File "HL-paper2.html"
Path: /IB QUESTIONBANKS/4 Fourth Edition - PAPER/HTML/Chemistry/Option A/HL-paper2html
File size: 20.03 KB
MIME-type: text/html
Charset: utf-8
<!DOCTYPE html>
<html>
<meta http-equiv="content-type" content="text/html;charset=utf-8">
<head>
<meta charset="utf-8">
<title>IB Questionbank</title>
<link rel="stylesheet" media="all" href="css/application-746ec5d03ead8d9e8b3bb7d32173f2b4e2e22a05f0c5278e086ab55b3c9c238e.css">
<link rel="stylesheet" media="print" href="css/print-6da094505524acaa25ea39a4dd5d6130a436fc43336c0bb89199951b860e98e9.css">
<script src="js/application-3c91afd8a2942c18d21ed2700e1bdec14ada97f1d3788ae229315e1276d81453.js"></script>
<script type="text/javascript" async src="https://cdnjs.cloudflare.com/ajax/libs/mathjax/2.7.5/MathJax.js?config=TeX-MML-AM_CHTML-full"></script>
<!--[if lt IE 9]>
<script src='https://cdnjs.cloudflare.com/ajax/libs/html5shiv/3.7.3/html5shiv.min.js'></script>
<![endif]-->
<meta name="csrf-param" content="authenticity_token">
<meta name="csrf-token" content="iHF+M3VlRFlNEehLVICYgYgqiF8jIFlzjGNjIwqOK9cFH3ZNdavBJrv/YQpz8vcspoICfQcFHW8kSsHnJsBwfg==">
<link href="favicon.ico" rel="shortcut icon">
</head>
<body class="teacher questions-show">
<div class="navbar navbar-fixed-top">
<div class="navbar-inner">
<div class="container">
<div class="brand">
<div class="inner"><a href="http://ibo.org/">ibo.org</a></div>
</div>
<ul class="nav">
<li>
<a href="../../index.html">Home</a>
</li>
<li class="active dropdown">
<a class="dropdown-toggle" data-toggle="dropdown" href="#">
Questionbanks
<b class="caret"></b>
</a><ul class="dropdown-menu">
<li>
<a href="../../geography.html" target="_blank">DP Geography</a>
</li>
<li>
<a href="../../physics.html" target="_blank">DP Physics</a>
</li>
<li>
<a href="../../chemistry.html" target="_blank">DP Chemistry</a>
</li>
<li>
<a href="../../biology.html" target="_blank">DP Biology</a>
</li>
<li>
<a href="../../furtherMath.html" target="_blank">DP Further Mathematics HL</a>
</li>
<li>
<a href="../../mathHL.html" target="_blank">DP Mathematics HL</a>
</li>
<li>
<a href="../../mathSL.html" target="_blank">DP Mathematics SL</a>
</li>
<li>
<a href="../../mathStudies.html" target="_blank">DP Mathematical Studies</a>
</li>
</ul></li>
<!-- - if current_user.is_language_services? && !current_user.is_publishing? -->
<!-- %li= link_to "Language services", tolk_path -->
</ul>
<ul class="nav pull-right">
<li>
<a href="https://06082010.xyz">IB Documents (2) Team</a>
</li></ul>
</div>
</div>
</div>
<div class="page-content container">
<div class="row">
<div class="span24">
</div>
</div>
<div class="page-header">
<div class="row">
<div class="span16">
<p class="back-to-list">
</p>
</div>
<div class="span8" style="margin: 0 0 -19px 0;">
<img style="width: 100%;" class="qb_logo" src="images/logo.jpg" alt="Ib qb 46 logo">
</div>
</div>
</div><h2>HL Paper 2</h2><div class="specification">
<p class="p1">Esters and amides can be produced by condensation reactions.</p>
</div>
<div class="specification">
<p class="p1">Under certain conditions but-2-ene can react with water to form butan-2-ol.</p>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p class="p1">State the names of <strong>two </strong>organic compounds required to produce ethyl methanoate and state suitable reaction conditions.</p>
<div class="marks">[2]</div>
<div class="question_part_label">a.i.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p class="p1">Deduce the structure of the simplest repeating unit of the polymer formed from the reaction between 1,6-diaminohexane and hexane-1,6-dioic acid and state <strong>one </strong>use of this product.</p>
<div class="marks">[3]</div>
