DOCSLIB.ORG

CALCULATING DENSITY Density of Common Metals Copper 8.96 G/Cm

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text
CALCULATING DENSITY Density of Common Metals Copper 8.96 G/Cm NAME __________________________________________ PER _______________ CALCULATING DENSITY Density of Common Metals Copper 8.96 g/cm3 Gold 19.32 g/cm3 Iron 7.87 g/cm3 Lead 11.36 /cm3 1. A substance has a mass of 1370.3 grams (g) and a volume of 71 cubic centimeters (cm3). Using the table above, what is this substance? A Iron B Lead C Gold D Copper 2. A substance has a mass of 375 grams (g) and a volume of 47.65 cm3. Using the table above, what is this substance? A Iron B Lead C Gold D Copper For questions 3 – 9, calculate the density and fill in the table. 10. What has the greater density, a cube of water measuring 1cmX1cmX1cm and having a mass of 1g, or a block of plastic measuring 2cmX3cmX1cm with a mass of 4g? A Cube of water B Block of plastic 11. A rock has a volume 57 cm3. Its mass is 14. Sam has to find the density of an 555.75 g. What is the density of this rock? irregularly shaped solid. The mass of the solid is 300.3 g. She uses water displacement to find the volume. The volume of the water alone is 100 mL. The volume of the water with the solid in it is 142 mL. What is the density of the solid? 12. Joe has to find the density of a rectangular box. He measures the width to be 6 cm, the length to be 7 cm, and the height to be 2 cm. He put the box on a balance and the mass is 15. Based on the table below, what is the 198.24 g. What is the density of the box? irregularly shaped solid in question 14 likely made of? __________________________________ Substance Average Density Aluminum 2.7 g/cm3 Titanium 4.5 g/cm3 3 Chromium 7.15 g/cm 13. We need to find the density of a cube of Silver 10.49 g/cm3 plastic that has sides measuring 4 cm. The mass of the cube is 279.744 g. What is the density of the cube? 16. Mr. Odum wants to know if his watch band is titanium or silver. He measures the mass of his watch band to be 90 g. The volume of his watch band is 20 cm3. Using the table above, _____________________________________ what is his watch band likely made of? _____________________________________ Use the table to help you answer questions 17 –21. 19. Mr. Valamides brought his cuff links down to 6th grade Science to find out if they were really the Metal Average Density metal that he thought they were. We found the Lithium 0.53 g/cm3 mass to be 720.25 g. When we put the cuff links Beryllium 1.85 g/cm3 into a graduated cylinder with 100 mL of water in it, the water rose 33.5 mL. Mr. Valamides was very Gallium 5.91 g/cm3 happy with the result because he knew the metal Tin 7.26 g/cm3 was ______________________________. Nickel 8.92 g/cm3 Palladium 12.0 g/cm3 Platinum 21.5 g/cm3 20. Mr. Odum was teaching Mrs. Burch how to find the volume of an unknown metal using water displacement. The picture below shows what Mrs. 17. The mass of an unknown metal is 222.5 g. Burch saw. Mrs. de Leon used water displacement to measure the volume of the mineral. The picture below shows the volume in mL before and after the metal was added to the graduated cylinder. Find the volume and then the density. Use the table above to identify the metal. The metal is _____________________________ Mrs. Burch measured the mass of the metal and the balance read 145.2 g. Mrs. Burch used the table to identify the mineral as Gallium. Was she correct? ____________ 21. Ms. Blackmon brings in a metal that she thinks is Palladium. She gives it to Mrs. de Leon so that 18. Mr. Odum measured the next metal and found she can find out for sure. The mass of the metal is 163.8 g. The volume is 13.65 mL. Does Ms. the volume was 27 mL and mass was 14.31 g. Calculate density, then use the table above. Blackmon have the metal that she thinks she has? The metal is __________________________ __________________ Part One: Calculate the densities of the following substances and write the densities in the table. MASS VOLUME DENSITY (g/mL) SUBSTANCE 22) 12.42 g 6 mL 23) 12.19 g 23 mL 24) 11.766 g 5.3 mL 25) 7.76 g 8 mL 26) 0.783 g 0.45 mL 27) 3.02 g 2 mL 28) 13.95 g 9 mL 29) 40.137 g 5.1 mL 30) 79.21 g 8.9 mL 31) 52.45 g 5 mL Part Two: You have just figured the densities of known substances. Look up the densities in the table below and write the corresponding substance in the table above. NAME DENSITY NAME DENSITY Aluminum 2.699 g/mL Magnesium 1.74 g/mL Arsenic 5.73 g/mL Mercury 13.55 g/ cm3 Calcium 1.55 g/ cm3 Nickel 8.9 g/mL Carbon 2.22 g/mL Platinum 21.45 g/ cm3 Chlorine 1.51 g/mL Potassium 0.86 g/mL Gold 19.32 g/ cm3 Silver 10.49 g/mL Iodine 4.93 g/mL Sodium 0.97 g/mL Iron 7.87 g/mL Sulfur 2.07 g/ cm3 Lead 11.34 g/ cm3 Lithium 0.53 g/mL .
