Thermodynamics-2.pptx
•Download as PPTX, PDF•
0 likes•4 views
This document contains questions about thermodynamics concepts such as entropy, Gibbs free energy, enthalpy of formation, and calculations involving heat, temperature, reactions, and phase changes. Specifically, it asks the reader to predict whether entropy increases or decreases in certain processes, calculate entropy changes, determine standard enthalpies of formation from reaction enthalpies, and find the temperature at which a reaction becomes spontaneous based on the standard entropy and enthalpy changes.
Report
Share
Report
Share
Recommended
#22 Key
1. An object can possess energy through kinetic energy from its motion or potential energy from its position. Kinetic energy depends on mass and velocity while potential energy depends on position.
2. A kilowatt-hour equals 3.6 million joules. An adult radiates heat at the same rate as a 100-watt bulb, so in 24 hours they radiate about 2.1 kilocalories of heat energy.
3. Chemical reactions that release heat are exothermic, while those that absorb heat are endothermic. Heat change equals internal energy change during constant pressure processes.
#22
1. An object can possess energy in two ways: potential energy due to position or configuration, and kinetic energy due to motion. Potential energy is stored energy due to factors like height or chemical composition, while kinetic energy is energy due to an object's motion.
2. A kilowatt-hour is equal to 3,600,000 joules. An adult radiates heat at about 100 watts, so in 24 hours would radiate 24,000 kcal of energy to the surroundings.
3. For the chemical reaction of silver ions and chloride ions forming silver chloride: a) the heat of reaction for 0.200 mol of AgCl forming is -13.12 kJ; b) the
8.0 thermochemistry (student's copy)
This document discusses thermo chemistry and key concepts like enthalpy, calorimetry, and Hess's law. It begins by defining open, closed, and isolated systems and explains endothermic and exothermic reactions using energy profile diagrams. It then discusses enthalpy and defines standard enthalpy. Various types of enthalpies are defined like enthalpy of formation, combustion, atomization, and more. Calorimetry is explained as a method to measure heat changes in reactions using calorimeters. Hess's law is introduced as the principle that the enthalpy change of a reaction is the same whether it occurs in one step or multiple steps.
Energetics
This document discusses various types of energetics in physical chemistry, including thermo chemistry concepts like standard enthalpy of combustion, standard enthalpy of formation, enthalpy of neutralization, atomization energy, sublimation energy, ionization energy, electron affinity, and lattice energy. It provides definitions and examples of each. Methods for calculating heat of formation from combustion data, bond energies, and other information are also described. Sample problems show how to use combustion data or bond energies to calculate enthalpy changes for chemical reactions.
Chapter 5 gen chem
This document discusses thermochemistry and energy changes in chemical reactions. It defines different types of energy, including kinetic energy, potential energy, and internal energy. The first law of thermodynamics states that energy is conserved in chemical reactions, with the change in internal energy of a system equaling the negative of the change in energy of the surroundings. Enthalpy is related to the internal energy and pressure-volume work term. Calorimetry experiments allow measurement of enthalpy changes using calorimeters and bomb calorimeters. Hess's law allows calculation of enthalpy changes from enthalpies of individual reaction steps. Fossil fuels are discussed as a non-renewable energy source.
2011 hr thermo study guide key
This document provides a study guide for thermochemistry with information in the following areas:
1. Key terms related to thermochemistry such as endothermic, exothermic, enthalpy, and entropy.
2. Equations to convert between energy units like calories, joules, and kilojoules.
3. Practice problems calculating things like specific heat, calorimetry, enthalpy of reaction, Hess' Law, heat of formation, and entropy.
4. Descriptions of molecular motion and order in different phases to explain how entropy changes with phase transitions.
Chemical Reactions: Thermochemistry
This document discusses various topics in thermochemistry including:
- Enthalpy changes in chemical reactions and how they are measured using calorimetry. Exothermic and endothermic reactions are explained.
- Hess's law, which states that the enthalpy change of a reaction is independent of the reaction pathway. It can be used to calculate enthalpy changes.
- Standard enthalpies of formation and how they allow calculation of enthalpy changes using Hess's law and bond dissociation enthalpies.
- Measuring enthalpy changes using bomb calorimetry and coffee cup calorimetry. Limitations of each method are discussed.
Chemistry zimsec chapter 6 chemical energetics
1) The document discusses chemical energetics, specifically enthalpy changes, standard enthalpy changes, and Hess' law.
2) It defines exothermic and endothermic reactions, and explains how to calculate enthalpy changes from experimental temperature change data using standard formulas.
3) Standard enthalpy changes are discussed for various types of reactions including formation, combustion, neutralization, and others. Hess' law is introduced which states that the total enthalpy change is independent of reaction path as long as initial and final states are the same.
Recommended
#22 Key
1. An object can possess energy through kinetic energy from its motion or potential energy from its position. Kinetic energy depends on mass and velocity while potential energy depends on position.
2. A kilowatt-hour equals 3.6 million joules. An adult radiates heat at the same rate as a 100-watt bulb, so in 24 hours they radiate about 2.1 kilocalories of heat energy.
3. Chemical reactions that release heat are exothermic, while those that absorb heat are endothermic. Heat change equals internal energy change during constant pressure processes.
#22
1. An object can possess energy in two ways: potential energy due to position or configuration, and kinetic energy due to motion. Potential energy is stored energy due to factors like height or chemical composition, while kinetic energy is energy due to an object's motion.
2. A kilowatt-hour is equal to 3,600,000 joules. An adult radiates heat at about 100 watts, so in 24 hours would radiate 24,000 kcal of energy to the surroundings.
3. For the chemical reaction of silver ions and chloride ions forming silver chloride: a) the heat of reaction for 0.200 mol of AgCl forming is -13.12 kJ; b) the
8.0 thermochemistry (student's copy)
This document discusses thermo chemistry and key concepts like enthalpy, calorimetry, and Hess's law. It begins by defining open, closed, and isolated systems and explains endothermic and exothermic reactions using energy profile diagrams. It then discusses enthalpy and defines standard enthalpy. Various types of enthalpies are defined like enthalpy of formation, combustion, atomization, and more. Calorimetry is explained as a method to measure heat changes in reactions using calorimeters. Hess's law is introduced as the principle that the enthalpy change of a reaction is the same whether it occurs in one step or multiple steps.
Energetics
This document discusses various types of energetics in physical chemistry, including thermo chemistry concepts like standard enthalpy of combustion, standard enthalpy of formation, enthalpy of neutralization, atomization energy, sublimation energy, ionization energy, electron affinity, and lattice energy. It provides definitions and examples of each. Methods for calculating heat of formation from combustion data, bond energies, and other information are also described. Sample problems show how to use combustion data or bond energies to calculate enthalpy changes for chemical reactions.