<div class="question_part_label">a.ii.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p class="p1">State and explain how the rate of step <strong>II </strong>would differ if 2-chlorobutane was used instead of 2-bromobutane.</p>
<div class="marks">[1]</div>
<div class="question_part_label">b.iii.</div>
</div>
<br><hr><br><div class="specification">
<p class="p1">Ethanol has many industrial uses.</p>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p class="p1">State an equation for the formation of ethanol from ethene and the necessary reaction conditions.</p>
<p class="p1">Equation:</p>
<p class="p1"> </p>
<p class="p1">Conditions:</p>
<div class="marks">[3]</div>
<div class="question_part_label">a.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p class="p1">Define the term <em>average bond enthalpy</em>.</p>
<div class="marks">[2]</div>
<div class="question_part_label">b.i.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p class="p1">Ethanol can be used as a fuel. Determine the enthalpy of combustion of ethanol at 298 K, in \({\text{kJ}}\,{\text{mo}}{{\text{l}}^{ - {\text{1}}}}\), using the values in table 10 of the data booklet, assuming all reactants and products are gaseous.</p>
<div class="marks">[4]</div>
<div class="question_part_label">b.ii.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p class="p1">Students can also measure the enthalpy of combustion of ethanol in the laboratory using calorimetry. Suggest the major source of systematic error in these procedures.</p>
<div class="marks">[1]</div>
<div class="question_part_label">c.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p class="p1">State the equation for the acid-catalysed reaction of ethanol with propanoic acid and state the name of the organic product.</p>
<p class="p1">Equation:</p>
<p class="p1"> </p>
<p class="p1"> </p>
<p class="p1">Name of the organic product:</p>
<div class="marks">[2]</div>
<div class="question_part_label">d.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p class="p1">A polyester can be formed when ethane-1,2-diol reacts with benzene-1,4-dicarboxylic acid.</p>
<p class="p1">Deduce the structure of the repeating unit and state the other product formed.</p>
<p class="p1">Repeating unit:</p>
<p class="p1"> </p>
<p class="p1"> </p>
<p class="p1"> </p>
<p class="p1">Other product:</p>
<div class="marks">[2]</div>
<div class="question_part_label">e.i.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p class="p1">State the type of polymerization that occurs.</p>
<div class="marks">[1]</div>
<div class="question_part_label">e.ii.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p class="p1"><span class="s1">The standard enthalpy change of combustion, \(\Delta H_{\text{c}}^\Theta \), of propanoic acid is \( - 1527{\text{ kJ}}\,{\text{mo}}{{\text{l}}^{ - 1}}\)</span>. Determine the standard enthalpy change of formation of propanoic acid, in \({\text{kJ}}\,{\text{mo}}{{\text{l}}^{ - 1}}\), using this information and data from table 12 of the data booklet.</p>
<div class="marks">[4]</div>
<div class="question_part_label">f.i.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p class="p1">Deduce, giving a reason, the sign of the standard entropy change of the system for the formation of propanoic acid from its elements.</p>
<div class="marks">[2]</div>
<div class="question_part_label">f.ii.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p class="p1">Identify <strong>three</strong> allotropes of carbon and describe their structures.</p>
<div class="marks">[4]</div>
<div class="question_part_label">g.</div>
</div>
<br><hr><br><div class="specification">