Load more

Recommended publications
  • Exploring Density
    Exploring Density Students investigate the densities of different liquids and solids and understand how density may help identify a substance. Suggested Grade Range: 6-8 Approximate Time: 1 hour Relevant National Content Standards: Next Generation Science Standards Science and Engineering Practices: Developing and using Models Modeling in 6–8 builds on K–5 experiences and progresses to developing, using, and revising models to describe, test, and predict more abstract phenomena and design systems. • Develop and use a model to describe phenomena. Science and Engineering Practices: Analyzing and Interpreting Data Analyzing data in 6-8 builds on K-5 and progresses to extending quantitative analysis to investigations, distinguishing between correlation and causation, and basic statistical techniques of data and error analysis. • Analyze and interpret data to determine similarities and differences in findings. Disciplinary Core Ideas: PS1.A Structure and Properties of Matter Each pure substance has characteristic physical and chemical properties (for any bulk quantity under given conditions) that can be used to identify it. Common Core State Standard: 7NS 2. Apply and extend previous understanding of multiplication and division and of fractions to multiply and divide rational numbers. 3. Solve real-world and mathematical problems involving the four operations with rational numbers. Common Core State Standard: 7EE Solve real-life and mathematical problems using numerical and algebraic expressions and equations. 4. Use variables to represent
    [Show full text]
  • Glossary of Terms
    GLOSSARY OF TERMS For the purpose of this Handbook, the following definitions and abbreviations shall apply. Although all of the definitions and abbreviations listed below may have not been used in this Handbook, the additional terminology is provided to assist the user of Handbook in understanding technical terminology associated with Drainage Improvement Projects and the associated regulations. Program-specific terms have been defined separately for each program and are contained in pertinent sub-sections of Section 2 of this handbook. ACRONYMS ASTM American Society for Testing Materials CBBEL Christopher B. Burke Engineering, Ltd. COE United States Army Corps of Engineers EPA Environmental Protection Agency IDEM Indiana Department of Environmental Management IDNR Indiana Department of Natural Resources NRCS USDA-Natural Resources Conservation Service SWCD Soil and Water Conservation District USDA United States Department of Agriculture USFWS United States Fish and Wildlife Service DEFINITIONS AASHTO Classification. The official classification of soil materials and soil aggregate mixtures for highway construction used by the American Association of State Highway and Transportation Officials. Abutment. The sloping sides of a valley that supports the ends of a dam. Acre-Foot. The volume of water that will cover 1 acre to a depth of 1 ft. Aggregate. (1) The sand and gravel portion of concrete (65 to 75% by volume), the rest being cement and water. Fine aggregate contains particles ranging from 1/4 in. down to that retained on a 200-mesh screen. Coarse aggregate ranges from 1/4 in. up to l½ in. (2) That which is installed for the purpose of changing drainage characteristics.
    [Show full text]
  • Carbon Dioxide
    Safetygram 18 Carbon dioxide Carbon dioxide is nonflammable, colorless, and odorless in the gaseous and liquid states. Carbon dioxide is a minor but important constituent of the atmosphere, averaging about 0.036% or 360 ppm by volume. It is also a normal end-prod- uct of human and animal metabolism. Dry carbon dioxide is a relatively inert gas. In the event moisture is present in high concentrations, carbonic acid may be formed and materials resistant to this acid should be used. High flow rates or rapid depressurization of a system can cause temperatures approaching the sublimation point (–109.3°F [–78.5°C]) to be attained within the system. Carbon dioxide will convert directly from a liquid to a solid if the liquid is depressurized below 76 psia (61 psig). The use of ma- terials which become brittle at low temperatures should be avoided in applications where temperatures less than –20°F (–29°C) are expected. Vessels and piping used in carbon dioxide service should be designed to the American Society of Mechanical Engineers (ASME) or Department of Transportation (DOT) codes for the pressures and temperatures involved. Physical properties are listed in Table 1. Carbon dioxide in the gaseous state is colorless and odorless and not easily detectable. Gaseous carbon dioxide is 1.5 times denser than air and therefore is found in greater concentrations at low levels. Ventilation systems should be designed to exhaust from the lowest levels and allow make-up air to enter at a higher level. Manufacture Carbon dioxide is produced as a crude by-product of a number of manufactur- ing processes.