Chapter 5 gen chem
This document discusses thermochemistry and energy changes in chemical reactions. It defines different types of energy, including kinetic energy, potential energy, and internal energy. The first law of thermodynamics states that energy is conserved in chemical reactions, with the change in internal energy of a system equaling the negative of the change in energy of the surroundings. Enthalpy is related to the internal energy and pressure-volume work term. Calorimetry experiments allow measurement of enthalpy changes using calorimeters and bomb calorimeters. Hess's law allows calculation of enthalpy changes from enthalpies of individual reaction steps. Fossil fuels are discussed as a non-renewable energy source.
2011 hr thermo study guide key
This document provides a study guide for thermochemistry with information in the following areas:
1. Key terms related to thermochemistry such as endothermic, exothermic, enthalpy, and entropy.
2. Equations to convert between energy units like calories, joules, and kilojoules.
3. Practice problems calculating things like specific heat, calorimetry, enthalpy of reaction, Hess' Law, heat of formation, and entropy.
4. Descriptions of molecular motion and order in different phases to explain how entropy changes with phase transitions.
Chemical Reactions: Thermochemistry
This document discusses various topics in thermochemistry including:
- Enthalpy changes in chemical reactions and how they are measured using calorimetry. Exothermic and endothermic reactions are explained.
- Hess's law, which states that the enthalpy change of a reaction is independent of the reaction pathway. It can be used to calculate enthalpy changes.
- Standard enthalpies of formation and how they allow calculation of enthalpy changes using Hess's law and bond dissociation enthalpies.
- Measuring enthalpy changes using bomb calorimetry and coffee cup calorimetry. Limitations of each method are discussed.
Chemistry zimsec chapter 6 chemical energetics
1) The document discusses chemical energetics, specifically enthalpy changes, standard enthalpy changes, and Hess' law.
2) It defines exothermic and endothermic reactions, and explains how to calculate enthalpy changes from experimental temperature change data using standard formulas.
3) Standard enthalpy changes are discussed for various types of reactions including formation, combustion, neutralization, and others. Hess' law is introduced which states that the total enthalpy change is independent of reaction path as long as initial and final states are the same.
AP_Chem_Thermodynamics.pptx
Thermodynamics is the study of energy and its transformations. Thermochemistry is the subdiscipline involving chemical reactions and energy changes. The first law of thermodynamics states that energy is conserved as it transforms between forms. Energy exists in kinetic and potential forms. Kinetic energy is associated with motion, while potential energy is stored energy due to position or composition. Heat is the transfer of kinetic energy between objects of different temperatures until they reach equilibrium. Exothermic processes release heat from a system, while endothermic processes absorb heat into a system. Enthalpy changes (ΔH) quantify the heat absorbed or released by chemical reactions. Spontaneous processes are those that proceed without outside intervention, as dictated by a negative change
Thermochemistry
Thermochemistry is the study of energy changes that occur during chemical reactions and phase changes. Heat (q) is energy that transfers from one object to another due to a temperature difference. Exothermic processes release heat (negative q value), while endothermic processes absorb heat (positive q value). Enthalpy (H) is the heat content of a system at constant pressure, and enthalpy changes (ΔH) quantify the heat absorbed or released during chemical reactions. Thermochemical equations relate the enthalpy change to the heat of reaction. Calorimetry problems use these equations and concepts to calculate energy changes involved in physical and chemical processes.
C13 enthalpy change
This document discusses enthalpy changes and exothermic and endothermic reactions. It defines exothermic reactions as reactions where heat is given out to the surroundings, while endothermic reactions absorb heat from the surroundings. The amount of heat given out or absorbed during a reaction is called the enthalpy change. Whether a reaction is exothermic or endothermic depends on whether bond breaking absorbs more energy than bond forming releases, or vice versa.
Ch17 thermo review
This document contains a study guide for a chapter on thermochemistry with 23 questions covering topics like thermochemical equations, heat in changes of state, Hess's law, and standard enthalpies of formation. The questions involve performing calculations related to specific heat, heat of fusion/vaporization, and enthalpy changes. Key terms defined include calorie, heat, heat of vaporization, endothermic, heat capacity, Joule, exothermic, heat of fusion, kinetic energy, molar heat capacity, specific heat, potential energy, and temperature.
F y b. sc. ii. chemical energetics
Need of thermodynamics and the Laws of Thermodynamics.
Important principles and definitions of thermochemistry.
Concept of standard state and standard enthalpies of formations,
Integral and differential enthalpies of solution and dilution.
Calculation of bond energy, bond dissociation energy and resonance energy from thermochemical data.
Variation of enthalpy of a reaction with temperature – Kirchhoff’s equation.
Statement of Third Law of thermodynamics and calculation of absolute entropies of substances.
JFI -just for information
�_CHAPTER2_Physical chemistry_Premidical _Thermochemistry.pdf
1. The document is a chapter-by-chapter summary of General Physical Chemistry by Dr. Fateh Eltaboni.
2. Chapter 2 discusses thermochemistry and thermodynamics, including heat transfer, exothermic and endothermic processes, state functions, the first law of thermodynamics, and enthalpy.
3. Key concepts covered are heat, temperature, thermochemistry, systems, state functions, the relationship between work and energy, and calorimetry.
Chemistry- JIB Topic 9 Thermochemistry
The document defines key terms in thermodynamics including system, surroundings, open system, closed system, isolated system, exothermic, endothermic, enthalpy, kinetic energy, potential energy, heat, work, state functions, standard enthalpy of formation, standard enthalpy of combustion, and entropy. It also discusses the first and second laws of thermodynamics, Gibbs free energy, and how to calculate thermodynamic properties using standard enthalpies of formation.
thermodynamics numericals TSH .pptx
The document contains 13 problems related to thermodynamics concepts like heat, work, internal energy, enthalpy, free energy, and chemical equilibrium. The problems involve calculations using these concepts for systems involving gases, reactions, and phase changes. Thermodynamic properties like heat capacities, enthalpies, and free energies are provided to calculate unknown values like temperature changes, energies, and equilibrium constants.
Inorganic Chemistry: Thermochemistry
This document provides an introduction to thermochemistry and the key concepts of enthalpy, enthalpy change, and standard enthalpy of formation. It defines system and surroundings, and the three types of systems - open, closed, and isolated. The key points are:
- Enthalpy change (ΔH) is the difference in enthalpies between products and reactants and indicates whether a reaction is endothermic or exothermic.
