...completes the statement or answers the question. 1) 1.00 mole of O2 contains the same number of molecules as A) 2.00 mole of CH3CH2 OH. C) all of the above. 1) B) 0.667 mole of O3 . D) 1.00 mole of CH3CO2H. SHORT ANSWER. Work must be shown for each problem as much as you can. Final answer only is not excepted (no woks no points) 2) How many oxygen atoms are in 3.00 g of sodium dichromate, Na2 Cr2 O7 ? 2) 3) What mass of sulfur hexafluoride, SF6, has the same number of fluorine atoms as 25.0 g of oxygen difluoride, OF2? 3) 4) Combustion analysis of 2.400 g of an unknown compound containing carbon, hydrogen, and oxygen produced 4.171 g of CO2 and 2.268 g of H2O. What is the empirical formula of the compound? 4) 5) How many Cl- ions are present in 50.0 g FeCl3? 5) 6) 200 pm is the same as __________ Å. 6) 1 7) The empirical formula of a compound with molecules containing 12 carbon atoms, 14 hydrogen atoms, and 6 oxygen atoms is __________. 7) 8) The charge on the manganese in the salt MnF3 is __________. 8) 9) The ions Ca 2+ and PO43- form a salt with the formula __________. 9) 10) The unit of force in the English measurement system is Newton, which is __________ in base SI units. lb · ft . The SI unit of force is the s2 10) 11) 45 m/s = __________ km/hr 11) 12) The correct answer (reported to the proper number of significant figures) to the following is __________. (12.67 + 19.2)(3.99) / (1.36 + 11.366)...
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...of the group project was to calculate the percent calcium in a natural calcium tablet from Prime Eastern Pharmaceuticals in order to compare it with the reported amount of 800 mg of calcium per tablet to determine the validity of complaints regarding a reduced amount of mineral in the multivitamin. The quantitative determination of the analyte was accomplished through three experiments: complexometric titrimetry, flame atomic absorption analysis, and potentiometry using an Ion Selective Electrode. The complexometric titrimetry involved titrating the unknown calcium solution made from the calcium tablet with standardized EDTA. Quantitative determination of the analyte calcium was possible due to the stable and quick formation of the metal-EDTA complex with a 1:1 reaction stoichiometry. Flame atomic absorption analysis is useful in determining the amount of analyte in an unknown because the measure absorbances of standard solutions can be used to plot a calibration curve that can be used to determine the concentration of the metal in an unknown solution. Potentiometry is useful for determination of analyte when an ion sensitive electrode is used to find the amount of ion in standard solutions. Week 1: Introduction and Background The first test for calcium in the multivitamin was complexometric titrimetry, a titration of a solution of calcium tablet with a standardized solution of EDTA. EDTA forms a stable complex with calcium metal with a reaction stoichiometry of 1:1, so an...
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...CHAPTER 3 MASS RELATIONSHIPS IN CHEMICAL REACTIONS This chapter reviews the mole concept, balancing chemical equations, and stoichiometry. The topics covered in this chapter are: • Atomic mass and average atomic mass • A vogadro’ s number, mole, and molar mass • Percent composition calculations • Empirical and molecular formula determinations • Chemical equations, amount of reactant and product calculations • Limiting reagents and reaction yield calculations Take Note: It is absolutely essential that you master the mole concept to do well on the quantitative aspects of AP Chemistry!! When solving quantitative problems on the Free Response section of the AP exam, supporting work must be shown to receive credit. Using dimensional analysis is a very powerful technique in solving problems. Be sure to report your answer to the correct number of significant figures (see Chapter 1 in this review book). Atomic mass and average atomic mass Atomic mass is the mass of an atom in atomic mass units (amu). One amu is defined as 1/12 of one C-12 atom. The C-12 isotope has a mass of exactly 12.000 amu. The C-12 isotope provides the relative scale for the masses of the other elements. Average atomic mass is the value reported on the periodic table, which takes into account the various isotopes of an element and their respective frequencies. To calculate the average atomic mass of an element, add up the different masses of the isotopes (using amu) multiplied by each isotope’s abundance...