    [Show full text]
  • Guidelines for the Use of Atomic Weights 5 10 11 12 DOI: ..., Received ...; Accepted
    IUPAC Guidelines for the us e of atomic weights For Peer Review Only Journal: Pure and Applied Chemistry Manuscript ID PAC-REC-16-04-01 Manuscript Type: Recommendation Date Submitted by the Author: 01-Apr-2016 Complete List of Authors: van der Veen, Adriaan; VSL Meija, Juris Possolo, Antonio; National Institute of Standards and Technology Hibbert, David; University of New South Wales, School of Chemistry atomic weights, atomic-weight intervals, molecular weight, standard Keywords: atomic weight, measurement uncertainty, uncertainty propagation Author-Supplied Keywords: P.O. 13757, Research Triangle Park, NC (919) 485-8700 Page 1 of 13 IUPAC Pure Appl. Chem. 2016; aop 1 2 3 4 Sponsoring body: IUPAC Inorganic Chemistry Division Committee: see more details on page XXX. 5 IUPAC Recommendation 6 7 Adriaan M. H. van der Veen*, Juris Meija, Antonio Possolo, and D. Brynn Hibbert 8 9 Guidelines for the use of atomic weights 5 10 11 12 DOI: ..., Received ...; accepted ... 13 14 Abstract: Standard atomicFor weights Peer are widely used Review in science, yet the uncertainties Only associated with these 15 values are not well-understood. This recommendation provides guidance on the use of standard atomic 16 weights and their uncertainties. Furthermore, methods are provided for calculating standard uncertainties 17 of molecular weights of substances. Methods are also outlined to compute material-specific atomic weights 10 18 whose associated uncertainty may be smaller than the uncertainty associated with the standard atomic 19 weights. 20 21 Keywords: atomic weights; atomic-weight intervals; molecular weight; standard atomic weight; uncertainty; 22 uncertainty propagation 23 24 25 1 Introduction 15 26 27 Atomic weights provide a practical link the SI base units kilogram and mole.
    [Show full text]
  • The Water Molecule
    Seawater Chemistry: Key Ideas Water is a polar molecule with the remarkable ability to dissolve more substances than any other natural solvent. Salinity is the measure of dissolved inorganic solids in water. The most abundant ions dissolved in seawater are chloride, sodium, sulfate, and magnesium. The ocean is in steady state (approx. equilibrium). Water density is greatly affected by temperature and salinity Light and sound travel differently in water than they do in air. Oxygen and carbon dioxide are the most important dissolved gases. 1 The Water Molecule Water is a polar molecule with a positive and a negative side. 2 1 Water Molecule Asymmetry of a water molecule and distribution of electrons result in a dipole structure with the oxygen end of the molecule negatively charged and the hydrogen end of the molecule positively charged. 3 The Water Molecule Dipole structure of water molecule produces an electrostatic bond (hydrogen bond) between water molecules. Hydrogen bonds form when the positive end of one water molecule bonds to the negative end of another water molecule. 4 2 Figure 4.1 5 The Dissolving Power of Water As solid sodium chloride dissolves, the positive and negative ions are attracted to the positive and negative ends of the polar water molecules. 6 3 Formation of Hydrated Ions Water dissolves salts by surrounding the atoms in the salt crystal and neutralizing the ionic bond holding the atoms together. 7 Important Property of Water: Heat Capacity Amount of heat to raise T of 1 g by 1oC Water has high heat capacity - 1 calorie Rocks and minerals have low HC ~ 0.2 cal.
    [Show full text]
  • Measuring Density
    Measuring Density Background All matter has mass and volume. Mass is a measure of the amount of matter an object has. Its measure is usually given in grams (g) or kilograms (kg). Volume is the amount of space an object occupies. There are numerous units for volume including liters (l), meters cubed (m3), and gallons (gal). Mass and volume are physical properties of matter and may vary with different objects. For example, it is possible for two pieces of metal to be made out of the same material yet for one piece to be bigger than the other. If the first piece of metal is twice as large as the second, then you would expect that this piece is also twice as heavy (or have twice the mass) as the first. If both pieces of metal are made of the same material the ratio of the mass and volume will be the same. We define density (ρ) as the ratio of the mass of an object to the volume it occupies. The equation is given by: M ρ = (1.1) V here the symbol M stands for the mass of the object, and V the volume. Density has the units of mass divided by volume such as grams per centimeters cube (g/cm3) or kilograms per liter (kg/l). Sample Problem #1 A block of wood has a mass of 8 g and occupies a volume of 10 cm3. What is its density? Solution 8g The density will be = 0.8g / cm 3 . 10cm 3 This means that every centimeter cube of this wood will have a mass of 0.8 grams.
