2016 topic 5.2 hess's law
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1. Hess's law states that the overall enthalpy change of a chemical process is independent of the path taken. 2. The document uses the reaction of sodium hydroxide and hydrochloric acid to illustrate Hess's law. It shows that the enthalpy change of the direct reaction is equal to the sum of the enthalpy changes for the stepwise reactions. 3. Representing the reactions on an enthalpy level diagram and enthalpy cycle confirms that Hess's law applies, with the enthalpy change for the overall reaction being the sum of the enthalpy changes for the individual steps.
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The document discusses electron configuration and trends in ionization energy. It explains that ionization energy decreases down a group and increases across a period due to changes in effective nuclear charge. Electrons fill atomic orbitals according to Aufbau principle and Hund's rule. The document provides examples of writing electron configurations and condensed configurations for various elements. Successive ionization energy data supports the electron configuration model.
Chapter 9 manufacture substances
This document discusses several important industrial products and manufactured substances. It provides details on the production and uses of sulphuric acid, ammonia, alloys, synthetic polymers, glass, ceramics, and composite materials. Sulphuric acid is manufactured through the contact process and is used to make fertilizers and batteries. Ammonia is produced via the Haber process and converted into fertilizers. Alloys are metal mixtures that are stronger than pure metals. Glass and ceramics are hard, brittle materials made from sand and clay, respectively. Composite materials combine substances like metals and polymers to produce materials with improved properties.
Chapter 7 acid & bases part 4
The document discusses neutralization reactions and acid-base titrations. It explains that neutralization is a reaction between acids and bases that produces salts and water. It provides examples of neutralization equations. It also describes acid-base titrations as a quantitative analysis involving gradually adding an acid or base from a burette to determine the endpoint, or point at which the indicator changes color. The document provides practice problems involving using molarity, volumes, and balanced equations to calculate concentrations or volumes in neutralization reactions.
IB Chemistry on Ionization energy and electron configuration
The document discusses the periodic table and electron configuration of elements. It is divided into s, p, d and f blocks. The s block elements have s orbitals that are partially filled. The d block elements have d orbitals that are partially filled and are known as transition elements. The f block elements have f orbitals that are partially filled. The p block elements have p orbitals that are partially filled. Electrons fill orbitals according to the Aufbau principle, Hund's rule and Pauli exclusion principle. Elements are written in their full electron configuration or condensed noble gas notation.
Chapter 7 Acid & Bases part 1
The document discusses acids, bases, and alkalis. It defines them, provides examples, and explains their properties and uses. Acids donate H+ ions in water, bases accept H+ ions and alkalis dissolve in water to form hydroxide ions. Properties of acids include sour taste and turning litmus red, while alkalis have a bitter taste and turn litmus blue. Common acids and bases are used in products like cleaners, soaps, batteries, and more.
IB Chemistry on Mole Concept
1. The document discusses moles, molar mass, and calculations involving moles. It provides examples of calculating the number of particles, ions, or molecules in 1 mole of various substances like iron, carbon dioxide, sodium chloride, and magnesium chloride.
2. It also explains how to calculate molar mass using relative atomic mass and gives examples for iron, carbon dioxide, sodium chloride, and magnesium chloride.
3. Key concepts discussed include the definition of 1 mole as 6.02 x 1023 particles and its relationship to the Avogadro constant, and how molar mass is used to express the mass of 1 mole of a substance.
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IB Chemistry on Ionization energy and electron configuration
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Similar to 2016 topic 5.2 hess's law
Question 1. Dscribe the change you observed when you added 1 mL of 0.pdf
Question 1 5 pts Given the cash flow diagram below, evaluate the value of \"A\" if the \"F\"
value is $24.000 for an interest rate of 7%. ?? 4A
Solution
Future Value of investents: Year Investment Future Value of Investment of 1 Future
Value of Investment a b c=1.07^(5-a) d=b*c 1 A 1.3108
1.3108 A 2 2A 1.2250 2.4501 A 3 3A 1.1449
3.4347 A 4 4A 1.0700 4.2800 A
11.4756 A Now, As per question, 11.4756 A = $
24,000 or, A = $ 2,091.40 Thus, Value of A $ 2,091.40.
