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Sodium hydroxide
Sodium hydroxide is manufactured through the Kellner-Solvay process and Castner-Kellner cell process. In the Kellner-Solvay process, brine is electrolyzed between a mercury cathode and graphite anode, producing sodium amalgam at the cathode which is later treated with water to produce sodium hydroxide and regenerate the mercury. In the Castner-Kellner cell process, a vessel is divided into compartments where sodium ions are reduced at the mercury cathode to form sodium amalgam, which then reacts with hydroxyl ions in another compartment to form sodium hydroxide. Sodium hydroxide is a white, highly alkaline and water-soluble solid with various industrial and laboratory uses such
Iron
There are three main varieties of iron based on carbon content: cast iron contains 2-5% carbon and is the impure form used to make steel and wrought iron; wrought iron contains 0.12-0.25% carbon and is the purest form used for chains and magnet cores; steel contains 0.1-1.5% carbon and has properties dependent on carbon content, used for many applications. Rusting of iron occurs via an electrochemical process where iron acts as the anode, releasing electrons and ferrous ions while hydrogen ions are reduced to hydrogen gas at cathode sites on the metal surface. The ferrous ions further oxidize to ferric oxide which absorbs moisture from the
Periodicity
The document discusses periodicity and how properties vary across periods and down groups in the periodic table. It specifically focuses on Period 3 elements (Na to Ar). Key points:
1) Atomic radius decreases across Period 3 as nuclear charge increases, attracting electrons more strongly. Radius increases down groups as atomic size increases.
2) Ionization energy generally increases across Period 3 as nuclear charge increases, requiring more energy to remove electrons. It decreases down groups as distance from nucleus increases.
3) Melting/boiling points are highest for metals/covalent networks and lower for weak molecular bonds. Electrical conductivity is highest for metals and lowest for nonmetals.
Thermodynamics ii
This document discusses spontaneous processes and the driving forces behind them in thermodynamics. It explains that spontaneous processes are driven by a decrease in enthalpy or an increase in entropy. While enthalpy change alone cannot predict spontaneity, the introduction of entropy and Gibbs free energy allows better determination of spontaneous processes. The document also discusses how temperature, entropy change, and the relationship between Gibbs free energy and equilibrium constant can be used to analyze spontaneity.
Thermodynamics ii
1. A spontaneous process is one that occurs without external influence, driven by a decrease in energy or increase in disorder.
2. Enthalpy change alone does not determine spontaneity, as some endothermic reactions are spontaneous. Entropy must also be considered.
3. Entropy is a measure of disorder - solids have lowest entropy and gases highest. Spontaneous processes favor higher entropy states.
4. The second law of thermodynamics states that the entropy of the universe always increases for spontaneous processes, with ∆Suniverse > 0.
As rate
1. The document discusses factors that affect the rate of chemical reactions, including surface area, concentration, pressure, temperature, and catalysis.
2. Catalysts work by lowering the activation energy of reactions, increasing the proportion of particles with energy exceeding this barrier.
3. Enzymes are biological catalysts that are highly specific and function via a lock-and-key mechanism to catalyze reactions in living organisms.
Air pollution
The document discusses various sources and effects of air pollution. It describes how burning fossil fuels from industries, automobiles, and power plants releases pollutants like carbon monoxide, sulfur dioxide, and nitrogen oxides into the air. This leads to issues like acid rain, photochemical smog, and global warming. Air pollution damages the environment, climate, plants, animals, and human health, causing problems like acidification of soils and water sources, reduced visibility, and respiratory illnesses. The text provides details on the formation and harmful impacts of acid rain and photochemical smog. Overall, the document analyzes the causes and wide-ranging consequences of air pollution from various human and industrial activities.