- Standard enthalpy of formation (H°f) is the enthalpy change when 1 mole of a substance is formed from its elements under standard conditions.
- Enthalpy of combustion (H°c) is the enthalpy change when 1 mole
Lect w10 abbrev_ thermochemistry_alg
The document provides information about thermochemistry and how to calculate the change in enthalpy (ΔH) of chemical reactions using standard enthalpy values and bond energies. It discusses how ΔH is measured experimentally using calorimetry and how Hess's law allows calculating ΔH from multiple reaction steps. Standard enthalpy values and bond dissociation energies allow predicting if reactions are endothermic or exothermic without direct experimentation.
Causes of change
The document defines key thermodynamic terms like heat, work, internal energy, temperature, enthalpy, and heat capacity. It distinguishes between heat and temperature. It discusses specific heat and molar heat capacity, and provides values for common substances. It describes how to calculate heat transfer and enthalpy change using specific heat, molar heat capacity, and temperature change. Hess's law and standard enthalpies of formation are also explained for calculating enthalpy changes in chemical reactions.
Thermochemistry
Thermochemistry is the study of heat changes in chemical reactions. Thermal energy is the energy associated with the random motion of atoms and molecules. Enthalpy (H) is a state function that represents the total energy of a system at constant pressure. The standard enthalpy of formation (ΔHf°) is the change in enthalpy that accompanies the formation of one mole of a compound from its elements in their standard states. Hess's law states that the enthalpy change for a reaction is equal to the sum of the enthalpy changes of the steps in any possible pathway between the initial and final states of the reaction.
Ch6 Thermochemistry (old version)
Thermochemistry is the study of heat changes in chemical reactions. There are several types of energy including chemical, thermal, nuclear, and potential energy. Heat is the transfer of thermal energy between objects at different temperatures. Exothermic processes release heat to the surroundings while endothermic processes absorb heat from the surroundings. Enthalpy (H) quantifies the heat flow into or out of a system during chemical reactions at constant pressure. The standard enthalpy of formation (ΔH°f) is the heat change when one mole of a compound forms from its elements. Hess's law states that the enthalpy change is the same whether a reaction occurs in one step or multiple steps.
TOPIC 4 THERMOCHEMISTRY - Copy.pptx
This document discusses various types of thermochemistry and enthalpy changes in chemical reactions. It begins by defining exothermic and endothermic reactions, and describes how enthalpy (ΔH) is the heat released or absorbed during a reaction. It then explains how to calculate enthalpy changes using specific heat and temperature change. The main types of enthalpy covered are heat of precipitation, neutralization, displacement, and combustion. Examples are provided for calculating enthalpy changes using thermochemical equations and experimental temperature changes. In summary, the document provides an overview of thermochemistry concepts and calculations involving enthalpy for different reaction types.
Chapter 17.1 : Thermochemistry
The document discusses thermochemistry and concepts related to heat, temperature, enthalpy, and thermochemical equations. It provides definitions and examples of:
- Specific heat and how to calculate it using the formula q=m*c*ΔT
- Enthalpy change (ΔH), enthalpy of reaction, enthalpy of formation (ΔHf), and enthalpy of combustion (ΔHc)
- How to use Hess's law to calculate enthalpy changes from individual reaction steps
ch6.pptx
What constitutes waste depends on the eye of the beholder; one person's waste can be a resource for another person.[1] Though waste is a physical object, its generation is a physical and psychological process.[1] The definitions used by various agencies are as below.
United Nations Environment Program
According to the Basel Convention on the Control of Transboundary Movements of Hazardous Wastes and Their Disposal of 1989, Art. 2(1), "'Wastes' are substance or objects, which are disposed of or are intended to be disposed of or are required to be disposed of by the provisions of national law".[2]
United Nations Statistics Division
The UNSD Glossary of Environment Statistics[3] describes waste as "materials that are not prime products (that is, products produced for the market) for which the generator has no further use in terms of his/her own purposes of production, transformation or consumption, and of which he/she wants to dispose. Wastes may be generated during the extraction of raw materials, the processing of raw materials into intermediate and final products, the consumption of final products, and other human activities. Residuals recycled or reused at the place of generation are excluded."
European Union
Under the Waste Framework Directive 2008/98/EC, Art. 3(1), the European Union defines waste as "an object the holder discards, intends to discard or is required to discard."[4] For a more structural description of the Waste Directive, see the European Commission's summary.
Types of Waste
Municipal Waste
The Organization for Economic Co-operation and Development also known as OECD defines municipal solid waste (MSW) as “waste collected and treated by or for municipalities”. [5] Typically this type of waste includes household waste, commercial waste, and demolition or construction waste. In 2018, the Environmental Protection Agency concluded that 292.4 tons of municipal waste was generated which equated to about 4.9 pounds per day per person. Out of the 292.4 tons, approximately 69 million tons were recycled, and 25 million tons were composted. [6]
Household Waste and Commercial Waste
Household waste more commonly known as trash or garbage are items that are typically thrown away daily from ordinary households. Items often included in this category include product packaging, yard waste, clothing, food scraps, appliance, paints, and batteries.[7] Most of the items that are collected by municipalities end up in landfills across the world. In the United States, it is estimated that 11.3 million tons of textile waste is generated. On an individual level, it is estimated that the average American throws away 81.5 pounds of clothes each year.[8] As online shopping becomes more prevalent, items such as cardboard, bubble wrap, shipping envelopes are ending up in landfills across the United States. The EPA has estimated that approximately 10.1 million tons of plastic containers and packaging ended up landfills in 2018. The EPA noted that only 30.
Thermochemical equations
Thermochemical Equations presentation, Enthalpy change,
exothermic and endothermic chemical reactions.
Enthalpy change
The document discusses enthalpy change (ΔH) which is the amount of heat released or absorbed during a chemical reaction under constant pressure. ΔH is calculated as the enthalpy of products minus reactants. Standard enthalpy change (ΔH°) is measured under standard temperature and pressure conditions. Some key enthalpy terms discussed include standard enthalpy of formation (ΔHf°), enthalpy of combustion (ΔHc°), enthalpy of solution (ΔHsoln), and enthalpy of neutralization. Practice problems are provided to calculate enthalpy changes using experimental heat and temperature change data.
Ppt 13 R1.2 Energy cycles in reactions.pptx
the ppt is on energy cycles in reactions and deal with Hess's law of constant heat summation where the law of conservation of mass is obeyed. The enthalpy change can be calculated no matter whatever path the reaction has taken place as long as reactants and products are same the enthalpy change can be determined. Thus if enthalpy change of reaction is to be calculated than we can use enthalpy of combustion and formation to calculate it.