Ch7_Section7.8 PrintableHandout.pdf
This document summarizes acid-base reactions and gas-forming reactions. It defines acids and bases according to Arrhenius theory and provides examples of strong and weak acids and bases. Acid-base reactions involve the reaction of hydrogen ions from acids with hydroxide ions from bases to form water. These reactions are also called neutralization reactions. Gas-forming reactions produce a gas, such as reactions between acids and carbonates or metals. Common gases formed include hydrogen, carbon dioxide, hydrogen sulfide and ammonia.
22 acids + bases
This document discusses acids and bases according to several theories. It begins by describing the properties of acids, including reacting with metals and carbonates, conducting electricity, turning litmus paper colors, and neutralizing bases. It then discusses the properties of bases. The Arrhenius theory defines acids as substances that produce H+ ions in water and bases as those that produce OH- ions. However, this theory has limitations and does not account for all acids and bases. The Brønsted-Lowry theory broadens the definition to any substance that can donate or accept protons. Strong acids fully dissociate in water while weak acids only partially dissociate. The pH scale measures the concentration of H+ ions on a
21 acids + bases
This document discusses acids and bases according to several theories. It begins by describing the properties of acids, including reacting with metals and carbonates, conducting electricity, turning litmus paper colors, and neutralizing bases. It then discusses the properties of bases. The Arrhenius theory defines acids as substances that produce H+ ions in water and bases as those that produce OH- ions. However, this theory has limitations and does not account for all acids and bases. The Brønsted-Lowry theory broadens the definition to any substance that can donate or accept protons. Strong acids fully dissociate in water while weak acids only partially dissociate. The pH scale measures the concentration of H+ ions on a
Equilibrium
This document covers various topics related to chemical equilibrium including:
1. Irreversible and reversible reactions, and examples of each.
2. Types of equilibrium including homogeneous, heterogeneous, physical, and chemical equilibrium.
3. The law of mass action and how equilibrium constants are calculated.
4. How changing conditions like temperature, pressure, and concentration affects chemical equilibria.
5. Additional topics like acid-base theories, buffer solutions, and solubility products are also briefly discussed.
Ch7PowerPoint_Section7.8.pdf
This document discusses acid-base reactions and gas-forming reactions. It defines acids and bases according to Arrhenius theory and provides examples of strong and weak acids and bases. Acid-base reactions involve the reaction of hydrogen ions from acids with hydroxide ions from bases to form water. This neutralizes the acid and base. Gas-forming reactions produce a gas, such as reactions of acids with carbonates or metals. These reactions are driven by the formation of products like water, salts, or gases.
Ch4 Reactions in Aqueous Solution (updated)
A document discusses various topics relating to chemistry solutions including:
1) The definition of solutions, solvents, and solutes. A solution is a homogeneous mixture of substances where the solute is the smaller component dissolved in the solvent.
2) Properties of aqueous solutions including that electrolytes can conduct electricity while nonelectrolytes cannot. Strong electrolytes dissociate completely while weak electrolytes only partially dissociate.
3) Reactions involving solutions such as precipitation reactions, acid-base reactions, and redox reactions. Precipitation occurs when an insoluble solid forms. Acid-base reactions involve acids and bases reacting to form water and a salt. Redox reactions involve the transfer of electrons
Chapter 11
This document describes chemical reactions and equations. It discusses:
1. The components of chemical equations including reactants and products.
2. The different types of chemical equations including word equations, skeleton equations, and chemical equations.
3. How to balance chemical equations by ensuring equal numbers of each type of atom on both sides of the reaction arrow.
4. The five major types of chemical reactions - combination, decomposition, single replacement, double replacement, and combustion.
5. How to predict whether a precipitation reaction will occur based on solubility rules for ionic compounds.
Tang 09 reactions - addition 2
This document discusses addition reactions, which involve a double bond becoming a single bond by the addition of two groups of atoms. It describes several types of addition reactions: halogenation, hydrogenation, hydrohalogenation, and hydration. Halogenation and hydrohalogenation result in the formation of alkyl halides, while hydrogenation forms alkanes and hydration forms alcohols. The document provides examples of addition reactions and uses the Markovnikov rule to predict product formation.
