N12/4/CHEMI/SPM/ENG/TZ0/XX 88126104 CHEMISTRY standard level Paper 1 Friday 9 November 2012 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES • Do not open this examination paper until instructed to do so. • Answer all the questions. • For each question‚ choose the answer you consider to be the best and indicate your choice on the answer sheet provided. • The periodic table is provided for reference on page 2 of this examination paper. • The maximum mark for this examination
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– of the second substance in the same reaction takes place. On the other hand‚ acid-base reaction is when a solution of known molarity2 and volume present in a conical flask is titrated against a solution of unknown molarity in a burette until neutralization is reached. As I have shown in eq.1‚ in this investigation it was an acid reacting with a base‚ hence‚ an acid-base titration. eq.1 – Hydrochloric Acid + Sodium hydroxide Sodium Chloride + water HCl(aq)
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This value is then placed over 1 mL of the t-pentyl alcohol so it can be converted into grams. In order to convert from grams to moles‚ t-pentyl alcohol is multiplied by 1 mole of t-pentyl alcohol and this value is placed over the molar mass of t-pentyl alcohol‚ 88.2 grams. This value is then multiplied by 1 mole of t-pentyl chloride over 1 mole of t-pentyl alcohol to get the theoretical yield‚ .201 moles of t-pentyl
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Chemistry‚ 2014 UNIT 1 – MATTER TRENDS AND CHEMICAL BONDING History of the atom DEMOCRITUS Smallest particle of matter is called an atom Atoms are in constant motion and have empty space between them ARISTOTLE 4 element theory of matter (earth‚ air‚ water‚ fire) Had different combinations of the 4 qualities: hot‚ cold‚ dry‚ moist JOHN DALTON Expanded on Democritus’s theory: All matter is composed of tiny‚ indivisible particles All atoms of an element have identical properties
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carry 5 marks each. (vii) Use Log Tables‚ if necessary‚ Use of calculators is not allowed. QUESTION PAPER CODE 56/1/1 1. 2. ’Crystalline solids are anisotropic in nature.’ What does this statement mean? Express the relation between conductivity and molar conductivity of a solution held in a cell. Define ’electrophoresis’. Draw the structure of XeF2 molecule. Write the IUPAC name of the following compound: (CH3)3 CCH2Br 6. 7. Draw the structure of 3-methylbutanal. Arrange the following compounds in
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Enthalpy changes can be calculated using average bond enthalpy data. i) The enthalpy change to convert methane into gaseous atoms is shown below. [pic] Calculate the average bond enthalpy of a C—H bond in methane. [1] ii) Use the data in the table below and your answer to (a)(i) to calculate the enthalpy change for [pic] [3] [pic] b) The standard enthalpy of formation of 1‚2-dibromoethane‚ CH2BrCH2Br‚ is – 37.8 kJmol-1. Suggest the main reason for
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T‚ ∅ is the rate of heating and R is the universal gas constant. The left‐hand side of equation (3) is plotted against 1/T‚ since (1-2RT/E^* ) ≈ 1. E^≠ was estimated from a slope of this plot. A was calculated from the intercept of this plot. The enthalpy of activation (∆H^≠)‚ the entropy
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A. MATTER * Nature of matter. * Describe the states of matter and explain their conversion in terms of the kinetic particle theory. * Describe and explain diffusion. * Describe dependence of rate of diffusion on molecular mass‚ qualitatively. * Experimental techniques Measurement. * Name appropriate apparatus for the measurement of time‚ temperature‚ mass and volume‚ including burettes‚ pipettes and measuring cylinders. Criteria of purity. * Identify substances
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Complete Solutions Manual GENERAL CHEMISTRY NINTH EDITION Ebbing/Gammon David Bookin Mt. San Jacinto College Darrell D. Ebbing Wayne State University‚ Emeritus Steven D. Gammon Western Washington University HOUGHTON MIFFLIN COMPANY BOSTON NEW YORK Vice President and Executive Publisher: George Hoffman Vice President and Publisher: Charles Hartford Senior Marketing Manager: Laura McGinn Development Editor: Kate Heinle Assistant Editor: Amy Galvin Editorial Assistant: Chip
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Chapter 5: Solutions‚ Colloids‚ and Membranes Chapter Summary Mixtures and Solutions * A mixture maintains its identity regardless of the proportions of its components. * A mixture can be separated into its pure components through physical separation techniques. * The components are distributed uniformly throughout a homogenous mixture. * The components are not distributed uniformly throughout a heterogeneous mixture. * A solution is composed of a solvent and one or more solutes
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