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... Chapter 5—Gases 5.1: Substances That Exist as Gases Air: 78% N2, 21% O2, 1% Other (such as CO2) Ionic compounds do not exist as gases at 25 degrees Celsius as well as 1 atm (due to strong electrostatic forces holding cations/anions together in an ionic solid). The stronger the attractions (intermolecular forces), the less likely the compound can exist as a gas at ordinary temperatures. The characteristics of gases include: assuming the volume/shape of their containers, most compressible of the states of matter, will mix evenly/completely when confined in the same container, lower densities than liquids and solids. 5.2: Pressure of A Gas Gas molecules are constantly in motion, causing them to exert pressure with the surfaces they come in contact with. Pressure is known as the most readily measurable properties of a gas. SI Units of Pressure • Velocity is the change in distance with elapsed time. It uses the unit m/s or cm/s • Velocity = distance moved/elapsed time • Acceleration is the change in velocity with time. It uses the measurements of m/s2 or cm/s2 • Acceleration = change in velocity/elapsed time • Second law of motion is formulated by Newton and this law defines force as mass times acceleration. The SI unit for force is newton (N): 1 N equals 1 kg m/s2 • Pressure is the force applied per unit area. The SI unit for pressure is pascal (Pa): 1 Pa equals 1 N/m2 • Pressure = force/area Atmospheric Pressure • Air’s density decreases rapidly...
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...CARIBBEAN EXAMINATIONS COUNCIL Caribbean Secondary Education Certificate CSEC® CHEMISTRY SYLLABUS Effective for examinations from May–June 2015 CXC 21/G/SYLL 13 Published by the Caribbean Examinations Council. All rights reserved. No part of this publication may be reproduced, stored in a retrieval system, or transmitted in any form, or by any means electronic, photocopying, recording or otherwise without prior permission of the author or publisher. Correspondence related to the syllabus should be addressed to: The Pro-Registrar Caribbean Examinations Council Caenwood Centre 37 Arnold Road, Kingston 5, Jamaica Telephone Number: + 1 (876) 630-5200 Facsimile Number: + 1 (876) 967-4972 E-mail Address: cxcwzo@cxc.org Website: www.cxc.org Copyright © 2013 by Caribbean Examinations Council The Garrison, St Michael BB14038, Barbados CXC 21/G/SYLL 13 Contents RATIONALE ................................................................................................................................... AIMS ............................................................................................................................................. CANDIDATE POPULATION ............................................................................................................. SUGGESTED TIME-TABLE ALLOCATION ........................................................................................ ORGANISATION OF THE SYLLABUS .................................................
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...solution and standardization of hydrochloric acid To prepare a standard solution of sodium carbonate and use it to standardize a given solution of dilute hydrochloric acid. Anhydrous sodium carbonate is a suitable chemical for preparing a standard solution (as a primary standard). The molarity of the given hydrochloric acid can be found by titrating it against the standard sodium carbonate solution prepared. The equation for the complete neutralization of sodium carbonate with dilute hydrochloric acid is Na2CO3(aq) + 2HCl(aq) → 2NaCl(aq) + CO2(g) + H2O(l) The end-point is marked by using methyl orange as indicator. Introduction : Chemicals : Apparatus : Procedure : solid sodium carbonate, 0.1 M hydrochloric acid 1. 2. 3. 4. 5. 6. 7. 8. Weight out about 1.3 g of anhydrous sodium carbonate accurately using the method of “weighing by difference”. Transfer the weighed carbonate to a beaker and add about 100 cm3 of distilled water to dissolve it completely. After dissolving, transfer the solution to a 250.00 cm3 volumetric flask. Rinse the beaker thoroughly and transfer all the washes into the volumetric flask. Remember not to overshoot the graduation mark of the flask. Make up the solution to the mark on the neck by adding water. Pipette 25.00 cm3 of sodium carbonate solution to a clean conical flask. Add 2 drops of methyl orange indicator to the carbonate solution. Titrate the carbonate solution with the given dilute hydrochloric acid until the colour of solution just changes...