It is a molecular process involving the exchange .pdf
It is a molecular process involving the exchange of bonds between the two reacting
chemical species, which results in the creation of products with similar or identical bonding
affiliations. This is represented by the general reaction scheme: AX + BY ? BX + AY These
chemical species can either be ionic or covalent. When referring to precipitation reactions
between solutions of ions in inorganic chemistry, these were formerly referred to as double
displacement or double replacement reactions, and these terms are still encouraged. It seems that
the term double decomposition is more specifically used when at least one of the substances does
not dissolve in the liquor, as the ligand or ion exchange takes place in the solid state of the
reactant, i.e. AX(aq) + BY(s) ? AY(aq) + BX(s). Types: Neutralization A neutralization reaction
is a specific type of double displacement reaction. Neutralization occurs when an acid reacts with
an equal amount of a base. A neutralization reaction creates a solution of a salt and water. For
example, hydrochloric acid reacts with sodium hydroxide to produce salt and water: HCl (aq) +
NaOH (aq) ? NaCl (aq) + H2O (l) Aqueous metathesis (precipitation) Metathesis reactions can
occur between two inorganic salts when one product is insoluble in water, driving the reaction
forward. For example, the precipitation of silver chloride from a mixture of silver nitrate and
sodium chloride causes sodium nitrate to be left in solution: AgNO3 (aq) + NaCl (aq) ? AgCl (s)
+ NaNO3 (aq) The formation of an insoluble gas that bubbles out of the solution, or a molecular
compound such as water, also drives the reaction to completion. Therefore, a solubility chart (or
general knowledge of solubility rules) can be used to predict whether two aqueous solutions will
react. HSAB theory can also be used to predict the products of a metathesis reaction. Aqueous
metathesis (double decomposition) The reactants need not to be dissolved for metathesis
reactions to take place. An example of this is the formation of barium thiocyanate when boiling a
mixture of copper(I)thiocyanate and barium hydroxide in water: Ba(OH)2 (s) + 2 CuCNS (s) ?
Ba(CNS)2 (aq) + 2CuOH (s) Acid and carbonates A subcategory of aqueous metathesis
reactions is the reaction of an acid with a carbonate or bicarbonate. Such a reaction always yields
carbonic acid as a product, which spontaneously decomposes into carbon dioxide and water. The
release of carbon dioxide gas from the reaction mixture drives the reaction to completion. For
example, a common, science-fair \"volcano\" reaction involves the reaction of acetic acid with
sodium bicarbonate: HCH3COO (aq) + NaHCO3 (s) ? NaCH3COO (aq) + CO2 (g) + H2O (l)
Solution
It is a molecular process involving the exchange of bonds between the two reacting
chemical species, which results in the creation of products with similar or identical bonding
affiliations. This is represented by the general reaction scheme: AX + BY ? BX + AY These
che.
Introduction_to_Chemical_Reactions_2011-2012.ppt
1) A chemical reaction is a process where one or more substances are destroyed and one or more new substances are created.
2) There are five main types of chemical reactions: single replacement, double replacement, synthesis, decomposition, and combustion.
3) Evidence for a chemical reaction includes evolution of light or heat, temperature changes, formation of gases or precipitates, and color changes.
Introduction_to_Chemical_Reactions_2011-2012.ppt
The document provides an introduction to chemical reactions, including definitions, parts of reactions, types of reactions, and evidence of reactions. It explains that a chemical reaction is a process where reactants are destroyed and products are formed, with the following key points:
- Reactants undergo chemical change to form products, as indicated by the yield arrow (→).
- Chemical equations must obey the law of conservation of mass, with the same number and type of atoms on both sides of the reaction.
- The five main types of chemical reactions are synthesis, decomposition, single replacement, double replacement, and combustion.
- Several tests can indicate if a chemical reaction has occurred, such as gas evolution, temperature change, color change,
Introduction to Chemical Reaction and types
1) A chemical reaction is a process where one or more substances are destroyed and one or more new substances are created.