Ch6 Thermochemistry (updated)
Thermochemistry is the study of heat changes in chemical reactions. There are several types of energy including chemical, thermal, nuclear, and radiant energy. Heat is the transfer of thermal energy between objects at different temperatures. Thermochemistry examines heat absorbed or released by chemical reactions using concepts like exothermic, endothermic, enthalpy, and calorimetry. The first law of thermodynamics states that energy cannot be created or destroyed, only transferred between systems and their surroundings.
The use of Nauplii and metanauplii artemia in aquaculture (brine shrimp).pptx
Although Artemia has been known to man for centuries, its use as a food for the culture of larval organisms apparently began only in the 1930s, when several investigators found that it made an excellent food for newly hatched fish larvae (Litvinenko et al., 2023). As aquaculture developed in the 1960s and ‘70s, the use of Artemia also became more widespread, due both to its convenience and to its nutritional value for larval organisms (Arenas-Pardo et al., 2024). The fact that Artemia dormant cysts can be stored for long periods in cans, and then used as an off-the-shelf food requiring only 24 h of incubation makes them the most convenient, least labor-intensive, live food available for aquaculture (Sorgeloos & Roubach, 2021). The nutritional value of Artemia, especially for marine organisms, is not constant, but varies both geographically and temporally. During the last decade, however, both the causes of Artemia nutritional variability and methods to improve poorquality Artemia have been identified (Loufi et al., 2024).
Brine shrimp (Artemia spp.) are used in marine aquaculture worldwide. Annually, more than 2,000 metric tons of dry cysts are used for cultivation of fish, crustacean, and shellfish larva. Brine shrimp are important to aquaculture because newly hatched brine shrimp nauplii (larvae) provide a food source for many fish fry (Mozanzadeh et al., 2021). Culture and harvesting of brine shrimp eggs represents another aspect of the aquaculture industry. Nauplii and metanauplii of Artemia, commonly known as brine shrimp, play a crucial role in aquaculture due to their nutritional value and suitability as live feed for many aquatic species, particularly in larval stages (Sorgeloos & Roubach, 2021).
Unlocking the mysteries of reproduction: Exploring fecundity and gonadosomati...
The pygmy halfbeak Dermogenys colletei, is known for its viviparous nature, this presents an intriguing case of relatively low fecundity, raising questions about potential compensatory reproductive strategies employed by this species. Our study delves into the examination of fecundity and the Gonadosomatic Index (GSI) in the Pygmy Halfbeak, D. colletei (Meisner, 2001), an intriguing viviparous fish indigenous to Sarawak, Borneo. We hypothesize that the Pygmy halfbeak, D. colletei, may exhibit unique reproductive adaptations to offset its low fecundity, thus enhancing its survival and fitness. To address this, we conducted a comprehensive study utilizing 28 mature female specimens of D. colletei, carefully measuring fecundity and GSI to shed light on the reproductive adaptations of this species. Our findings reveal that D. colletei indeed exhibits low fecundity, with a mean of 16.76 ± 2.01, and a mean GSI of 12.83 ± 1.27, providing crucial insights into the reproductive mechanisms at play in this species. These results underscore the existence of unique reproductive strategies in D. colletei, enabling its adaptation and persistence in Borneo's diverse aquatic ecosystems, and call for further ecological research to elucidate these mechanisms. This study lends to a better understanding of viviparous fish in Borneo and contributes to the broader field of aquatic ecology, enhancing our knowledge of species adaptations to unique ecological challenges.
More Related Content
Similar to Thermodynamics-2.pptx
AP_Chem_Thermodynamics.pptx
Thermodynamics is the study of energy and its transformations. Thermochemistry is the subdiscipline involving chemical reactions and energy changes. The first law of thermodynamics states that energy is conserved as it transforms between forms. Energy exists in kinetic and potential forms. Kinetic energy is associated with motion, while potential energy is stored energy due to position or composition. Heat is the transfer of kinetic energy between objects of different temperatures until they reach equilibrium. Exothermic processes release heat from a system, while endothermic processes absorb heat into a system. Enthalpy changes (ΔH) quantify the heat absorbed or released by chemical reactions. Spontaneous processes are those that proceed without outside intervention, as dictated by a negative change
Thermochemistry
Thermochemistry is the study of energy changes that occur during chemical reactions and phase changes. Heat (q) is energy that transfers from one object to another due to a temperature difference. Exothermic processes release heat (negative q value), while endothermic processes absorb heat (positive q value). Enthalpy (H) is the heat content of a system at constant pressure, and enthalpy changes (ΔH) quantify the heat absorbed or released during chemical reactions. Thermochemical equations relate the enthalpy change to the heat of reaction. Calorimetry problems use these equations and concepts to calculate energy changes involved in physical and chemical processes.
C13 enthalpy change
This document discusses enthalpy changes and exothermic and endothermic reactions. It defines exothermic reactions as reactions where heat is given out to the surroundings, while endothermic reactions absorb heat from the surroundings. The amount of heat given out or absorbed during a reaction is called the enthalpy change. Whether a reaction is exothermic or endothermic depends on whether bond breaking absorbs more energy than bond forming releases, or vice versa.
Ch17 thermo review
This document contains a study guide for a chapter on thermochemistry with 23 questions covering topics like thermochemical equations, heat in changes of state, Hess's law, and standard enthalpies of formation. The questions involve performing calculations related to specific heat, heat of fusion/vaporization, and enthalpy changes. Key terms defined include calorie, heat, heat of vaporization, endothermic, heat capacity, Joule, exothermic, heat of fusion, kinetic energy, molar heat capacity, specific heat, potential energy, and temperature.
F y b. sc. ii. chemical energetics
Need of thermodynamics and the Laws of Thermodynamics.
Important principles and definitions of thermochemistry.
Concept of standard state and standard enthalpies of formations,
Integral and differential enthalpies of solution and dilution.
Calculation of bond energy, bond dissociation energy and resonance energy from thermochemical data.
Variation of enthalpy of a reaction with temperature – Kirchhoff’s equation.
Statement of Third Law of thermodynamics and calculation of absolute entropies of substances.
JFI -just for information
�_CHAPTER2_Physical chemistry_Premidical _Thermochemistry.pdf
1. The document is a chapter-by-chapter summary of General Physical Chemistry by Dr. Fateh Eltaboni.
2. Chapter 2 discusses thermochemistry and thermodynamics, including heat transfer, exothermic and endothermic processes, state functions, the first law of thermodynamics, and enthalpy.
3. Key concepts covered are heat, temperature, thermochemistry, systems, state functions, the relationship between work and energy, and calorimetry.