    [Show full text]
  • Density Objective Learn How to Calculate Density
    Density Objective Learn how to calculate density Density is a way of comparing the mass of an object to its size (volume). If an object feels heavy for its size, it has a high density. A dense object has more material (atoms) packed into a smaller area. Density cannot be measured directly, it must be calculated. The formula used to calculate density is density = mass/volume or D = m/v. The typical label for density is g/mL or g/cm3. Density is a useful tool for scientist. It is often used to help identify a pure substance. A pure substance will have one unique density. For example, each element on the periodic table has a density from any other element. If you had an unknown gas, you could calculate the density of it to identify it. The same is true for minerals- though several minerals may have the same density so other properties would also need to be used to identify the mineral. If you have ever noticed oil floating on water, that is an example of density. Objects that are less dense than water, it will float. Waters density is 1.0g/mL. 1. In general terms, describe what density is. 2. How could density be used to identify an unknown substance? 3. Density must be calculated using a math formula. What is the formula for density? 4. What is a typical label for density? *Obviously both water and ice are the same substance- so should have the same density. But does it? Then why does ice float? Suggest an explanation.
    [Show full text]
  • DENSITY and SPECIFIC GRAVITY Most Students Have Felt How Heavy
    DENSITY and SPECIFIC GRAVITY Most students have felt how heavy “normal” rocks and minerals are. But many have never handled especially light minerals such as borax, or very heavy ones, such as a nugget of pure gold. This gives you an opportunity to surprise them, for some of the lightest and heaviest (more correctly, least and most dense) solids known are to be found among our naturally occurring minerals. Many ore minerals can be used to teach about these properties. Density and Specific Gravity defined Density is expressed in terms of mass per unit volume. The density of water, often used for comparisons, can be expressed as 1.0 g/cm3 or 1,000 kg/m3. Mineralogists often use the unit-less measurements of specific gravity, which is the density of a mineral relative to that of an equivalent volume of water. A mineral that weighs four times as much as water has a specific gravity (abbreviated SG) of 4.0. Here is one example. Galena (chemically, lead sulfide) has long been mined for the lead, which was widely used in Roman times to make water pipes. (The Latin name, plumbum, is the origin of the English word plumbing, although modern pipes are not made with lead.) Galena often occurs with perfect cubic cleavage. If you were to make a cube of pure galena measuring exactly 1.0 cm on a side and place that cube on a laboratory balance, you would find that its mass is 7.58 g—its density is 7.58 g/cm3, and its specific gravity is: 7.58 g/cm3 ÷ 1.0 g/cm3 = 7.58 Densities of minerals Most common minerals in Earth’s crust have specific gravities ranging from 2.6 to 2.8.
    [Show full text]
  • International Alloy Designations and Chemical Composition Limits for Wrought Aluminum and Wrought Aluminum Alloys
    International Alloy Designations and Chemical Composition Limits for Wrought Aluminum and Wrought Aluminum Alloys 1525 Wilson Boulevard, Arlington, VA 22209 www.aluminum.org With Support for On-line Access From: Aluminum Extruders Council Australian Aluminium Council Ltd. European Aluminium Association Japan Aluminium Association Alro S.A, R omania Revised: January 2015 Supersedes: February 2009 © Copyright 2015, The Aluminum Association, Inc. Unauthorized reproduction and sale by photocopy or any other method is illegal . Use of the Information The Aluminum Association has used its best efforts in compiling the information contained in this publication. Although the Association believes that its compilation procedures are reliable, it does not warrant, either expressly or impliedly, the accuracy or completeness of this information. The Aluminum Association assumes no responsibility or liability for the use of the information herein. All Aluminum Association published standards, data, specifications and other material are reviewed at least every five years and revised, reaffirmed or withdrawn. Users are advised to contact The Aluminum Association to ascertain whether the information in this publication has been superseded in the interim between publication and proposed use. CONTENTS Page FOREWORD ........................................................................................................... i SIGNATORIES TO THE DECLARATION OF ACCORD ..................................... ii-iii REGISTERED DESIGNATIONS AND CHEMICAL COMPOSITION
    [Show full text]
  • Eureka! Density! by Cindy Grigg
    Eureka! Density! By Cindy Grigg 1 What is density? Density is simply the amount of "stuff" in a given space. Scientists measure density by dividing the mass of something by its volume (d = m/v). This is a story about how the concept of density was first "discovered." 2 It is the story of a Greek mathematician named Archimedes who lived around 250 B.C. The King of Syracuse, where Archimedes lived, thought that he was being cheated by the metal craftsman who made his golden crown. The King called Archimedes to him and gave him the task of finding out whether the craftsman had replaced some of the gold in the King's crown with silver. Silver was worth less money than gold, and it also was an insult to the King to be wearing a crown that was not pure gold. 3 The King gave Archimedes some rules. Archimedes could not damage the crown in any way. He could not melt down the crown to see if it was made of other metals. He could not scratch the crown to see if there was silver underneath the golden outside. Archimedes thought about the problem while taking a bath. As he entered the bathing pool, he noticed that water spilled over the sides of the pool. He realized that the amount of water that spilled was equal in volume to the space that his body occupied. This fact suddenly provided him with a method for finding out if the King's crown was made of pure gold. 4 Archimedes knew that silver is not as "heavy" as gold.
