The document discusses volume, which is the amount of space an object occupies. It describes how to measure volume using beakers or graduated cylinders and notes units like liters and milliliters. For liquids, a graduated cylinder should always be used to measure volume and the meniscus read from the bottom. For solids, regular objects use the formula of length x width x height while irregular objects use water displacement by finding the difference in water level before and after the object is added.
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Exothermic and endothermic
- 2. How did fossil fuels form? 500 million years ago living matter- mostly plants- died and was buried in sediment. Pressure, heat, and microbes converted the organic matter into petroleum. Buried sunshine?
- 4. Potential Energy Stored energy or energy of position
- 5. Kinetic Energy Energy related to motion video clip
- 6. Chemical energy A form of potential energy that is stored in the bonds of chemical compounds. Burning hydrocarbons releases energy in the form of heat and light
- 7. Types of energy in chemical reactions Endothermic: energy “enters” the reaction Feels ________________ Exothermic: energy “exits” the reaction Feels ________________
- 8. Reactions take place in 2 steps: 1) Bonds must be broken in the starting reactants. * When bonds are broken, energy is released. So this is an exothermic process. CH4 + 2O2 C + 4H + 4O + Energy
- 9. Step 2: Separated atoms now join to form a new bonds to make the products. It takes energy to form bonds, so this process is endothermic. Energy + C + 4H + 4O CO2 + 2 H2O
- 10. CH4 + 2O2 C + 4H + 4O
- 11. Net equation for burning of methane CH4 + 2O2 CO2 + 2H2O + energy Notice the energy shows up as a product so more energy was released so the reaction is exothermic. gummy bear experiment
- 12. Energy + 2H2O 2H2 + O2 Is more energy put into the reaction or released by the reaction? Is the reaction endothermic or exothermic? endothermic reaction