Recommandé
Sodium hydroxide
Sodium hydroxide is manufactured through the Kellner-Solvay process and Castner-Kellner cell process. In the Kellner-Solvay process, brine is electrolyzed between a mercury cathode and graphite anode, producing sodium amalgam at the cathode which is later treated with water to produce sodium hydroxide and regenerate the mercury. In the Castner-Kellner cell process, a vessel is divided into compartments where sodium ions are reduced at the mercury cathode to form sodium amalgam, which then reacts with hydroxyl ions in another compartment to form sodium hydroxide. Sodium hydroxide is a white, highly alkaline and water-soluble solid with various industrial and laboratory uses such
Iron
There are three main varieties of iron based on carbon content: cast iron contains 2-5% carbon and is the impure form used to make steel and wrought iron; wrought iron contains 0.12-0.25% carbon and is the purest form used for chains and magnet cores; steel contains 0.1-1.5% carbon and has properties dependent on carbon content, used for many applications. Rusting of iron occurs via an electrochemical process where iron acts as the anode, releasing electrons and ferrous ions while hydrogen ions are reduced to hydrogen gas at cathode sites on the metal surface. The ferrous ions further oxidize to ferric oxide which absorbs moisture from the
Periodicity
The document discusses periodicity and how properties vary across periods and down groups in the periodic table. It specifically focuses on Period 3 elements (Na to Ar). Key points:
1) Atomic radius decreases across Period 3 as nuclear charge increases, attracting electrons more strongly. Radius increases down groups as atomic size increases.
2) Ionization energy generally increases across Period 3 as nuclear charge increases, requiring more energy to remove electrons. It decreases down groups as distance from nucleus increases.
3) Melting/boiling points are highest for metals/covalent networks and lower for weak molecular bonds. Electrical conductivity is highest for metals and lowest for nonmetals.
Thermodynamics ii
This document discusses spontaneous processes and the driving forces behind them in thermodynamics. It explains that spontaneous processes are driven by a decrease in enthalpy or an increase in entropy. While enthalpy change alone cannot predict spontaneity, the introduction of entropy and Gibbs free energy allows better determination of spontaneous processes. The document also discusses how temperature, entropy change, and the relationship between Gibbs free energy and equilibrium constant can be used to analyze spontaneity.
Thermodynamics ii
1. A spontaneous process is one that occurs without external influence, driven by a decrease in energy or increase in disorder.
2. Enthalpy change alone does not determine spontaneity, as some endothermic reactions are spontaneous. Entropy must also be considered.
3. Entropy is a measure of disorder - solids have lowest entropy and gases highest. Spontaneous processes favor higher entropy states.
4. The second law of thermodynamics states that the entropy of the universe always increases for spontaneous processes, with ∆Suniverse > 0.
As rate
1. The document discusses factors that affect the rate of chemical reactions, including surface area, concentration, pressure, temperature, and catalysis.
2. Catalysts work by lowering the activation energy of reactions, increasing the proportion of particles with energy exceeding this barrier.
3. Enzymes are biological catalysts that are highly specific and function via a lock-and-key mechanism to catalyze reactions in living organisms.
Air pollution
The document discusses various sources and effects of air pollution. It describes how burning fossil fuels from industries, automobiles, and power plants releases pollutants like carbon monoxide, sulfur dioxide, and nitrogen oxides into the air. This leads to issues like acid rain, photochemical smog, and global warming. Air pollution damages the environment, climate, plants, animals, and human health, causing problems like acidification of soils and water sources, reduced visibility, and respiratory illnesses. The text provides details on the formation and harmful impacts of acid rain and photochemical smog. Overall, the document analyzes the causes and wide-ranging consequences of air pollution from various human and industrial activities.
Metals and metallurgy
The document discusses the principles of metallurgy and metal extraction processes. It defines metals, non-metals and metalloids based on their properties. The processes involved in metal extraction include mining, crushing, concentration, roasting, reduction and refining. Concentration methods separate the metal ore from gangue using techniques like gravity separation, magnetic separation or froth flotation. Reduction converts the metal oxide into pure metal using carbon or aluminothermic processes. Refining further purifies the metal using techniques like liquation, distillation, electrolysis or poling. Overall, the document provides an overview of the key concepts and steps involved in extracting and processing metals from their ores.
