Punjab Technical University‚ Jalandhar B.Tech. Chemical Engg. Scheme of Syllabi ( 3rd Semester ) Sr. no 1 2 3 4 5 6 7 8 9 Course Code Ch-201 Ch-203 Ch-205 Ch-207 Ch-209 Ch-211 Ch-213 Ch-215 Ch-217 Course Title Mechanical Operations Numerical Methods in Chemical Engineering Organic & Biotechnology Chemical Process Calculations Fluid Flow Strength of Materials Strength of Materials Lab. Fluid Flow Lab. Numerical Methods in Chem. Engg. Lab. L 3 3 3 3 3 3 - T 1 1 1 1 1 - P 2 3 4
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can quickly change between the different forms of H2O by either increasing or decreasing temperature. We have worked with hot plates and thermometers in other labs before‚ so we know how to be safe. I wonder what a graph of the changing temperatures over time between the phases would look like. Hypothesis Based on prior learning‚ I predict that the graph of the water phase changes will not be one straight slope‚ but instead will plateau‚ or be flat‚ and then slope between the change of ice to
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term ‘physical change’ A physical change is where the appearance or traits of the substance/item change these changes can be‚ change of size‚ shape‚ color‚ volume and state. The molecules in the substance can be rearranged but their composition must stay the same. No new substance can be formed. They can be reversed most of the time. 2. Describe one example of a physical change in everyday life and explain why it is a physical change. Melting an ice cube is a common physical change. Melting an ice
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Alloy - An alloy is a substance made by melting two or more elements together‚ at least one of them a metal. An Example: Examples of alloys include brass‚ bronze‚ 14k gold‚ and sterling silver. covalent bond - A covalent bond is a chemical link between two atoms in which electrons are shared between them. An Example: There is covalent between the oxygen and each hydrogen in (H 2 O). Each of the bonds contains two electrons - one from a hydrogen atom and one from the oxygen atom. Both atoms
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1. Ozone (O3) in the atmosphere can react with nitric oxide (NO): O3(g) + NO(g) ( NO2(g) + O2(g)‚ with (H( = -199 kJ/mol‚ (S( = -4.1 J/K·mol. Calculate the (G( for this reaction at 25(C. A. 1020 kJ/mol B. -1.22 ( 103 kJ/mol C. 2.00 ( 103 kJ/mol D. -1.42 ( 103 kJ/mol E. -198 kJ/mol 2. For the reaction H2(g) + S(s) ( H2S(g)‚ (H( = -20.2 kJ/mol and (S( = +43.1 J/K·mol. Which of these statements is true? A. The reaction is only spontaneous
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“Climate Change Over Time” I. Introduction a. In this lab‚ the question being investigated is‚ “Has climate changed over time?” b. The hypothesis is‚ “If CO2 levels affect climate‚ then the climate has changed overtime because of the increased greenhouse effect caused by higher levels of CO2 emissions.” c. Variables: 1. Independent Variable: Amount of CO2 2. Dependent Variable: Climate change II. Background Information Climate is the weather pattern in an area over long period of
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PHYSICAL SCIENCE physical change-changes affecting the form of a chemical substance‚Physical changes are used to separate mixtures into their component compounds Example:breaking glass Chemical changes- when a substance combines with another to form a new substance ‚called chemical synthesis. Example: burning wood Law of Conservation of Mass-The law of conservation of mass states that mass in an isolated system is neither created nor destroyed by chemical reactions or physical transformations
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Photocatalytic degradation of methylene blue using TiO2 nanoparticles Nupur Mittal Chemical Engineering‚ IIT (BHU) Varanasi. Abstract: The aim of this research is to reduce the pollution caused by methylene blue dye in waste water coming from textile industries. For this purpose‚ TiO2 nanoparticles are made as they show good photocatalytic activity in degradation of dyes into harmless products. Synthesis is done using titanium butoxide and 2-propanol. The particles formed were a little larger
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Experiment 1: Observations of Chemical Changes Lab Partners: None Date of Experiment: February 25‚ 2015 Location: My House Abstract: The experiment intended to provide observations of chemical changes as the primary objective. The experiment was divided into two parts‚ first‚ mixing two aqueous solutions of ionic compounds. The second part involved the observance of heating and combustion reactions‚ using the supplied solid elements and compounds. Experiment and Observations: The first part of
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with hydrochloric acid (HCl) to determine the molar volume of hydrogen gas (H2) (converted to the molar volume at STP) and then‚ to compare obtained results with the molar volume of an ideal gas. To determine the measured molar volume of hydrogen gas‚ we are going to use this equation: The molar volume of the ideal gas will be determined by the equation ‚ where T = 237 K‚ P = 101.3 kPa. The hydrogen gas will be collected as a product of chemical reaction where Magnesium reacts with hydrochloric
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