2) There are five main types of chemical reactions: single replacement, double replacement, synthesis, decomposition, and combustion.
3) Evidence for a chemical reaction includes evolution of light or heat, temperature changes, formation of gases or precipitates, and color changes.
Chemical_Reactions.ppt
1) A chemical reaction is a process where one or more substances are destroyed and one or more new substances are created.
2) There are five main types of chemical reactions: single replacement, double replacement, synthesis, decomposition, and combustion.
3) Evidence for a chemical reaction includes evolution of light or heat, temperature changes, formation of gases or precipitates, and color changes.
22 acids + bases
The document discusses the key properties and reactions of acids and bases. It defines acids as substances that produce hydrogen ions (H+) in water and bases as substances that produce hydroxide ions (OH-). Acids react with metals, carbonates, conduct electricity, turn litmus paper red, and neutralize bases. Bases conduct electricity, turn litmus paper blue, and neutralize acids. Theories of acids and bases including Arrhenius, Brønsted-Lowry, and Lewis are explained. Strong and weak acids/bases, monoprotic/diprotic/triprotic acids, pH, titrations, and acid-base indicators are also covered.
Ch04 outline
This document summarizes key concepts in solution chemistry and stoichiometry, including:
1) Solutions, electrolytes, dissociation, and precipitation reactions are discussed. Strong and weak electrolytes are defined.
2) Acid-base reactions such as neutralization and gas-forming reactions are covered. Oxidation-reduction reactions and displacement reactions are also summarized.
3) Concepts including molarity, dilution, and titration reactions are introduced for quantitative chemical calculations.
AP Chemistry Chapter 4 Outline
This document summarizes key concepts in solution chemistry and stoichiometry, including:
1) Solutions, electrolytes, dissociation, and precipitation reactions are discussed. Strong and weak electrolytes are defined.
2) Acid-base reactions such as neutralization and gas-forming reactions are covered. Oxidation-reduction reactions and oxidation numbers are also introduced.
3) Concepts like molarity, dilution, and titration are explained as methods to quantify concentrations in solutions and chemical reactions.
Class 10 l Science l Chemistry l Lesson 1: Chemical equations and reactions
A chemical reaction involves one or more reactants forming new products with different properties. Chemical equations represent reactions symbolically, with balanced equations showing equal numbers of atoms on both sides. There are several types of reactions including combination, decomposition, exothermic/endothermic, displacement, neutralization, and oxidation-reduction. Identification of a reaction can occur through changes in state, color, gas evolution, temperature change, or precipitate formation.
hesses low.pptx
1) Hess's law states that the total enthalpy change of a chemical reaction is independent of the pathway as long as the initial and final states are the same.
2) The enthalpy change for a reaction can be calculated by adding the enthalpy changes of formation of the products and subtracting the enthalpy changes of formation of the reactants.
3) Examples are provided to demonstrate calculating enthalpy changes of reactions using Hess's law and standard enthalpy of formation values.
6.4
The document discusses acids, bases, and salt hydrolysis. Acids are substances that donate hydrogen ions in water, while bases donate hydroxide ions. The modified Arrhenius definition accounts for salts dissociating in water, with their ions sometimes accepting or donating hydrogen ions. This causes solutions of salts to be slightly acidic or basic, explaining why some neutralization reactions do not reach a pH of 7. Examples show sodium acetate hydrolyzing to produce hydroxide ions, making its solution basic, while ammonium chloride hydrolyzes to produce hydrogen ions, making its solution acidic.
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It is a molecular process involving the exchange .pdf
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Class 10 l Science l Chemistry l Lesson 1: Chemical equations and reactions
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A projectile is an object moving under the influence of gravity with a parabolic path. Its motion can be analyzed by separating the horizontal and vertical components. In the horizontal direction, the velocity is constant, while in the vertical direction there is a constant acceleration due to gravity. Projectile motion is used to model many real-world scenarios like thrown objects, diving, and artillery fire. Solving projectile motion problems involves separating the horizontal and vertical motions and using kinematic equations with the initial velocities and gravitational acceleration.