Chemistry- JIB Topic 9 Thermochemistry
The document defines key terms in thermodynamics including system, surroundings, open system, closed system, isolated system, exothermic, endothermic, enthalpy, kinetic energy, potential energy, heat, work, state functions, standard enthalpy of formation, standard enthalpy of combustion, and entropy. It also discusses the first and second laws of thermodynamics, Gibbs free energy, and how to calculate thermodynamic properties using standard enthalpies of formation.
thermodynamics numericals TSH .pptx
The document contains 13 problems related to thermodynamics concepts like heat, work, internal energy, enthalpy, free energy, and chemical equilibrium. The problems involve calculations using these concepts for systems involving gases, reactions, and phase changes. Thermodynamic properties like heat capacities, enthalpies, and free energies are provided to calculate unknown values like temperature changes, energies, and equilibrium constants.
Inorganic Chemistry: Thermochemistry
This document provides an introduction to thermochemistry and the key concepts of enthalpy, enthalpy change, and standard enthalpy of formation. It defines system and surroundings, and the three types of systems - open, closed, and isolated. The key points are:
- Enthalpy change (ΔH) is the difference in enthalpies between products and reactants and indicates whether a reaction is endothermic or exothermic.
- Standard enthalpy of formation (H°f) is the enthalpy change when 1 mole of a substance is formed from its elements under standard conditions.
- Enthalpy of combustion (H°c) is the enthalpy change when 1 mole
Lect w10 abbrev_ thermochemistry_alg
The document provides information about thermochemistry and how to calculate the change in enthalpy (ΔH) of chemical reactions using standard enthalpy values and bond energies. It discusses how ΔH is measured experimentally using calorimetry and how Hess's law allows calculating ΔH from multiple reaction steps. Standard enthalpy values and bond dissociation energies allow predicting if reactions are endothermic or exothermic without direct experimentation.
Causes of change
The document defines key thermodynamic terms like heat, work, internal energy, temperature, enthalpy, and heat capacity. It distinguishes between heat and temperature. It discusses specific heat and molar heat capacity, and provides values for common substances. It describes how to calculate heat transfer and enthalpy change using specific heat, molar heat capacity, and temperature change. Hess's law and standard enthalpies of formation are also explained for calculating enthalpy changes in chemical reactions.
Thermochemistry
Thermochemistry is the study of heat changes in chemical reactions. Thermal energy is the energy associated with the random motion of atoms and molecules. Enthalpy (H) is a state function that represents the total energy of a system at constant pressure. The standard enthalpy of formation (ΔHf°) is the change in enthalpy that accompanies the formation of one mole of a compound from its elements in their standard states. Hess's law states that the enthalpy change for a reaction is equal to the sum of the enthalpy changes of the steps in any possible pathway between the initial and final states of the reaction.
Ch6 Thermochemistry (old version)
Thermochemistry is the study of heat changes in chemical reactions. There are several types of energy including chemical, thermal, nuclear, and potential energy. Heat is the transfer of thermal energy between objects at different temperatures. Exothermic processes release heat to the surroundings while endothermic processes absorb heat from the surroundings. Enthalpy (H) quantifies the heat flow into or out of a system during chemical reactions at constant pressure. The standard enthalpy of formation (ΔH°f) is the heat change when one mole of a compound forms from its elements. Hess's law states that the enthalpy change is the same whether a reaction occurs in one step or multiple steps.
TOPIC 4 THERMOCHEMISTRY - Copy.pptx
This document discusses various types of thermochemistry and enthalpy changes in chemical reactions. It begins by defining exothermic and endothermic reactions, and describes how enthalpy (ΔH) is the heat released or absorbed during a reaction. It then explains how to calculate enthalpy changes using specific heat and temperature change. The main types of enthalpy covered are heat of precipitation, neutralization, displacement, and combustion. Examples are provided for calculating enthalpy changes using thermochemical equations and experimental temperature changes. In summary, the document provides an overview of thermochemistry concepts and calculations involving enthalpy for different reaction types.
Chapter 17.1 : Thermochemistry
The document discusses thermochemistry and concepts related to heat, temperature, enthalpy, and thermochemical equations. It provides definitions and examples of:
- Specific heat and how to calculate it using the formula q=m*c*ΔT
- Enthalpy change (ΔH), enthalpy of reaction, enthalpy of formation (ΔHf), and enthalpy of combustion (ΔHc)
- How to use Hess's law to calculate enthalpy changes from individual reaction steps
ch6.pptx
What constitutes waste depends on the eye of the beholder; one person's waste can be a resource for another person.[1] Though waste is a physical object, its generation is a physical and psychological process.[1] The definitions used by various agencies are as below.
United Nations Environment Program
According to the Basel Convention on the Control of Transboundary Movements of Hazardous Wastes and Their Disposal of 1989, Art. 2(1), "'Wastes' are substance or objects, which are disposed of or are intended to be disposed of or are required to be disposed of by the provisions of national law".[2]
United Nations Statistics Division
The UNSD Glossary of Environment Statistics[3] describes waste as "materials that are not prime products (that is, products produced for the market) for which the generator has no further use in terms of his/her own purposes of production, transformation or consumption, and of which he/she wants to dispose. Wastes may be generated during the extraction of raw materials, the processing of raw materials into intermediate and final products, the consumption of final products, and other human activities. Residuals recycled or reused at the place of generation are excluded."
European Union
Under the Waste Framework Directive 2008/98/EC, Art. 3(1), the European Union defines waste as "an object the holder discards, intends to discard or is required to discard."[4] For a more structural description of the Waste Directive, see the European Commission's summary.
Types of Waste
Municipal Waste
The Organization for Economic Co-operation and Development also known as OECD defines municipal solid waste (MSW) as “waste collected and treated by or for municipalities”. [5] Typically this type of waste includes household waste, commercial waste, and demolition or construction waste. In 2018, the Environmental Protection Agency concluded that 292.4 tons of municipal waste was generated which equated to about 4.9 pounds per day per person. Out of the 292.4 tons, approximately 69 million tons were recycled, and 25 million tons were composted. [6]
Household Waste and Commercial Waste
Household waste more commonly known as trash or garbage are items that are typically thrown away daily from ordinary households. Items often included in this category include product packaging, yard waste, clothing, food scraps, appliance, paints, and batteries.[7] Most of the items that are collected by municipalities end up in landfills across the world. In the United States, it is estimated that 11.3 million tons of textile waste is generated. On an individual level, it is estimated that the average American throws away 81.5 pounds of clothes each year.[8] As online shopping becomes more prevalent, items such as cardboard, bubble wrap, shipping envelopes are ending up in landfills across the United States. The EPA has estimated that approximately 10.1 million tons of plastic containers and packaging ended up landfills in 2018. The EPA noted that only 30.