Metallurgy
The document discusses the various processes involved in metallurgy, which is the extraction of metals from ores and their purification. There are three main types of metallurgical processes - pyrometallurgy which uses high temperatures, hydrometallurgy which uses aqueous solutions, and electrometallurgy which uses electrolysis. Common steps in metal extraction include mining the ore, crushing and grinding it, concentrating the ore to remove impurities, roasting or calcining it, reducing the metal oxides to the pure metal, and finally refining the metal through processes like liquation, distillation, or electrolysis.
Sodium
- Alkali metals have low ionization energies and readily lose their outer electron to form cations with a +1 oxidation state. They are soft, reactive metals that form ionic compounds.
- Sodium is the second alkali metal and is found abundantly in nature as the mineral sodium chloride. It is extracted commercially via the Downs process, which involves electrolysis of molten sodium chloride at lower temperatures using calcium chloride. This allows pure sodium to be produced at the cathode and chlorine gas to be collected at the anode.
Chemical thermodynamics
This document discusses key concepts in chemical thermodynamics including:
- Thermodynamics deals with different forms of energy and quantitative relationships between them. Chemical thermodynamics focuses on chemical changes.
- Systems, surroundings, boundaries, closed/open/isolated systems, and state functions like internal energy are defined.
- The first law of thermodynamics states that energy is conserved and can be converted between different forms like work and heat but not created or destroyed.
Water
Water has a simple molecular structure composed of one oxygen atom covalently bonded to two hydrogen atoms. This gives water a polar molecular structure with partial positive charges near the hydrogen atoms and a partial negative charge near the oxygen atom. This polarity allows water to dissolve ionic compounds through electrostatic interactions between the ions and polar water molecules but not non-polar covalent compounds which do not interact strongly with water. Heavy water, composed of deuterium and oxygen, is produced through electrolysis or distillation of ordinary water. It has similar but not identical chemical properties as ordinary water and is used as a neutron moderator and to produce deuterium.
Nitric acid
Nitric acid is manufactured through Ostwald's process, which involves the catalytic oxidation of ammonia by air over a platinum catalyst heated to 800°C, forming nitric oxide. The nitric oxide is cooled and oxidized to nitrogen dioxide, which is then absorbed in water in an absorption tower to produce nitric acid solution. The dilute nitric acid is further concentrated by distillation under reduced pressure to obtain approximately 98% nitric acid.
Water
Water has a simple molecular structure composed of one oxygen atom covalently bonded to two hydrogen atoms. This gives water a polar molecular structure with partial positive charges near the hydrogen atoms and a partial negative charge near the oxygen atom. This polarity allows water to dissolve ionic compounds through electrostatic interactions between the ions and polar water molecules, but not non-polar covalent compounds which do not interact strongly with water. Heavy water, composed of deuterium instead of hydrogen, is used as a neutron moderator in nuclear reactions and to produce deuterium through electrolysis or reaction with metals.
Chemical kinetics
This document summarizes key concepts in chemical kinetics including:
1. Chemical kinetics deals with the rates of chemical reactions and factors that affect rates. Rates can be expressed in terms of changes in concentrations over time.
2. Reaction rates depend on temperature, catalysts, and concentrations as expressed in rate laws. Rate constants are measures of reaction speeds.
3. Reactions can have different orders depending on which concentrations influence the rate. Pseudo-order reactions appear higher order but actually follow lower order kinetics.
Chemical equiilibrium
The document discusses chemical equilibrium, which occurs when opposing chemical processes proceed at equal rates, such that the concentrations of reactants and products remain constant over time. It provides examples of physical equilibria like liquid-vapor and solid-liquid, and chemical equilibria like reversible reactions. The document also explains concepts like Le Chatelier's principle, the law of mass action, equilibrium constants, and how concentration, temperature, and pressure can affect chemical equilibrium.
Electrochemistry
This document discusses key concepts in electrochemistry including:
- Electrochemistry deals with chemical and physical processes involving the production or consumption of electricity.