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...organic reserves dwindle, new sources of the organic chemicals presently used have to be found. In addition, chemists are continually searching for compounds to be used in the design and production of new materials to replace those that have been deemed no longer satisfactory for needs. This module increases students’ understanding of the implications of chemistry for society and the environment and the current issues, research and developments in chemistry. 1.1 Construct word and balanced formulae equations of all chemical reactions as they are encountered in this module: • Acid reactions: o acid (aq) + base (aq) salt (aq) + water (l) o acid (aq) + active metal (s) salt (aq) + hydrogen (g) o acid (aq) + metal carbonate (s) salt (aq) + water (l) + carbon dioxide (g) • Cracking of long chain alkanes (e.g. decane) to give a shorter chain alkene & alkane o Thermal cracking (heated with steam in absence of O2 to 750-900°C) Initiation: C10H22 2C5H11· Propagation: C5H11· C3H7· + C2H4 Termination: 2C3H7· C6H14 o Catalytic cracking zeolite (heated in absence of O2 to 500°C)...
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...10 CHAPTER SOLUTIONS MANUAL The Mole Section 10.1 Measuring Matter page 320–324 b. 2.50 ϫ 1020 atoms Fe 2.50 ؋ 1020 atoms Fe ؋ Practice Problems ؋ 51.4 ؍ 10؊4 1 mol Fe __ 6.02 ؋ 1023 atoms Fe mol Fe pages 323–324 1. Zinc (Zn) is used to form a corrosion-inhibiting surface on galvanized steel. Determine the number of Zn atoms in 2.50 mol of Zn. 2.50 mol Zn ؋ 4201 ؋ 15.1 ؍ ___ 6.02 ؋ 1023 atoms Zn 1 mol Zn atoms of Zn 2. Calculate the number of molecules in 11.5 mol of water (H2O). 11.5 mol H O ؋ ___ 6.02 ؋ 1023 molecules H2O 2 ؋ 29.6 ؍ 1024 1 mol H2O molecules of H2O 3. Silver nitrate (AgNO3) is used to make several Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. different silver halides used in photographic films. How many formula units of AgNO3 are there in 3.25 mol AgNO3? 3.25 mol AgNO3 ؋ 4201 ؋ 69.1 ؍ ____ 6.02 ؋ 1023 formula units AgNO3 1 mol AgNO3 formula units of AgNO3 4. Challenge Calculate the number of oxygen atoms in 5.0 mol of oxygen molecules. Oxygen is a diatomic molecule, O2. 5.00 mol O2 ؋ ___ 6.02 ؋ 1023 molecules O2 1 mol O2 2 O atoms ؋ __ 01 ؋ 20.6 ؍ 24 molecule O2 atoms O 5. How many moles contain each of the following? a. 5.75 ϫ 1024 atoms Al for each formula and convert the given number of representative particles to moles. a. 3.75 ϩ 1024 CO2 The representative particle is a molecule...
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... 3 1. Stoichiometry I. Balancing equations 4 2. Stoichiometry II. Calculation exercises 9 3. The gaseous state 13 4. Concentrations of solutions 17 5. Calculations connected to titrimetry 28 6. Electrolytic dissociation 33 7. Dilute solutions 38 8. Hydrogen ion concentration, pH, buffers 44 9. Heterogeneous equilibria. Crystallisation, solubility product, partition coefficient 55 10. Thermochemistry 64 11. Electrochemistry 67 2 INTRODUCTION The chapter is devoted to helping the students practice the most important topics of General Chemistry. The order of the sections follows the schedule of the lectures and seminars, and their volume indicates the importance of the topic. Each section begins with a few solved problems. They represent the minimum requirement at the exam. The worked-out solutions are not the only ones. For an easier self-checking, the numerical results of the unsolved calculation exercises are given in parentheses after each question. Sources: 1.) Laboratory experiments in medical chemistry, ed. György Oszbach, Pécs, 1998. 2.) Villányi Attila: Ötösöm lesz kémiából, (6. ed.) Mőszaki Könyvkiadó, Budapest., 1999 3.) Charles E. Mortimer, Ulrich Müller: Chemie- Das Basiswissen der Chemie (8.komplett überarbeitete und erweiterte Auflage), Thieme, 2003 4.) Villányi Attila: Kémia feladatgyőjtemény a kétszintő érettségire. Kemavill. Bt., Budapest, ...