Thermochemical equations
Thermochemical Equations presentation, Enthalpy change,
exothermic and endothermic chemical reactions.
Enthalpy change
The document discusses enthalpy change (ΔH) which is the amount of heat released or absorbed during a chemical reaction under constant pressure. ΔH is calculated as the enthalpy of products minus reactants. Standard enthalpy change (ΔH°) is measured under standard temperature and pressure conditions. Some key enthalpy terms discussed include standard enthalpy of formation (ΔHf°), enthalpy of combustion (ΔHc°), enthalpy of solution (ΔHsoln), and enthalpy of neutralization. Practice problems are provided to calculate enthalpy changes using experimental heat and temperature change data.
Ppt 13 R1.2 Energy cycles in reactions.pptx
the ppt is on energy cycles in reactions and deal with Hess's law of constant heat summation where the law of conservation of mass is obeyed. The enthalpy change can be calculated no matter whatever path the reaction has taken place as long as reactants and products are same the enthalpy change can be determined. Thus if enthalpy change of reaction is to be calculated than we can use enthalpy of combustion and formation to calculate it.
Ch6 Thermochemistry (updated)
Thermochemistry is the study of heat changes in chemical reactions. There are several types of energy including chemical, thermal, nuclear, and radiant energy. Heat is the transfer of thermal energy between objects at different temperatures. Thermochemistry examines heat absorbed or released by chemical reactions using concepts like exothermic, endothermic, enthalpy, and calorimetry. The first law of thermodynamics states that energy cannot be created or destroyed, only transferred between systems and their surroundings.
Similar to Thermodynamics-2.pptx (20)
�_CHAPTER2_Physical chemistry_Premidical _Thermochemistry.pdf
�_CHAPTER2_Physical chemistry_Premidical _Thermochemistry.pdf
Recently uploaded
The use of Nauplii and metanauplii artemia in aquaculture (brine shrimp).pptx
Although Artemia has been known to man for centuries, its use as a food for the culture of larval organisms apparently began only in the 1930s, when several investigators found that it made an excellent food for newly hatched fish larvae (Litvinenko et al., 2023). As aquaculture developed in the 1960s and ‘70s, the use of Artemia also became more widespread, due both to its convenience and to its nutritional value for larval organisms (Arenas-Pardo et al., 2024). The fact that Artemia dormant cysts can be stored for long periods in cans, and then used as an off-the-shelf food requiring only 24 h of incubation makes them the most convenient, least labor-intensive, live food available for aquaculture (Sorgeloos & Roubach, 2021). The nutritional value of Artemia, especially for marine organisms, is not constant, but varies both geographically and temporally. During the last decade, however, both the causes of Artemia nutritional variability and methods to improve poorquality Artemia have been identified (Loufi et al., 2024).
Brine shrimp (Artemia spp.) are used in marine aquaculture worldwide. Annually, more than 2,000 metric tons of dry cysts are used for cultivation of fish, crustacean, and shellfish larva. Brine shrimp are important to aquaculture because newly hatched brine shrimp nauplii (larvae) provide a food source for many fish fry (Mozanzadeh et al., 2021). Culture and harvesting of brine shrimp eggs represents another aspect of the aquaculture industry. Nauplii and metanauplii of Artemia, commonly known as brine shrimp, play a crucial role in aquaculture due to their nutritional value and suitability as live feed for many aquatic species, particularly in larval stages (Sorgeloos & Roubach, 2021).
Unlocking the mysteries of reproduction: Exploring fecundity and gonadosomati...
The pygmy halfbeak Dermogenys colletei, is known for its viviparous nature, this presents an intriguing case of relatively low fecundity, raising questions about potential compensatory reproductive strategies employed by this species. Our study delves into the examination of fecundity and the Gonadosomatic Index (GSI) in the Pygmy Halfbeak, D. colletei (Meisner, 2001), an intriguing viviparous fish indigenous to Sarawak, Borneo. We hypothesize that the Pygmy halfbeak, D. colletei, may exhibit unique reproductive adaptations to offset its low fecundity, thus enhancing its survival and fitness. To address this, we conducted a comprehensive study utilizing 28 mature female specimens of D. colletei, carefully measuring fecundity and GSI to shed light on the reproductive adaptations of this species. Our findings reveal that D. colletei indeed exhibits low fecundity, with a mean of 16.76 ± 2.01, and a mean GSI of 12.83 ± 1.27, providing crucial insights into the reproductive mechanisms at play in this species. These results underscore the existence of unique reproductive strategies in D. colletei, enabling its adaptation and persistence in Borneo's diverse aquatic ecosystems, and call for further ecological research to elucidate these mechanisms. This study lends to a better understanding of viviparous fish in Borneo and contributes to the broader field of aquatic ecology, enhancing our knowledge of species adaptations to unique ecological challenges.
在线办理(salfor毕业证书)索尔福德大学毕业证毕业完成信一模一样
学校原件一模一样【微信：741003700 】《(salfor毕业证书)索尔福德大学毕业证》【微信：741003700 】学位证，留信认证（真实可查，永久存档）原件一模一样纸张工艺/offer、雅思、外壳等材料/诚信可靠,可直接看成品样本，帮您解决无法毕业带来的各种难题！外壳，原版制作，诚信可靠，可直接看成品样本。行业标杆！精益求精，诚心合作，真诚制作！多年品质 ,按需精细制作，24小时接单,全套进口原装设备。十五年致力于帮助留学生解决难题，包您满意。
本公司拥有海外各大学样板无数，能完美还原。
1:1完美还原海外各大学毕业材料上的工艺：水印，阴影底纹，钢印LOGO烫金烫银，LOGO烫金烫银复合重叠。文字图案浮雕、激光镭射、紫外荧光、温感、复印防伪等防伪工艺。材料咨询办理、认证咨询办理请加学历顾问Q/微741003700
【主营项目】
一.毕业证【q微741003700】成绩单、使馆认证、教育部认证、雅思托福成绩单、学生卡等！
二.真实使馆公证(即留学回国人员证明,不成功不收费)
三.真实教育部学历学位认证（教育部存档！教育部留服网站永久可查）
四.办理各国各大学文凭(一对一专业服务,可全程监控跟踪进度)
如果您处于以下几种情况：
◇在校期间，因各种原因未能顺利毕业……拿不到官方毕业证【q/微741003700】
◇面对父母的压力，希望尽快拿到；
◇不清楚认证流程以及材料该如何准备；
◇回国时间很长，忘记办理；
◇回国马上就要找工作，办给用人单位看；
◇企事业单位必须要求办理的
◇需要报考公务员、购买免税车、落转户口
◇申请留学生创业基金
留信网认证的作用:
1:该专业认证可证明留学生真实身份
2:同时对留学生所学专业登记给予评定
3:国家专业人才认证中心颁发入库证书
4:这个认证书并且可以归档倒地方
5:凡事获得留信网入网的信息将会逐步更新到个人身份内，将在公安局网内查询个人身份证信息后，同步读取人才网入库信息
6:个人职称评审加20分
7:个人信誉贷款加10分
8:在国家人才网主办的国家网络招聘大会中纳入资料，供国家高端企业选择人才
Remote Sensing and Computational, Evolutionary, Supercomputing, and Intellige...