- Electrode potential is the potential difference that exists between a metal and its ions in solution, arising from their relative tendencies to undergo oxidation or reduction reactions.
- Standard hydrogen electrode is used as a reference electrode to measure standard electrode potentials of other half-cells.
- Standard electrode potential of a half-cell indicates its voltage when connected to the standard hydrogen electrode under standard conditions.
- Electromotive force is the difference in potential between the cathode and anode half-cells of an electrochemical cell.
9701 y16 sm_2 (1)
This document consists of 7 printed pages and 1 blank page containing the specimen mark scheme for Paper 2 (AS Level Structured Questions) of the Cambridge International A Level Chemistry exam. The mark scheme provides detailed guidance on how answers should be marked, including the points awarded for different parts of questions and acceptable alternative responses. Key information includes abbreviations used in the mark scheme, the maximum number of marks available for each question, and detailed annotations for multi-part questions to indicate which parts of answers are correct.
9701 y16 sp_2 (1)
This document consists of a specimen paper for the Cambridge International AS Level Chemistry exam. It contains two sample exam questions with multiple parts testing knowledge of topics including:
- Properties of different elements and compounds
- Bonding and molecular structure
- Reaction rates and activation energy
- Periodic trends and properties of elements
- Properties of oxides and fluorides
The document provides context for two sample exam questions along with spaces for students to show their work. It aims to prepare students for the structure and style of questions on the actual AS Level Chemistry exam.
World environment day
World Environment Day occurs annually on June 5th and is coordinated by the United Nations to promote worldwide awareness and action to protect the environment. It has brought attention to issues like marine pollution, overpopulation, climate change, and sustainability. Each year it focuses on a new theme adopted by governments, organizations, and celebrities to advocate for environmental causes. The theme in 2017 was "Connecting People to Nature" and highlighted the importance of natural systems for humanity. World Environment Day encourages ongoing advocacy and action to promote environmental responsibility and conservation of natural resources.
Paper 2 2069
This document provides instructions and questions for a chemistry exam. It states that the exam is for Chemistry 9701, Paper 2, Structured Questions, lasting 1 hour and 15 minutes. It provides instructions for candidates to write their name, roll number, and to answer all questions in dark blue or black pen. Questions cover topics like the kinetic molecular theory of gases, chemical reactions involving ethanol, ethane, ethene, cyclohexene, malic acid, and determining an empirical formula from elemental composition data. Students are asked to write balanced equations, determine products, draw structural formulas, and explain reaction types.
Cw stoichiometry intro 041112
The document provides an introduction to stoichiometry and the mole concept. It discusses key topics including:
1. The mole is a unit used to describe the amount of substance in chemistry and is equal to 6.022x1023 particles.
2. The molar mass of an element or compound is the mass in grams of one mole and can be used to calculate amounts in chemical reactions.
3. Conversions can be made between moles, particles, masses, and volumes using the molar mass and molar relationships like moles = mass/molar mass.
4. Solution concentration is expressed in molarity, which is the moles of solute per liter of solution. M
4 calorimetry
Calorimetry involves measuring the heat transferred to or from a chemical reaction by using the heat transferred to raise the temperature of water. The enthalpy change of a reaction can be calculated using the formula: ΔH = mass of water x specific heat capacity of water x temperature change. This document provides the process for measuring enthalpy changes including using a calorimeter, allowing reactants to reach temperature of surroundings before mixing, measuring temperature change, and calculating enthalpy change using the formula. An example calculation is included.
Iris van Herpen. pptx
Power-point sur une exposition qui a eu lieu dans le Musée des Arts décoratifs à Paris sur Iris van Herpen
Contenu connexe
Plus de Gandaki Boarding School,Lamachaur-16 Pokhara, Nepal
Metals and metallurgy
The document discusses the principles of metallurgy and metal extraction processes. It defines metals, non-metals and metalloids based on their properties. The processes involved in metal extraction include mining, crushing, concentration, roasting, reduction and refining. Concentration methods separate the metal ore from gangue using techniques like gravity separation, magnetic separation or froth flotation. Reduction converts the metal oxide into pure metal using carbon or aluminothermic processes. Refining further purifies the metal using techniques like liquation, distillation, electrolysis or poling. Overall, the document provides an overview of the key concepts and steps involved in extracting and processing metals from their ores.