    [Show full text]
  • Handbook for the Application of the Caesium-137 Technique
    Use of Caesium - 3 7 as a Tracer of XA04N1922 Erosion and Sedimentation: Handbook for the Application of the Caesium-137 Technique fNIS-XA-N-- 79 UK Overseas Development Administration Research Scheme R4579 .4T. te, October 1993 D.E. Walling C,- TA. uIlIc Department o'Geqqi-apky, nhei-slty of Exctc;-. Use of Caesium-137 as a Tracer of Erosion and Sedimentation: Handbook for the Application of the Caesium-137 Technique. UK Overseas Development Administration Research Scheme R4579 D.E.Walling & T.A.Ouine October 1993 Department of Geography University of Exeter Contents Part I Methodology Chapter Soil Erosion - The Problem and its Assessment 1.1 The Impacts of Soil Erosion 1.1.1 On-site impact on agricultural productivitV. 1.1.2 Off-siteimpactsoterodedsediment. 1.2 The Data Requirement 1.2.1 Data required to assess the impact on productiv 1.2.2 Data required to assess the off-site impact 1.2.3 Data required to target conservation resources 1.3 Current Methods of Erosion Assessment and the Resultant Data 1.3.1 Long-term monitoring of experimental plots 1.3.2 Field survey of erosion features 1.3.3 Erosion modelling 1.4 Meeting the Data Requirements 1.5 The Potential of the Caesium- 137 Technique 1.6 References Chapter 2 The Caesium-137 Technique 2.1 The Basis of the Caesium-137 Technique 2.2 The Source of Caesium-137 in the Environment 2.3 Deposition of Caesium-137 2.3.1 Bomb-derived caesium-137 2.3.2 ChernobVI-derived caesium-137 2.4 Caesium-137 adsorption by mineral sediment 2.4.1 Experimental studies 2.4.2 Field studies 2.5 Sediment-associated redistribution of caesium-1 37 2.5.1 Field evidence 2.6 Use of Caesium-137 Measurements in Erosion Assessment 2.7 Establishment of a Reference Inventory 2.8 Measurement of the Spatial Distribution of Caesiurn- 1 37 2.9 Identification of Caesium-137 Redistribution 2.10 Development of 'Calibration' Procedures 2.11 Estimation of Erosion and Aggradation Rates 2.12 Summary 2.13 References Chapter 3 Sample Collection, Preparation and Analysis 3.1 Sample Collection 3.
    [Show full text]
  • Press and Sintering of Titanium
    Press and sintering of titanium Robert Frykholma * and Benjamin Brashb Höganäs AB, SE-263 83 Höganäs, Sweden [email protected], [email protected] Keywords: Compaction, Titanium hydride, Densification keyword index. Abstract. Titanium based alloys show very high strength to density ratio, and could be the choice of material for a wide range of applications. By practicing press and sintering for production of Ti components, high materials utilization can be assured, and at the same time costly machining operations can be limited. Difficulties in processing and high cost for powders have been limiting factors for progress, but recent development indicates good possibilities on cost effective use of TiH2 powder in the press and sintering segment. In this paper, influence of processing parameters and powder properties on final sintered component properties are discussed. Introduction Titanium alloys and near net shape processing is a very attractive combination since it allows good material utilization, and difficult and expensive machining operations can be avoided. However, high material cost has been a limiting factor, and applications have mainly been found in aerospace and medical sectors. More and more efforts have during the last years been put into development of processes for production of so called low-cost titanium powder, where the aim is set to reduce powder cost by more than 70% compared to atomized powder. With low-cost powders new application areas, such as automotive where low weight and high performance is of interest, could open up. Powder techniques for component manufacturing where Ti alloys are used today are e.g. metal injection molding (MIM), and additive manufacturing (AM).
    [Show full text]