Chemistry for Engineers Lesson 1 PDF

CHEMISTRY FOR ENGINEERS FIRST SEMESTER LESSON 1: INTRODUCTION THE FOUNDATIONS OF CHEMISTRY PREPARED BY: ENGR. PATRICIA EMMANUELLE RAGANIT  TOPIC OUTLINE 01. Introduction - Chemistry in Engineering...

CHEMISTRY FOR ENGINEERS FIRST SEMESTER LESSON 1: INTRODUCTION THE FOUNDATIONS OF CHEMISTRY PREPARED BY: ENGR. PATRICIA EMMANUELLE RAGANIT  TOPIC OUTLINE 01. Introduction - Chemistry in Engineering 04. Chemical and Physical Properties Field 02. Matter and Energy 05. Use of Numbers 03. Classification of Matter 06. The Unit Factor Method Introduction to Chemistry Chemistry is the science that describes matter, its properties, the changes it undergoes and the energy changes those processes “central science” Organic Chemistry Inorganic Chemistry Analytical Chemistry Physical Chemistry Biochemistry Introduction to Chemistry Organic Chemistry- The study of carbon-containing compounds, particularly those found in living organisms. Inorganic Chemistry - The study of inorganic compounds, which generally do not contain carbon-hydrogen bonds Analytical Chemistry - Analytical chemists develop techniques to identify and quantify the chemical components of natural and artificial materials. Introduction to Chemistry Physical Chemistry - It combines concepts from physics and chemistry to understand the behavior of matter at a molecular and atomic level Biochemistry - The study of chemical processes within and related to living organisms. This branch merges biology and chemistry to explore cellular and molecular biology.  Importance of Chemistry in the Field of Engineering 1 Material Science 3 Component Design Battery 2 Optimization 4 Environmental Solutions  Chemistry in Electrical Engineering 1. Materials Science: Chemistry informs properties of electrical materials like semiconductors, conductors, and insulators. 2. Battery Optimization: Chemical knowledge enhances battery performance, safety, and longevity in electrical devices.  Chemistry in Electrical Engineering 3. Component Design: Chemistry guides design of electronic components like transistors, capacitors, and diodes. 4. Environmental Solutions: Chemistry aids in developing sustainable practices for electronics production and disposal. 1.1 MATTER AND ENERGY Matter - anything that occupies space and has mass. Mass- a measure of the quantity of matter in a sample of any material Energy - defined as the capacity to do work or to transfer heat Kinetic Energy - energy possessed by an object due to its motion e.g. translational energy, rotational energy, etc. Potential Energy - energy of an object due to its position, condition, or composition e.g. gravitational potential energy, elastic potential energy, chemical energy, etc. 1.1 MATTER AND ENERGY Law of Conservation of Energy states that energy cannot be created or destroyed in a chemical reaction or a physical change. It can only be converted from one form to another The relationship between matter and energy is given by Albert Einstein’s Equation: The combined amount of matter and energy in the universe is fixed 1.3 STATES OF MATTER SOLID Composed of particles that are tightly packed and have a regular arrangement It has definite volume and shape LIQUID Individual particles are confined to a given volume Definite volume but no specific shape GAS Composed of particles with no regular arrangement It has no definite volume and shape 1.2 STATES OF MATTER PLASMA a gas to which sufficient energy is provided to free electrons from atoms conductor of electricity BOSE- EINSTEIN CONDENSATE occurs at ultralow temperature (very near absolute zero) close to the point that atoms are not moving at all 1.1 MATTER AND ENERGY 1.2 STATES OF MATTER PROPERTY SOLID LIQUID GAS Flows and assumes the Fills any container RIGIDITY Rigid shape of the completely container EXPANSION ON Slight Slight Expands infinitely HEATING Easily COMPRESSIBILITY Slight Slight Compressed 1.4 CLASSIFICATIONS OF MATTER SUBSTANCE is a form of matter that has a definite composition and distinct properties ELEMENT simplest form of matter since it only contains one kind of atom COMPOUND are pure substances that contains two or more elements combined in a definite proportion. 1.4 CLASSIFICATIONS OF MATTER MIXTURE a combination of two or more substances in which the substances retain their distinct identities Homogeneous mixture - has the same composition throughout Heterogeneous mixture - do not have the same composition throughout, components are distinguishable 1.3 CLASSIFICATION OF MATTER (Separated by physical means) (Separated by chemical means) 1.4 CHEMICAL AND PHYSICAL PROPERTIES CHEMICAL PROPERTIES exhibited by matter as it undergoes changes in composition PHYSICAL PROPERTIES can be observed in the absence of any change in composition can be dependent on the conditions under which they are measured EXTENSIVE PROPERTIES properties that are dependent on the amount of substance present e.g. mass, volume, etc. INTENSIVE PROPERTIES properties that are independent of the amount of substance being examined e.g. density, color etc. CHEMICAL