1.3 velocity
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1.2 displacement and position vs time graphs
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2) Victor's displacement is calculated as his final position (2km North of Starbucks) minus his initial position (3km South of Starbucks), equaling 5km North.
3) A position-time graph shows an object's position over time. The slope of the line between any two points represents the average velocity during that time interval.
1.1 vectors
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2) Vectors can be described by their magnitude, direction, and reference frame. Direction is measured in degrees from the x-axis.
3) Vector operations like addition, subtraction, multiplication and division can be performed graphically or using components and trigonometry. Parallel vectors can be added/subtracted algebraically but others require using components.
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2016 topic 4.5 bonding - metallic
Metallic bonding involves a lattice of positive metal ions surrounded by delocalized electrons that form a negative "electron cloud". This electron cloud binds the positively charged ions together and is responsible for metals' properties. Metals exhibit high electrical conductivity because the mobile electron cloud allows electrons to move freely throughout the structure. The strength of metallic bonding depends on electron density and ionic radius - greater electron density and smaller ionic radius lead to stronger bonding and higher melting points. Alloys are mixtures of metals designed to enhance properties like strength, corrosion resistance, magnetism, and ductility.
2016 topic 4.2 bonding - covalent
This document provides an overview of ionic bonding. Ionic bonds form between elements when one atom loses electrons to become a positively charged ion and another atom gains those electrons to become a negatively charged ion. For example, in sodium chloride, sodium atoms lose electrons to form Na+ ions and chloride atoms gain electrons to form Cl- ions. The oppositely charged ions are then held together by electrostatic forces in a repeating crystal lattice structure. Ionic compounds have high melting points, are brittle, and do not conduct electricity in solid form but do conduct when molten or dissolved in water as the ions become mobile.
Unit 4 2014 ppt sound
This document discusses the basics of sound waves. It explains that sound waves are caused by vibrations, requiring a medium like air, liquid or solid to transfer energy. It describes how compression and rarefaction of molecules transfers sound waves. Frequency determines pitch, with higher frequencies being higher pitched. Amplitude determines loudness, with greater amplitude being louder. Graphs can show the displacement over time of sound waves to represent characteristics like frequency and amplitude. The speed of sound depends on the medium and temperature.
Unit 4 2014 ppt wave characteristics
The document summarizes key concepts about waves, including:
1) Waves can be classified as mechanical or electromagnetic depending on whether they require a medium to travel. Mechanical waves include sound and water waves while electromagnetic waves include radio and light waves.
2) Waves can be transverse, with oscillations perpendicular to the direction of travel, or longitudinal, with oscillations parallel to the direction of travel.
3) Key wave properties include frequency, wavelength, period, amplitude, and speed. The speed of a wave depends on properties of the medium and can be calculated from the wavelength and period.
2016 topic 01 part 1
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- A mole is a unit used to count fundamental particles and represents 6.02x1023 particles.
- The mole allows converting between large numbers of particles and more manageable units like grams.
- Molar mass relates the mass of a sample of a substance to the number of moles it contains.
- Problems use molar mass to calculate moles, particles, or mass given any two of those quantities.
Chemistry 1 - Atomic Structure
- Atoms consist of a nucleus containing protons and neutrons surrounded by electrons in orbitals.
- The atomic number is the number of protons, which identifies the element. The mass number is the total number of protons and neutrons.
- Isotopes are atoms of the same element with different numbers of neutrons. The relative atomic mass takes into account the natural abundance of isotopes.
2016 Topic 2: Electron Configuration
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2016 Topic 2: Atomic Structure
This document discusses atomic structure and properties. It begins by reviewing the basic atomic model including protons, neutrons, and electrons. It then discusses atomic number, mass number, isotopes, ions, and electron configuration. The document also covers average atomic mass and mass spectrometry. It concludes by discussing the Bohr model of the atom and how this helped explain emission spectra of elements. In summary, the key topics covered are the fundamental particles of atoms, atomic notation, isotopes, ions, electron configuration, and early atomic structure models.