Remote Sensing and Computational, Evolutionary, Supercomputing, and Intellige...University of Maribor
Slides from talk:
Aleš Zamuda: Remote Sensing and Computational, Evolutionary, Supercomputing, and Intelligent Systems.
11th International Conference on Electrical, Electronics and Computer Engineering (IcETRAN), Niš, 3-6 June 2024
Inter-Society Networking Panel GRSS/MTT-S/CIS Panel Session: Promoting Connection and Cooperation
https://www.etran.rs/2024/en/home-english/Compexometric titration/Chelatorphy titration/chelating titration
Classification
Metal ion ion indicators
Masking and demasking reagents
Estimation of Magnisium sulphate
Calcium gluconate
Complexometric Titration/ chelatometry titration/chelating titration, introduction, Types-
1.Direct Titration
2.Back Titration
3.Replacement Titration
4.Indirect Titration
Masking agent, Demasking agents
formation of complex
comparition between masking and demasking agents,
Indicators/Metal ion indicators/ Metallochromic indicators/pM indicators,
Visual Technique,PM indicators (metallochromic), Indicators of pH, Redox Indicators
Instrumental Techniques-Photometry
Potentiometry
Miscellaneous methods.
Complex titration with EDTA.
ESR spectroscopy in liquid food and beverages.pptx
With increasing population, people need to rely on packaged food stuffs. Packaging of food materials requires the preservation of food. There are various methods for the treatment of food to preserve them and irradiation treatment of food is one of them. It is the most common and the most harmless method for the food preservation as it does not alter the necessary micronutrients of food materials. Although irradiated food doesn’t cause any harm to the human health but still the quality assessment of food is required to provide consumers with necessary information about the food. ESR spectroscopy is the most sophisticated way to investigate the quality of the food and the free radicals induced during the processing of the food. ESR spin trapping technique is useful for the detection of highly unstable radicals in the food. The antioxidant capability of liquid food and beverages in mainly performed by spin trapping technique.
Thornton ESPP slides UK WW Network 4_6_24.pdf
ESPP presentation to EU Waste Water Network, 4th June 2024 “EU policies driving nutrient removal and recycling
and the revised UWWTD (Urban Waste Water Treatment Directive)”
The binding of cosmological structures by massless topological defects
Assuming spherical symmetry and weak field, it is shown that if one solves the Poisson equation or the Einstein field
equations sourced by a topological defect, i.e. a singularity of a very specific form, the result is a localized gravitational
field capable of driving flat rotation (i.e. Keplerian circular orbits at a constant speed for all radii) of test masses on a thin
spherical shell without any underlying mass. Moreover, a large-scale structure which exploits this solution by assembling
concentrically a number of such topological defects can establish a flat stellar or galactic rotation curve, and can also deflect
light in the same manner as an equipotential (isothermal) sphere. Thus, the need for dark matter or modified gravity theory is
mitigated, at least in part.
Describing and Interpreting an Immersive Learning Case with the Immersion Cub...
Current descriptions of immersive learning cases are often difficult or impossible to compare. This is due to a myriad of different options on what details to include, which aspects are relevant, and on the descriptive approaches employed. Also, these aspects often combine very specific details with more general guidelines or indicate intents and rationales without clarifying their implementation. In this paper we provide a method to describe immersive learning cases that is structured to enable comparisons, yet flexible enough to allow researchers and practitioners to decide which aspects to include. This method leverages a taxonomy that classifies educational aspects at three levels (uses, practices, and strategies) and then utilizes two frameworks, the Immersive Learning Brain and the Immersion Cube, to enable a structured description and interpretation of immersive learning cases. The method is then demonstrated on a published immersive learning case on training for wind turbine maintenance using virtual reality. Applying the method results in a structured artifact, the Immersive Learning Case Sheet, that tags the case with its proximal uses, practices, and strategies, and refines the free text case description to ensure that matching details are included. This contribution is thus a case description method in support of future comparative research of immersive learning cases. We then discuss how the resulting description and interpretation can be leveraged to change immersion learning cases, by enriching them (considering low-effort changes or additions) or innovating (exploring more challenging avenues of transformation). The method holds significant promise to support better-grounded research in immersive learning.
如何办理(uvic毕业证书)维多利亚大学毕业证本科学位证书原版一模一样
原版纸张【微信：741003700 】【(uvic毕业证书)维多利亚大学毕业证】【微信：741003700 】学位证，留信认证（真实可查，永久存档）offer、雅思、外壳等材料/诚信可靠,可直接看成品样本，帮您解决无法毕业带来的各种难题！外壳，原版制作，诚信可靠，可直接看成品样本。行业标杆！精益求精，诚心合作，真诚制作！多年品质 ,按需精细制作，24小时接单,全套进口原装设备。十五年致力于帮助留学生解决难题，包您满意。
本公司拥有海外各大学样板无数，能完美还原海外各大学 Bachelor Diploma degree, Master Degree Diploma
1:1完美还原海外各大学毕业材料上的工艺：水印，阴影底纹，钢印LOGO烫金烫银，LOGO烫金烫银复合重叠。文字图案浮雕、激光镭射、紫外荧光、温感、复印防伪等防伪工艺。材料咨询办理、认证咨询办理请加学历顾问Q/微741003700
留信网认证的作用:
1:该专业认证可证明留学生真实身份
2:同时对留学生所学专业登记给予评定
3:国家专业人才认证中心颁发入库证书
4:这个认证书并且可以归档倒地方
5:凡事获得留信网入网的信息将会逐步更新到个人身份内，将在公安局网内查询个人身份证信息后，同步读取人才网入库信息
6:个人职称评审加20分
7:个人信誉贷款加10分
8:在国家人才网主办的国家网络招聘大会中纳入资料，供国家高端企业选择人才
Sharlene Leurig - Enabling Onsite Water Use with Net Zero Water
Sharlene Leurig - Enabling Onsite Water Use with Net Zero WaterTexas Alliance of Groundwater Districts
Presented at June 6-7 Texas Alliance of Groundwater Districts Business Meeting20240520 Planning a Circuit Simulator in JavaScript.pptx
Evaporation step counter work. I have done a physical experiment.