AND PHYSICAL PROPERTIES 1.4.1 CHEMICAL AND PHYSICAL CHANGES PHYSICAL CHANGE occurs with no change in chemical composition includes changes in state, shape, size and mostly reversible e.g melting of ice, breaking of glass, etc. CHEMICAL CHANGES one or more substances are used up (at least partially) one or more new substances are formed energy is absorbed or released change in color and formation of bubbles MAY be a sign of chemical change e.g decomposition, burning, etc. MEASUREMENTS IN CHEMISTRY The Seven Fundamental Units of Measurement (SI) PHYSICAL PROPERTIES NAME OF UNIT SYMBOL length meter m mass kilogram kg time second s electric current ampere A temperature kelvin K luminous intensity candela cd amount of substanx mole mol Prefixes for Powers of Ten yocto  Important Conversion Factors LENGTH MASS VOLUME 1m 100 cm 1 kg 1000 g 1 cubic 1mL cm 1 in 2.54 cm 1 kg 2.2 lb 1 mL 20 drops 1m 3.28 ft 1 ton 2000 lb 1L 1000 mL 1 mile 5280 ft 1 metric 1000 kg ton 1 gal 3.79 L 1 ft 12 in 1 slug 14.59 kg 1 yard 3 feet 1 cubic m 264.2 gal 1 lb 16 ounces 1 cubic m 1000 L  Important Conversion Factors and Derived Units TIME 1N 1 kg-m/s^2 1 minute 60 s 1J 1N-m 1 hour 60 mins 1 slug- 1W 1 J/s 1 lbf 1 day 24 hours ft/s^2 1 hp 746 Watts 1 week 7 days 1 lbf 4.45 N 1 Pa 1 N/m^2 1 year 52 weeks 101, 325 1 atm 1 year 365 days Pa  TEMPERATURE CONVERSION Celsius to Fahrenheit Fahrenheit to Celsius Fahrenheit to Rankine Celsius to Kelvin  TEMPERATURE CONVERSION Examples: 1. Convert 20 degrees F to: Celsius Rankine Kelvin 2. Convert 89 degrees C to: Fahrenheit Rankine Kelvin 1.5 USE OF NUMBERS SCIENTIFIC NOTATIONS used to express very large and/or very small numbers we place one nonzero digit to the left of the decimal e.g SIGNIFICANT FIGURES numbers obtained by counting or from definition are exact numbers obtained from measurements are inexact and all measurements involves estimation Precision - how closely individual measurements agree with one another Accuracy - how closely a measured value agrees with the correct value 1.5 USE OF NUMBERS GUIDELINES FOR THE USE OF SIGNIFICANT FIGURES 1. Nonzero digits are ALWAYS significant 2. Zeroes are sometimes significant, and sometimes they are not Zeros at the beginning of a number (used just to position the decimal point are NEVER significant Zeroes between nonzero digits are ALWAYS significant 1.5 USE OF NUMBERS GUIDELINES FOR THE USE OF SIGNIFICANT FIGURES Zeroes at the end of a number that contains a decimal point are ALWAYS significant Zeroes at the end of a number that does not contain a decimal point may or may not be significant 3. Exact numbers can be considered as having unlimited number of significant figures EXAMPLES SCIENTIFIC NOTATION (Rewrite each item in scientific notation) 1. 12 756 200 meters = 2. 0.00000625 ms = 3. 602214076 = SIGNIFICANT FIGURES (Identify how many S.F does each measurement has) 1. 440.0 lbs 2. 2024. g 3. 0.0008 in 4. 3.14 x 10^4 km 5. 7.680 x 10^-6 cm 6. 24300 hectares 7. 101.10000 mL RULES IN OPERATIONS ADDITION AND SUBTRACTION Check if the quantities have the same units The answer cannot have more digits to the right of the decimal point than any of the original numbers Examples: 1. 37.24 mL + 10.3 mL = 2. 78.0 m - 50.53 ft = 3. Subtract 178.56 lbs from 300.75 lbs 4. 78.09789 cm + 34.675468 cm RULES IN OPERATIONS MULTIPLICATION OR DIVISION The number of significant figures in the result is set by the original number that has the least number of significant figures Examples: 1. 8.90 x 56.13 = 2. 3.3333 x 1.3 = 3. 76.01 x 89.045 = 4. 10.025 / 6.78 = 5. 1979.666 / 10.0 = 1.6 The Unit Factor Method Also known as “dimensional analysis” or “factor-label method” Essentially performing conversions by “multiplying by one” Example: Convert the ff. into the desired units 1. 78 gallons to liters 2. 2 short tons to hectograms 3. 0.98 miles to inches 4. 2.07 atm to KPa 5. 8.07 x 10^7 cm to yards 1.6 The Unit Factor Method SEATWORK I. Convert 12 degrees Celsius into: a. Fahrenheit b. Kelvin c. Rankine II. Convert the ff. into the desired units 1. )1 megameter to miles 2. )3 tons to slugs 3. ) 40×10^6 drops to cubic cm 4. )360 KPa to atm 5. )3780 cc of saltwater to kilograms ( density of saltwater: 1.03)  1.6 The Unit Factor Method Area Conversion 1. How many square meters are there in 250 square feet? 2. Which lot is bigger? (a) 500 square feet (b) 200 square meters Volume Conversion 1. How many cubic millimeters are there in 5 Liters ? 2. 10000 drops is equal to how many cubic centimeters? 1.6 The Unit Factor Method ASSIGNMENT NO.1 1. Suppose that your automobile gas tank holds 4 gal and the price per liter is Php 65, how much would it cost to fill half of your tank? 2. Titanium is used in airplanes because it is strong and light, it has a density of 4.55 g/cm^3. If a cylinder of titanium is 10.67 cm long and has a mass of 456.90 g. Calculate the radius of the cylinder. 3. A small crystal of sucrose (table sugar) had a mass of 6.08 mg. The dimensions of the box-like structure crystal were 2.2 mm x 1.36 mm x 1.23 mm. What is the density of the sucrose as expressed in g/cm^3?