Metallurgy
The document discusses the various processes involved in metallurgy, which is the extraction of metals from ores and their purification. There are three main types of metallurgical processes - pyrometallurgy which uses high temperatures, hydrometallurgy which uses aqueous solutions, and electrometallurgy which uses electrolysis. Common steps in metal extraction include mining the ore, crushing and grinding it, concentrating the ore to remove impurities, roasting or calcining it, reducing the metal oxides to the pure metal, and finally refining the metal through processes like liquation, distillation, or electrolysis.
Sodium
- Alkali metals have low ionization energies and readily lose their outer electron to form cations with a +1 oxidation state. They are soft, reactive metals that form ionic compounds.
- Sodium is the second alkali metal and is found abundantly in nature as the mineral sodium chloride. It is extracted commercially via the Downs process, which involves electrolysis of molten sodium chloride at lower temperatures using calcium chloride. This allows pure sodium to be produced at the cathode and chlorine gas to be collected at the anode.
Chemical thermodynamics
This document discusses key concepts in chemical thermodynamics including:
- Thermodynamics deals with different forms of energy and quantitative relationships between them. Chemical thermodynamics focuses on chemical changes.
- Systems, surroundings, boundaries, closed/open/isolated systems, and state functions like internal energy are defined.
- The first law of thermodynamics states that energy is conserved and can be converted between different forms like work and heat but not created or destroyed.
Water
Water has a simple molecular structure composed of one oxygen atom covalently bonded to two hydrogen atoms. This gives water a polar molecular structure with partial positive charges near the hydrogen atoms and a partial negative charge near the oxygen atom. This polarity allows water to dissolve ionic compounds through electrostatic interactions between the ions and polar water molecules but not non-polar covalent compounds which do not interact strongly with water. Heavy water, composed of deuterium and oxygen, is produced through electrolysis or distillation of ordinary water. It has similar but not identical chemical properties as ordinary water and is used as a neutron moderator and to produce deuterium.
Nitric acid
Nitric acid is manufactured through Ostwald's process, which involves the catalytic oxidation of ammonia by air over a platinum catalyst heated to 800°C, forming nitric oxide. The nitric oxide is cooled and oxidized to nitrogen dioxide, which is then absorbed in water in an absorption tower to produce nitric acid solution. The dilute nitric acid is further concentrated by distillation under reduced pressure to obtain approximately 98% nitric acid.
Water
Water has a simple molecular structure composed of one oxygen atom covalently bonded to two hydrogen atoms. This gives water a polar molecular structure with partial positive charges near the hydrogen atoms and a partial negative charge near the oxygen atom. This polarity allows water to dissolve ionic compounds through electrostatic interactions between the ions and polar water molecules, but not non-polar covalent compounds which do not interact strongly with water. Heavy water, composed of deuterium instead of hydrogen, is used as a neutron moderator in nuclear reactions and to produce deuterium through electrolysis or reaction with metals.
Chemical kinetics
This document summarizes key concepts in chemical kinetics including:
1. Chemical kinetics deals with the rates of chemical reactions and factors that affect rates. Rates can be expressed in terms of changes in concentrations over time.
2. Reaction rates depend on temperature, catalysts, and concentrations as expressed in rate laws. Rate constants are measures of reaction speeds.
3. Reactions can have different orders depending on which concentrations influence the rate. Pseudo-order reactions appear higher order but actually follow lower order kinetics.
Chemical equiilibrium
The document discusses chemical equilibrium, which occurs when opposing chemical processes proceed at equal rates, such that the concentrations of reactants and products remain constant over time. It provides examples of physical equilibria like liquid-vapor and solid-liquid, and chemical equilibria like reversible reactions. The document also explains concepts like Le Chatelier's principle, the law of mass action, equilibrium constants, and how concentration, temperature, and pressure can affect chemical equilibrium.