<p>Iron rusts in the presence of oxygen and water. Rusting is a redox process involving several steps that produces hydrated iron(III) oxide, \({\text{F}}{{\text{e}}_{\text{2}}}{{\text{O}}_{\text{3}}} \bullet {\text{n}}{{\text{H}}_{\text{2}}}{\text{O}}\), as the final product.</p>
<p>The half-equations involved for the first step of rusting are given below.</p>
<p> Half-equation 1: \({\text{Fe(s)}} \to {\text{F}}{{\text{e}}^{2 + }}{\text{(aq)}} + {\text{2}}{{\text{e}}^ - }\)</p>
<p> Half-equation 2: \({{\text{O}}_{\text{2}}}{\text{(aq)}} + {\text{4}}{{\text{e}}^ - } + {\text{2}}{{\text{H}}_{\text{2}}}{\text{O(l)}} \to {\text{4O}}{{\text{H}}^ - }{\text{(aq)}}\)</p>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p>(i) Identify whether half-equation 1 represents oxidation or reduction, giving a reason for your answer.</p>
<p> </p>
<p> </p>
<p>(ii) Identify the oxidation number of each atom in the three species in half-equation 2.</p>
<p style="text-align: center;"><img src="images/Schermafbeelding_2016-08-22_om_05.46.30.png" alt="N14/4/CHEMI/HP2/ENG/TZ0/10.a.ii"></p>
<p>(iii) Deduce the overall redox equation for the first step of rusting by combining half-equations 1 and 2.</p>
<p> </p>
<p> </p>
<p>(iv) Identify the reducing agent in the redox equation in part (iii).</p>
<div class="marks">[5]</div>
<div class="question_part_label">a.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p>The oxygen in half-equation 2 is atmospheric oxygen that is found dissolved in water in very small concentrations. Explain, in terms of intermolecular forces, why oxygen is not very soluble in water.</p>
<div class="marks">[2]</div>
<div class="question_part_label">b.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p>State the relationship between the electron arrangement of an element and its group and period in the periodic table.</p>
<div class="marks">[2]</div>
<div class="question_part_label">c.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p>Transition metals and their compounds often catalyse reactions. The catalyzed decomposition of hydrogen peroxide by CuO is an example. State <strong>two other</strong> examples of catalyzed reactions giving the transition metal or its compound acting as catalyst.</p>
<div class="marks">[2]</div>
<div class="question_part_label">d.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p>(i) State a chemical equation for the partial dissociation of water into ions, including state symbols.</p>
<p> </p>
<p>(ii) The dissociation of water into ions is reversible. State the expression for the ionic product constant of water.</p>
<p> </p>
<p>(iii) The ionic product constant of water was measured at three different temperatures.</p>
<p style="text-align: center;"><img src="images/Schermafbeelding_2016-08-22_om_06.07.14.png" alt="N14/4/CHEMI/HP2/ENG/TZ0/10.e.iii"></p>
<p>Deduce whether the ionization of water is exothermic or endothermic, giving your reason.</p>
<p> </p>
<p> </p>
<p> </p>
<p>(iv) Use the data in part (iii) to determine the pH of water at 373 K, correct to <strong>two</strong> decimal places.</p>
<div class="marks">[6]</div>
<div class="question_part_label">e.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p>(i) An aqueous solution of sodium chloride is electrolysed using inert electrodes. Explain which product is obtained at the positive electrode (anode) if the concentration of sodium chloride is high.</p>
<p> </p>
<p> </p>
<p> </p>
<p> </p>
<p> </p>
<p>(ii) State the half-equations occurring at the electrodes during the electrolysis of the <strong>concentrated </strong>aqueous solution of sodium chloride.</p>
<p> </p>
<p>Negative electrode (cathode):</p>
<p> </p>
<p>Positive electrode (anode):</p>
<div class="marks">[5]</div>
