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CHEM 141 Week 2

by: Isabella Sturgeon

CHEM 141 Week 2 CHMY 141N - 00

Isabella Sturgeon
GPA 3.67
College Chemistry I
Mark Cracolice (P)

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About this Document

Hi all, These are my notes from General Chemistry: An Inquiry Approach and Think Out Loud! both by Mark Cracolice, and CHEM 141 lecture for week two. I will be posting notes for this course weekl...
College Chemistry I
Mark Cracolice (P)
Class Notes
CHEM 141, College Chemistry 1, General Chemistry, Cracolice, Lesson 4, Lesson 5
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This 3 page Class Notes was uploaded by Isabella Sturgeon on Sunday September 13, 2015. The Class Notes belongs to CHMY 141N - 00 at University of Montana taught by Mark Cracolice (P) in Fall 2015. Since its upload, it has received 101 views. For similar materials see College Chemistry I in Chemistry at University of Montana.


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Date Created: 09/13/15
Week 2 Chemistry 141 Lecture Notes Lessons 45 Please note that these lessons came from General Chemistry An Inquiry Approach Lesson 4 How do Scientists Make Report and Work with Quantitative Measurements Overview This lesson explains the importance of uncertainty in measurements by looking at the precision and accuracy of a tool used for measurement This lesson also deals with significant figures and how to manipulate answers to go from ambigious to having the correct number of significant figures for that problem Vocabulary Precision a tools ability to reproduce results Accuracy how close the results are to a true value Calibration a way of testing a measuring device with a known standard Significant figure convention Express all known digits with certainty plus one uncertain digit 0 If your measuring tool only measures to a tenth of a gram you would estimate to the hundredths place and that hundredths digit would be the uncertain digit Density is mass divided by volume United States Customary System USCS the system of measurement used in the United States Quantitative problem requires the manipulation of quantities Qualitative problem requires an analysis of the qualities of a substance and does not use calculations Rounding If the digit is 4 or below we leave the proceeding digit unchanged If the digit is 5 or more we increase the proceeding digit by 1 Significant Figure Rule for Addition and Subtraction Round the sum or difference to the highest value column Ex If you add 1375 15 and 166 you can only go to the tenths place with your final answer Significant Figure Rule for Manipulation and Division Count the number of sig figs in each value The answer can only have as many sig figs as the smallest amount of sig figs If multiplying something with 1 sig fig 3 sig figs and 100 sig figs the answer can only contain 1 sig fig Ex 110x2123 Relative Heaviness of a Substance This is called density It can be used to compare the mass of substances when they have the same volume Density is mass over volume Water has a density of 1000gL at 4 degrees C Practice Problems 1 a Add up the following Remember to use the sig fig rule for addition 1401 ft 11 ft 78096 ft 1508g 39 171g 13007g 2 An aluminum sphere has a mass of 1332 g A graduated cylinder is filled with water to the 351 mL mark When the marble is dropped into the cylinder the water rises to the 475 mL mark What is the marbles density Conversions to Become Familiar With Length ins 254 cm definition Mass lbs 45359237 g definition Volume gala 3785411784 L exactly USCSUSCS Conversion Length Mass Volume 1ft512in 1lbal6oz 1qt52pt ydE3ft 1qta32floz 1mi55280ft 1gals4qt This table should be memorized Practice Problem A 450 lb rectangular block has a density of 116 g cubic cm It is 451 in long and 609 in tall what is the width in inches How many quarts are in a tank that hold 68 liters How many pounds of gasoline are in a tank that is 15 m by 10 m by 57 m The density of gasoline is 07 gmL How many fluid ounces are in a tank that is 37 ft by 41 ft by 17 ft Lesson 5 How do Scientists Classify Matter Overview This lesson is about the different phases and changes matter can go through These changes can be physical or chemical This lesson also deals with the concepts of pure substance mixture element and compound This lesson is mainlyjust vocabulary that has to do with matter Vocabulary Water clear colorless odorless tasteless substance found almost everywhere on Earth it is essential to support life Petroleum thick flammable yellow to black substance found underground Petrochemical any subctance made from petroleum coal ir natural gas Petrochemical era started in the 19405 to present Solid a phase of matter which has a constant shape and volume 0 Ex ce Liquid a phase of matter which has variable shapes and constant volume 0 Ex Water Gas a phase of matter which has variable shapes and volume 0 Ex Water Vapor Pure substance a kind of matter composed of all of the same molecules which has distinct physical and chemical properties 0 Coffee or sugar Mixture matter that is comprised of two or more chemicals 0 Ex Coffee and sugar Element a pure substance that cannot be decomposed into any other pure substances 0 Ex Hydrogen Compound a pure substance that can be broken down into two or more pure substances 0 Ex Carbon Dioxide Physical property measureable and detectable by senses 0 Ex Color Physical change new form of the same substance 0 Ex Change form of matter Chemical property list of all chemical changes that are possible 0 Reactivity Chemical change new substance is formed 0 Something burning to form new chemicals Homogeneous uniform appearance and composition 0 Water Heterogeneous visibly different composition throughout 0 Dirt


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