2016 topic 0 - oxidation and reduction (INTRODUCTION)
The document discusses oxidation and reduction reactions. It defines oxidation as the loss of electrons or an increase in oxidation state, and reduction as the gain of electrons or a decrease in oxidation state. Redox reactions involve both oxidation and reduction occurring simultaneously. Oxidation states can be used to identify what is oxidized and reduced in a reaction. The document provides examples of calculating oxidation states in various compounds and ions using rules like the sum of oxidation states equaling the overall charge.
2016 topic 0 - elements & periodic table
- An element is a substance composed of a single type of atom that cannot be broken down further. A compound is a substance made of two or more elements chemically bonded together.
- Elements can exist as individual atoms, molecules of two bonded atoms, or giant molecular or network structures made of many bonded atoms like metals. Elements are categorized as metals, nonmetals, or metalloids based on their physical and chemical properties.
Introduction to elements & periodic table
- An element is a substance composed of a single type of atom that cannot be broken down further. A compound is a substance made of two or more elements chemically bonded together.
- Elements can exist as individual atoms, molecules of two bonded atoms, or giant molecular or network structures made of many bonded atoms like metals. Elements are categorized as metals, nonmetals, or metalloids based on their physical and chemical properties.
Physics ii djy 2013 ppt wave characteristics
This document discusses key characteristics and concepts related to waves, including:
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Topic 20 6 stereoisomers
This document provides an overview of organic chemistry topics related to stereoisomers, including:
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2) It discusses the importance of stereochemistry in fields like biochemistry, medicine, and studying reaction mechanisms.
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Topic 20 4 condensation reactions
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2016 topic 5.2 hess's law
- 1. Lesson Hess’s Law IB Chemistry Power Points Topic 05 Energetics www.pedagogics.ca
- 2. Great thanks to JONATHAN HOPTON & KNOCKHARDY PUBLISHING www.knockhardy.org.uk/sci.htm Some taken from ENTHALPY CHANGES
- 3. “The overall enthalpy change of a chemical process is independent of the path taken” The enthalpy change going from A to B can be found by adding the values of the enthalpy changes for the reactions A to X, X to Y and Y to B. ΔHr = ΔH1 + ΔH2 + ΔH3 HESS’S LAW
- 4. Dissolving solid sodium hydroxide in water This process produces sodium and hydroxide ions ie. NaOH (aq) solution. 1. NaOH(s) + H2O NaOH (aq) + H2O ΔH1 Consider three reactions
- 5. Reacting the sodium hydroxide solution with a hydrochloric acid solution = neutralization Na+ OH- 2. NaOH (aq) +HCl (aq) NaCl (aq) + H2O ΔH2
- 6. Alternatively - add solid sodium hydroxide directly to hydrochloric acid solution. H3O+ Cl- 3. NaOH(s) + HCl (aq) NaCl (aq) + H2O ΔH3
- 7. Recap: 1. NaOH(s) + H2O NaOH (aq) + H2O ΔH1 2. NaOH (aq) +HCl (aq) NaCl (aq) + H2O ΔH2 3. NaOH(s) + HCl (aq) NaCl (aq) + H2O ΔH3 Show that equation 1 plus equation 2 is the same as equation 3 What conclusion about enthalpy can be made?
- 8. Equation 1 + 2 1. NaOH(s) + H2O NaOH (aq) + H2O ΔH1 2. NaOH (aq) +HCl (aq) NaCl (aq) + H2O ΔH2 3. NaOH(s) + HCl (aq) NaCl (aq) + H2O ΔH3 Combined – equations 1 and 2 give equation 3 Since the equation 1 then 2 sequence starts and finishes with the same reactants and products as equation 3, Hess’s Law says ΔH3 = ΔH1 + ΔH2
- 9. Represented as an enthalpy level diagram NaOH (aq) +HCl (aq) ΔH3 NaOH (s) reactants + HCl (aq) products NaCl (aq) + H2O ΔH1 ΔH2 + H2O - 42 kJ/mol - 57 kJ/mol - 99 kJ/mol ΔH3 ΔH1 ΔH2
- 10. Represented as an enthalpy cycle + H2O NaOH (aq) ΔH3 NaOH (s) + HCl NaCl (aq) + H2O ΔH1 + HCl ΔH2