Electrochemistry
This document discusses key concepts in electrochemistry including:
- Electrochemistry deals with chemical and physical processes involving the production or consumption of electricity.
- Electrode potential is the potential difference that exists between a metal and its ions in solution, arising from their relative tendencies to undergo oxidation or reduction reactions.
- Standard hydrogen electrode is used as a reference electrode to measure standard electrode potentials of other half-cells.
- Standard electrode potential of a half-cell indicates its voltage when connected to the standard hydrogen electrode under standard conditions.
- Electromotive force is the difference in potential between the cathode and anode half-cells of an electrochemical cell.
9701 y16 sm_2 (1)
This document consists of 7 printed pages and 1 blank page containing the specimen mark scheme for Paper 2 (AS Level Structured Questions) of the Cambridge International A Level Chemistry exam. The mark scheme provides detailed guidance on how answers should be marked, including the points awarded for different parts of questions and acceptable alternative responses. Key information includes abbreviations used in the mark scheme, the maximum number of marks available for each question, and detailed annotations for multi-part questions to indicate which parts of answers are correct.
9701 y16 sp_2 (1)
This document consists of a specimen paper for the Cambridge International AS Level Chemistry exam. It contains two sample exam questions with multiple parts testing knowledge of topics including:
- Properties of different elements and compounds
- Bonding and molecular structure
- Reaction rates and activation energy
- Periodic trends and properties of elements
- Properties of oxides and fluorides
The document provides context for two sample exam questions along with spaces for students to show their work. It aims to prepare students for the structure and style of questions on the actual AS Level Chemistry exam.
World environment day
World Environment Day occurs annually on June 5th and is coordinated by the United Nations to promote worldwide awareness and action to protect the environment. It has brought attention to issues like marine pollution, overpopulation, climate change, and sustainability. Each year it focuses on a new theme adopted by governments, organizations, and celebrities to advocate for environmental causes. The theme in 2017 was "Connecting People to Nature" and highlighted the importance of natural systems for humanity. World Environment Day encourages ongoing advocacy and action to promote environmental responsibility and conservation of natural resources.
Paper 2 2069
This document provides instructions and questions for a chemistry exam. It states that the exam is for Chemistry 9701, Paper 2, Structured Questions, lasting 1 hour and 15 minutes. It provides instructions for candidates to write their name, roll number, and to answer all questions in dark blue or black pen. Questions cover topics like the kinetic molecular theory of gases, chemical reactions involving ethanol, ethane, ethene, cyclohexene, malic acid, and determining an empirical formula from elemental composition data. Students are asked to write balanced equations, determine products, draw structural formulas, and explain reaction types.
Cw stoichiometry intro 041112
The document provides an introduction to stoichiometry and the mole concept. It discusses key topics including:
1. The mole is a unit used to describe the amount of substance in chemistry and is equal to 6.022x1023 particles.
2. The molar mass of an element or compound is the mass in grams of one mole and can be used to calculate amounts in chemical reactions.
3. Conversions can be made between moles, particles, masses, and volumes using the molar mass and molar relationships like moles = mass/molar mass.
4. Solution concentration is expressed in molarity, which is the moles of solute per liter of solution. M
4 calorimetry
Calorimetry involves measuring the heat transferred to or from a chemical reaction by using the heat transferred to raise the temperature of water. The enthalpy change of a reaction can be calculated using the formula: ΔH = mass of water x specific heat capacity of water x temperature change. This document provides the process for measuring enthalpy changes including using a calorimeter, allowing reactants to reach temperature of surroundings before mixing, measuring temperature change, and calculating enthalpy change using the formula. An example calculation is included.
Plus de Gandaki Boarding School,Lamachaur-16 Pokhara, Nepal (20)
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Power-point sur une exposition qui a eu lieu dans le Musée des Arts décoratifs à Paris sur Iris van Herpen
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