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...Scientific Research and Essays Vol. 5(14), pp. 1796-1808, 18 July, 2010 Available online at http://www.academicjournals.org/SRE ISSN 1992-2248 ©2010 Academic Journals Review Biodiesel production from Jatropha curcas: A review Wilson Parawira Department of Applied Biology, Kigali Institute of Science and Technology (KIST), Avenue de I' Armee, B. P. 3900 Kigali, Rwanda, E-mail: aparawira@yahoo.co.uk. Tel: +250785561670. Accepted 2 July, 2010 Biodiesel has attracted considerable attention during the past decade as a renewable, biodegradable and non-toxic fuel alternative to fossil fuels. Biodiesel can be obtained from vegetable oils (both edible and non-edible) and from animal fat. Jatropha curcas Linnaeus, a multipurpose plant, contains high amount of oil in its seeds which can be converted to biodiesel. J. curcas is probably the most highly promoted oilseed crop at present in the world. The availability and sustainability of sufficient supplies of less expensive feedstock in the form of vegetable oils, particularly J. curcas and efficient processing technology to biodiesel will be crucial determinants of delivering a competitive biodiesel. Oil contents, physicochemical properties, fatty acid composition of J. curcas reported in literature are provided in this review. The fuel properties of Jatropha biodiesel are comparable to those of fossil diesel and confirm to the American and European standards. The objective of this review is to give an update on the J. curcas...
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...Physical Chemistry Understanding our Chemical World Physical Chemistry Understanding our Chemical World Paul Monk Manchester Metropolitan University, UK Copyright 2004 John Wiley & Sons Ltd, The Atrium, Southern Gate, Chichester, West Sussex PO19 8SQ, England Telephone (+44) 1243 779777 Email (for orders and customer service enquiries): cs-books@wiley.co.uk Visit our Home Page on www.wileyeurope.com or www.wiley.com All Rights Reserved. No part of this publication may be reproduced, stored in a retrieval system or transmitted in any form or by any means, electronic, mechanical, photocopying, recording, scanning or otherwise, except under the terms of the Copyright, Designs and Patents Act 1988 or under the terms of a licence issued by the Copyright Licensing Agency Ltd, 90 Tottenham Court Road, London W1T 4LP, UK, without the permission in writing of the Publisher. Requests to the Publisher should be addressed to the Permissions Department, John Wiley & Sons Ltd, The Atrium, Southern Gate, Chichester, West Sussex PO19 8SQ, England, or emailed to permreq@wiley.co.uk, or faxed to (+44) 1243 770620. This publication is designed to provide accurate and authoritative information in regard to the subject matter covered. It is sold on the understanding that the Publisher is not engaged in rendering professional services. If professional advice or other expert assistance is required, the services of a competent professional should be sought. Other Wiley...
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...AS/A Level GCE GCE Chemistry A OCR Advanced Subsidiary GCE in Chemistry A H034 OCR Advanced GCE in Chemistry A H434 Vertical black lines indicate a significant change to the previous printed version. © OCR 2008 version 2 – February 2008 QAN 500/2425/5 QAN 500/2347/0 Contents 1 About these Qualifications 1.1 1.2 1.3 1.4 1.5 The Three-Unit AS The Six-Unit Advanced GCE Qualification Titles and Levels Aims Prior Learning/Attainment 4 4 4 5 5 5 2 Summary of Content 2.1 2.2 AS Units A2 Units 6 6 7 3 Unit Content 3.1 3.2 3.3 3.4 3.5 3.6 AS Unit F321: Atoms, Bonds and Groups AS Unit F322: Chains, Energy and Resources AS Unit F323: Practical Skills in Chemistry 1 A2 Unit F324: Rings, Polymers and Analysis A2 Unit F325: Equilibria, Energetics and Elements A2 Unit F326: Practical Skills in Chemistry 2 8 8 20 38 40 51 62 4 Schemes of Assessment 4.1 4.2 4.3 4.4 4.5 4.6 4.7 4.8 AS GCE Scheme of Assessment Advanced GCE Scheme of Assessment Unit Order Unit Options (at AS/A2) Synoptic Assessment (A Level GCE) Assessment Availability Assessment Objectives Quality of Written Communication 64 64 65 66 66 66 67 67 68 5 Technical Information 5.1 5.2 5.3 5.4 5.5 5.6 5.7 5.8 5.9 Making Unit Entries Making Qualification Entries Grading Result Enquiries and Appeals Shelf-life of Units Unit and Qualification Re-sits Guided Learning Hours Code of Practice/Subject Criteria/Common Criteria Requirements Arrangements for Candidates with Particular...
