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Knowledge in chemical engineering
Yash Bhat
Radioactivity and radiation - engineering first year
Detailed handwritten notes on topic radioactivity.
shubhangi Gupta
Wave equation - first year engineering
Handwritten clear described notes. Accurate and precise data.
Forging - engineering first year
Notes on forging. informative and accurate data on the topic.
Energy balance - IIT BOMBAY
Notes issued by IIT Bombay on energy balance. Printed textual material.
THERMOCHEMISTRY
Thermochemistry is the study of the heat energy associated with chemical reactions and/or physical transformations. A reaction may release or absorb energy, and a phase change may do the same, such as in melting and boiling. Thermochemistry focuses on these energy changes, particularly on the system's energy exchange with its surroundings. Thermochemistry is useful in predicting reactant and product quantities throughout the course of a given reaction. In combination with entropy determinations, it is also used to predict whether a reaction is spontaneous or non-spontaneous, favorable or unfavorable. Endothermic reactions absorb heat, while exothermic reactions release heat. Thermochemistry coalesces the concepts of thermodynamics with the concept of energy in the form of chemical bonds. The subject commonly includes calculations of such quantities as heat capacity, heat of combustion, heat of formation, enthalpy, entropy, free energy, and calories. The world's first ice-calorimeter, used in the winter of 1782-83, by Antoine Lavoisier and Pierre-Simon Laplace, to determine the heat evolved in various chemical changes; calculations which were based on Joseph Black’s prior discovery of latent heat. These experiments mark the foundation of thermochemistry. Contents 1 History 2 Calorimetry 3 Systems 4 Processes 5 See also 6 References 7 External links History Thermochemistry rests on two generalizations. Stated in modern terms, they are as follows:[1] Lavoisier and Laplace's law (1780): The energy change accompanying any transformation is equal and opposite to energy change accompanying the reverse process.[2] Hess' law (1840): The energy change accompanying any transformation is the same whether the process occurs in one step or many. These statements preceded the first law of thermodynamics (1845) and helped in its formulation. Lavoisier, Laplace and Hess also investigated specific heat and latent heat, although it was Joseph Black who made the most important contributions to the development of latent energy changes. Gustav Kirchhoff showed in 1858 that the variation of the heat of reaction is given by the difference in heat capacity between products and reactants: dΔH / dT = ΔCp. Integration of this equation permits the evaluation of the heat of reaction at one temperature from measurements at another temperature.[3][4] Calorimetry The measurement of heat changes is performed using calorimetry, usually an enclosed chamber within which the change to be examined occurs. The temperature of the chamber is monitored either using a thermometer or thermocouple, and the temperature plotted against time to give a graph from which fundamental quantities can be calculated. Modern calorimeters are frequently supplied with automatic devices to provide a quick read-out of information, one example being the differential scanning calori
Shantha Kumar . V
THERMOCHEMISTRY
Thermochemistry is the study of the heat energy associated with chemical reactions and/or physical transformations. A reaction may release or absorb energy, and a phase change may do the same, such as in melting and boiling. Thermochemistry focuses on these energy changes, particularly on the system's energy exchange with its surroundings. Thermochemistry is useful in predicting reactant and product quantities throughout the course of a given reaction. In combination with entropy determinations, it is also used to predict whether a reaction is spontaneous or non-spontaneous, favorable or unfavorable. Endothermic reactions absorb heat, while exothermic reactions release heat. Thermochemistry coalesces the concepts of thermodynamics with the concept of energy in the form of chemical bonds. The subject commonly includes calculations of such quantities as heat capacity, heat of combustion, heat of formation, enthalpy, entropy, free energy, and calories. The world's first ice-calorimeter, used in the winter of 1782-83, by Antoine Lavoisier and Pierre-Simon Laplace, to determine the heat evolved in various chemical changes; calculations which were based on Joseph Black’s prior discovery of latent heat. These experiments mark the foundation of thermochemistry. Contents 1 History 2 Calorimetry 3 Systems 4 Processes 5 See also 6 References 7 External links History Thermochemistry rests on two generalizations. Stated in modern terms, they are as follows:[1] Lavoisier and Laplace's law (1780): The energy change accompanying any transformation is equal and opposite to energy change accompanying the reverse process.[2] Hess' law (1840): The energy change accompanying any transformation is the same whether the process occurs in one step or many. These statements preceded the first law of thermodynamics (1845) and helped in its formulation. Lavoisier, Laplace and Hess also investigated specific heat and latent heat, although it was Joseph Black who made the most important contributions to the development of latent energy changes. Gustav Kirchhoff showed in 1858 that the variation of the heat of reaction is given by the difference in heat capacity between products and reactants: dΔH / dT = ΔCp. Integration of this equation permits the evaluation of the heat of reaction at one temperature from measurements at another temperature.[3][4] Calorimetry The measurement of heat changes is performed using calorimetry, usually an enclosed chamber within which the change to be examined occurs. The temperature of the chamber is monitored either using a thermometer or thermocouple, and the temperature plotted against time to give a graph from which fundamental quantities can be calculated. Modern calorimeters are frequently supplied with automatic devices to provide a quick read-out of information, one example being the differential scanning calori
CHEMICAL KINETICS
Order and molecularity,Chemical kinetics is the branch of physical chemistry which deals with a study of the speed of chemical reactions. Such studies also enable us to understand the mechanism by which the reaction occurs. Thus, in chemical kinetics we can also determine the rate of chemical reaction. From the kinetic stand point the reactions are classified into two groups: a)homogeneousreactionswhichoccurentirelyinonephaseb)heterogeneousreactions where the transformation takes place on the surface of a catalyst or the walls of a container. 1.2 Rateofreaction The rate of reaction i.e. the velocity of a reaction is the amount of a chemical change occurring per unit time. The rate is generally expressed as the decrease in concentration of a reactant or as the increase in concentration of the product. IfCthe concentration of a reactant at any time t is, the rate is−dC dt or if the concentration of a product be xat any time t, the rate would bedx dt. The time is usually expressed in seconds. The rate will have units of concentration divided by time. The concentrations are taken in gm-moles/litre, hence rate is moles/litre/second.
Material balance in Coke making
Notes by IIT KHARAGPUR, printed study material detailed and informative.
Chemical reaction engineering notes (aktu, MIET MEERUT)
Chemical reaction engineering basic concept First order system Second order system Zero order system Plug flow reactor Cstr(continous stirred tank reactor) Entropy Thiele modulus Pfr in series Pfr in parallel Cstr in series Recycle reactor Uses Benefits From meerut institude of engineering and technology Meerut For GATE 2019 PREPARATION IMPORTANT NOTES
Varshika Singhal