<div class="question_part_label">f.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p>Describe how electrolysis can be used to electroplate a bracelet with a layer of silver metal. Include the choice of electrodes and electrolyte needed in your description.</p>
<div class="marks">[3]</div>
<div class="question_part_label">g.</div>
</div>
<br><hr><br><div class="specification">
<p>Magnesium, a reactive metal found in many common minerals, is also an essential nutrient for both plants and animals.</p>
</div>
<div class="specification">
<p>Successive ionization energies of magnesium are given in the table below.</p>
<p><img src="images/Schermafbeelding_2016-08-14_om_07.56.03.png" alt="M14/4/CHEMI/HP2/ENG/TZ2/08.b"></p>
</div>
<div class="specification">
<p>Magnesium metal is mainly used as a component in lightweight alloys, particularly in combination with aluminium and titanium.</p>
</div>
<div class="specification">
<p>Magnesium is usually produced by the electrolysis of molten magnesium chloride.</p>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p>Define the term <em>first ionization energy</em>.</p>
<div class="marks">[2]</div>
<div class="question_part_label">a.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p>(i) Explain why the second ionization energy is greater than the first ionization energy.</p>
<p> </p>
<p> </p>
<p> </p>
<p> </p>
<p>(ii) Explain why the third ionization energy is much greater than the second ionization energy.</p>
<div class="marks">[4]</div>
<div class="question_part_label">b.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p>Although magnesium is usually found as \({\text{M}}{{\text{g}}^{2 + }}\) in its compounds, it is possible to use the Born-Haber cycle to investigate the possibility of \({\text{M}}{{\text{g}}^ + }\) being able to form stable compounds.</p>
<p>Use the ionization energy data from part (b), along with the other data provided below, to determine the enthalpy change of formation of MgCl(s). Assume that, because \({\text{M}}{{\text{g}}^ + }\) would be similar in size to \({\text{N}}{{\text{a}}^ + }\), MgCl would have a similar lattice enthalpy to NaCl.</p>
<p> Enthalpy of atomization of Mg \( + 146{\text{ kJ}}\,{\text{mo}}{{\text{l}}^{ - 1}}\)</p>
<p> Bond enthalpy in \({\text{C}}{{\text{l}}_{\text{2}}}\) \( + 243{\text{ kJ}}\,{\text{mo}}{{\text{l}}^{ - 1}}\)</p>
<p> Electron affinity of Cl \( + 349{\text{ kJ}}\,{\text{mo}}{{\text{l}}^{ - 1}}\)</p>
<p> Lattice enthalpy of NaCl \( + 790{\text{ kJ}}\,{\text{mo}}{{\text{l}}^{ - 1}}\)</p>
<div class="marks">[3]</div>
<div class="question_part_label">c.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p>Consider the lattice enthalpies of \({\text{Mg}}{{\text{F}}_{\text{2}}}\), \({\text{MgC}}{{\text{l}}_2}\) and \({\text{CaC}}{{\text{l}}_{\text{2}}}\). List these from the most endothermic to the least endothermic and explain your order.</p>
<p> </p>
<p>\({\text{Most endothermic}} \to {\text{Least endothermic}}\)</p>
<div class="marks">[3]</div>
<div class="question_part_label">d.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p>Magnesium hydroxide, \({\text{Mg(OH}}{{\text{)}}_{\text{2}}}\), is only sparingly soluble in water and the equilibrium below exists when excess solid is in contact with a saturated solution.</p>
<p>\[{\text{Mg(OH}}{{\text{)}}_2}{\text{(s)}} \rightleftharpoons {\text{M}}{{\text{g}}^{2 + }}{\text{(aq)}} + {\text{2O}}{{\text{H}}^ - }{\text{(aq)}}\]</p>
<p>Outline how the solubility of magnesium hydroxide will vary with pH.</p>
<div class="marks">[2]</div>
<div class="question_part_label">e.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p>(i) Describe the bonding present in magnesium metal.</p>
<p> </p>
<p> </p>
<p> </p>
<p>(ii) Suggest why magnesium is harder than sodium.</p>