(Work in progress.)
Randomised Optimisation Algorithms in DAPHNE
Slides from talk:
Aleš Zamuda: Randomised Optimisation Algorithms in DAPHNE .
Austrian-Slovenian HPC Meeting 2024 – ASHPC24, Seeblickhotel Grundlsee in Austria, 10–13 June 2024
https://ashpc.eu/
Cytokines and their role in immune regulation.pptx
This presentation covers the content and information on "Cytokines " and their role in immune regulation .
8.Isolation of pure cultures and preservation of cultures.pdf
Isolation of pure culture, its various method.
Applied Science: Thermodynamics, Laws & Methodology.pdf
When I was asked to give a companion lecture in support of ‘The Philosophy of Science’ (https://shorturl.at/4pUXz) I decided not to walk through the detail of the many methodologies in order of use. Instead, I chose to employ a long standing, and ongoing, scientific development as an exemplar. And so, I chose the ever evolving story of Thermodynamics as a scientific investigation at its best.
Conducted over a period of >200 years, Thermodynamics R&D, and application, benefitted from the highest levels of professionalism, collaboration, and technical thoroughness. New layers of application, methodology, and practice were made possible by the progressive advance of technology. In turn, this has seen measurement and modelling accuracy continually improved at a micro and macro level.
Perhaps most importantly, Thermodynamics rapidly became a primary tool in the advance of applied science/engineering/technology, spanning micro-tech, to aerospace and cosmology. I can think of no better a story to illustrate the breadth of scientific methodologies and applications at their best.
Recently uploaded (20)
The use of Nauplii and metanauplii artemia in aquaculture (brine shrimp).pptx
The use of Nauplii and metanauplii artemia in aquaculture (brine shrimp).pptx
Unlocking the mysteries of reproduction: Exploring fecundity and gonadosomati...
Unlocking the mysteries of reproduction: Exploring fecundity and gonadosomati...
Remote Sensing and Computational, Evolutionary, Supercomputing, and Intellige...
Remote Sensing and Computational, Evolutionary, Supercomputing, and Intellige...
Compexometric titration/Chelatorphy titration/chelating titration
Compexometric titration/Chelatorphy titration/chelating titration
ESR spectroscopy in liquid food and beverages.pptx
ESR spectroscopy in liquid food and beverages.pptx
The binding of cosmological structures by massless topological defects
The binding of cosmological structures by massless topological defects
Describing and Interpreting an Immersive Learning Case with the Immersion Cub...
Describing and Interpreting an Immersive Learning Case with the Immersion Cub...
Sharlene Leurig - Enabling Onsite Water Use with Net Zero Water
Sharlene Leurig - Enabling Onsite Water Use with Net Zero Water
20240520 Planning a Circuit Simulator in JavaScript.pptx
20240520 Planning a Circuit Simulator in JavaScript.pptx
Cytokines and their role in immune regulation.pptx
Cytokines and their role in immune regulation.pptx
8.Isolation of pure cultures and preservation of cultures.pdf
8.Isolation of pure cultures and preservation of cultures.pdf
Applied Science: Thermodynamics, Laws & Methodology.pdf
Applied Science: Thermodynamics, Laws & Methodology.pdf
Thermodynamics-2.pptx
- 1. 1 Learn Practically Learn Practically Learn Practically THERMODYNAMICS-2
- 2. 2 Learn Practically Learn Practically Learn Practically
- 3. 3 Learn Practically Learn Practically Learn Practically Learn Practically Entropy :
- 4. 4 Learn Practically Learn Practically Learn Practically Learn Practically Predict in which of the following, entropy increases/decreases : (i) A liquid crystallizes into a solid. (ii) Temperature of a crystalline solid is from 0 K to 115 K. iii) H2(g) → 2H(g)
- 5. 5 Learn Practically Learn Practically Learn Practically Learn Practically Calculate the entropy change in surroundings when 1.00 mol of H2O(l) is formed under standard conditions. ∆f H = –286 kJ mol–1.
- 6. 6 Learn Practically Learn Practically Learn Practically Learn Practically
- 7. 7 Learn Practically Learn Practically Learn Practically Learn Practically Gibb’s Free Energy :
- 8. 8 Learn Practically Learn Practically Learn Practically Learn Practically
- 9. 9 Learn Practically Learn Practically Learn Practically Learn Practically Given N2(g) + 3H2(g) → 2NH3(g) ; ∆rH = –92.4 kJ mol–1 What is the standard enthalpy of formation of NH3 gas?
- 10. 10 Learn Practically Learn Practically Learn Practically Learn Practically If water vapour is assumed to be a perfect gas, molar enthalpy change for vapourisation of 1 mol of water at 1bar and 100°C is 41kJ mol–1. Calculate the internal energy change, when 1 mol of water is vapourised at 1 bar pressure and 100°C.
- 11. 11 Learn Practically Learn Practically Learn Practically Learn Practically 11
- 12. 12 Learn Practically Learn Practically Learn Practically Learn Practically A swimmer coming out from a pool is covered with a film of water weighing about 18g. How much heat must be supplied to evaporate this water at 298 K ? Calculate the internal energy of vaporisation at 298K. ∆vap H for water at 298K= 44.01kJ mol–1
- 13. 13 Learn Practically Learn Practically Learn Practically Learn Practically 13
- 14. 14 Learn Practically Learn Practically Learn Practically Learn Practically The enthalpy of combustion of methane, graphite and dihydrogen at 298 K are, –890.3 kJ mol–1 –393.5 kJ mol–1, and –285.8 kJ mol–1 respectively. Enthalpy of formation of CH4(g) will be
- 15. 15 Learn Practically Learn Practically Learn Practically Learn Practically 15
- 16. 16 Learn Practically Learn Practically Learn Practically Learn Practically 16
- 17. 17 Learn Practically Learn Practically Learn Practically Learn Practically For the reaction at 298 K, 2A + B → C ∆H = 400 kJ mol–1 and ∆S = 0.2 kJ K–1 mol–1 At what temperature will the reaction become spontaneous considering ∆H and ∆S to be constant over the temperature range.
- 18. 18 Learn Practically Learn Practically Learn Practically Learn Practically 18
- 19. 19 Learn Practically Learn Practically Learn Practically
- 20. 20 Learn Practically Learn Practically 20 Learn Practically Previous Lecture Next Lecture