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...How to go to your page This eBook set contains two volumes. The main content pages are contiguously numbered: use the Table of Contents to find those page numbers. The front matter pages and indices are labeled with the Volume number and page separated by a colon. For example, to go to page vi of Volume 1, type Vol1:vi in the “page #” box at the top of the screen and click “Go”. To go to page vi of Volume 2, type Vol2:vi in the "page #" box… and so forth. Encyclopedia of Human Body Systems This page intentionally left blank Encyclopedia of Human Body Systems VOLUME 1 Julie McDowell, Editor Copyright 2010 by ABC-CLIO, LLC All rights reserved. No part of this publication may be reproduced, stored in a retrieval system, or transmitted, in any form or by any means, electronic, mechanical, photocopying, recording, or otherwise, except for the inclusion of brief quotations in a review, without prior permission in writing from the publisher. Library of Congress Cataloging-in-Publication Data McDowell, Julie. Encyclopedia of human body systems / Julie McDowell. p. cm. Includes bibliographical references and index. ISBN 978–0–313–39175–0 (hard copy : alk. paper) 1. Human physiology—Encyclopedias. I. Title. QP11.M33 2011 612.003—dc22 2010021682 ISBN: 978–0–313–39175–0 EISBN: 978–0–313–39176–7 14 13 12 11 10 1 2 3 4 5 This book is also available on the World Wide Web as an eBook. Visit www.abc-clio.com for details. Greenwood An Imprint of ABC-CLIO, LLC ABC-CLIO, LLC...
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...Answers to Conceptual Integrated Science End-of-Chapter Questions Chapter 1: About Science Answers to Chapter 1 Review Questions 1 The era of modern science in the 16th century was launched when Galileo Galilei revived the Copernican view of the heliocentric universe, using experiments to study nature’s behavior. 2 In Conceptual Integrated Science, we believe that focusing on math too early is a poor substitute forconcepts. 3 We mean that it must be capable of being proved wrong. 4 Nonscientific hypotheses may be perfectly reasonable; they are nonscientific only because they are not falsifiable—there is no test for possible wrongness. 5 Galileo showed the falseness of Aristotle’s claim with a single experiment—dropping heavy and lightobjects from the Leaning Tower of Pisa. 6 A scientific fact is something that competent observers can observe and agree to be true; a hypothesis is an explanation or answer that is capable of being proved wrong; a law is a hypothesis that has been tested over and over and not contradicted; a theory is a synthesis of facts and well-tested hypotheses. 7 In everyday speech, a theory is the same as a hypothesis—a statement that hasn’t been tested. 8 Theories grow stronger and more precise as they evolve to include new information. 9 The term supernatural literally means “above nature.” Science works within nature, not above it. 10 They rely on subjective personal experience and do not lead to testable hypotheses. They lie outside...
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...Chemistry Modern Analytical Chemistry David Harvey DePauw University Boston Burr Ridge, IL Dubuque, IA Madison, WI New York San Francisco St. Louis Bangkok Bogotá Caracas Lisbon London Madrid Mexico City Milan New Delhi Seoul Singapore Sydney Taipei Toronto McGraw-Hill Higher Education A Division of The McGraw-Hill Companies MODERN ANALYTICAL CHEMISTRY Copyright © 2000 by The McGraw-Hill Companies, Inc. All rights reserved. Printed in the United States of America. Except as permitted under the United States Copyright Act of 1976, no part of this publication may be reproduced or distributed in any form or by any means, or stored in a data base or retrieval system, without the prior written permission of the publisher. This book is printed on acid-free paper. 1 2 3 4 5 6 7 8 9 0 KGP/KGP 0 9 8 7 6 5 4 3 2 1 0 ISBN 0–07–237547–7 Vice president and editorial director: Kevin T. Kane Publisher: James M. Smith Sponsoring editor: Kent A. Peterson Editorial assistant: Jennifer L. Bensink Developmental editor: Shirley R. Oberbroeckling Senior marketing manager: Martin J. Lange Senior project manager: Jayne Klein Production supervisor: Laura Fuller Coordinator of freelance design: Michelle D. Whitaker Senior photo research coordinator: Lori Hancock Senior supplement coordinator: Audrey A. Reiter Compositor: Shepherd, Inc. Typeface: 10/12 Minion Printer: Quebecor Printing Book Group/Kingsport Freelance cover/interior designer: Elise Lansdon Cover image: © George Diebold/The...
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