<p> </p>
<p> </p>
<p>(iii) Outline why alloys are generally less malleable than their component metals.</p>
<div class="marks">[4]</div>
<div class="question_part_label">f.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p>(i) Draw a labelled diagram of a suitable apparatus for the electrolysis.</p>
<p> </p>
<p>(ii) State equations for the reactions that take place at the electrodes.</p>
<p> </p>
<p>Negative electrode (cathode) reaction:</p>
<p> </p>
<p>Positive electrode (anode) reaction:</p>
<p> </p>
<p>(iii) When dilute aqueous magnesium chloride is used as the electrolyte, the reactions at both electrodes are different. State equations for the reactions that occur in aqueous solution.</p>
<p> </p>
<p>Negative electrode (cathode) reaction:</p>
<p> </p>
<p>Positive electrode (anode) reaction:</p>
<p> </p>
<p>(iv) Outline why magnesium metal is not produced in the electrolysis of aqueous magnesium chloride.</p>
<div class="marks">[7]</div>
<div class="question_part_label">g.</div>
</div>
<br><hr><br><div class="specification">
<p class="p1">The rate of reaction is an important factor in industrial processes such as the Contact process to make sulfur trioxide, \({\text{S}}{{\text{O}}_{\text{3}}}{\text{(g)}}\).</p>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p class="p1">Define the term <em>rate of reaction</em>.</p>
<div class="marks">[1]</div>
<div class="question_part_label">a.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p class="p1">Describe the collision theory.</p>
<div class="marks">[3]</div>
<div class="question_part_label">b.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p>The Contact process involves this homogeneous equilibrium:</p>
<p>\[{\text{2S}}{{\text{O}}_{\text{2}}}{\text{(g)}} + {{\text{O}}_{\text{2}}}{\text{(g)}} \rightleftharpoons {\text{2S}}{{\text{O}}_{\text{3}}}{\text{(g)}}\,\,\,\,\,\Delta H = - 198{\text{ kJ}}\]</p>
<p>State and explain how increasing the pressure of the reaction mixture affects the yield of \({\text{S}}{{\text{O}}_{\text{3}}}\).</p>
<div class="marks">[2]</div>
<div class="question_part_label">c.i.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p>The Contact process involves this homogeneous equilibrium:</p>
<p>\[{\text{2S}}{{\text{O}}_{\text{2}}}{\text{(g)}} + {{\text{O}}_{\text{2}}}{\text{(g)}} \rightleftharpoons {\text{2S}}{{\text{O}}_{\text{3}}}{\text{(g)}}\,\,\,\,\,\Delta H = - 198{\text{ kJ}}\]</p>
<p>2.00 mol of \({\text{S}}{{\text{O}}_{\text{2}}}{\text{(g)}}\) are mixed with 3.00 mol of \({{\text{O}}_{\text{2}}}{\text{(g)}}\) in a \({\text{1.00 d}}{{\text{m}}^{\text{3}}}\) container until equilibrium is reached. At equilibrium there are 0.80 mol of \({\text{S}}{{\text{O}}_{\text{3}}}{\text{(g)}}\).</p>
<p>Determine the equilibrium constant (\({K_{\text{c}}}\)) assuming all gases are at the same temperature and pressure.</p>
<div class="marks">[4]</div>
<div class="question_part_label">c.ii.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p>The Contact process involves this homogeneous equilibrium:</p>
<p>\[{\text{2S}}{{\text{O}}_{\text{2}}}{\text{(g)}} + {{\text{O}}_{\text{2}}}{\text{(g)}} \rightleftharpoons {\text{2S}}{{\text{O}}_{\text{3}}}{\text{(g)}}\,\,\,\,\,\Delta H = - 198{\text{ kJ}}\]</p>
<p class="p1">State the effect of increasing temperature on the value of \({K_{\text{c}}}\) for this reaction.</p>
<div class="marks">[1]</div>
<div class="question_part_label">c.iii.</div>
</div>
<div class="question" style="padding-left: 20px; padding-right: 20px;">
<p class="p1">Outline the economic importance of using a catalyst in the Contact process.</p>
<div class="marks">[2]</div>
<div class="question_part_label">d.</div>
</div>
<br><hr><br>