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Collision theory and rates of reaction <a href="#" class="mark-page-favorite pull-right" data-pid="892" title="Mark as favorite" onclick="return false;"><i class="fa fa-star-o"></i></a> </h1> <ol class="breadcrumb"> <li><a href="../../../chemistry.html"><i class="fa fa-home"></i></a><i class="fa fa-fw fa-chevron-right divider"></i></li><li><a href="../359/kinetics.html">Kinetics</a><i class="fa fa-fw fa-chevron-right divider"></i></li><li><span class="gray">Collision theory and rates of reaction</span></li> <span class="pull-right" style="color: #555" title="Suggested study time: 30 minutes"><i class="fa fa-clock-o"></i> 30'</span> </ol> <article id="main-article"> <p> <img alt="" src="../../images/test-images/crash-1.png" style="width: 160px; height: 121px; float: left;">You are likely to have met much of this topic in your previous chemistry studies. Confidence with your recall of the collision theory and the effect of temperature, surface area and concentration upon rate of reaction is critical. It is also important to understanding of the Maxwell-Boltzmann distribution and be able to draw it (so practise this)!</p> <hr class="hidden-separator"> <div class="panel panel-has-colored-body panel-turquoise"> <div class="panel-heading"><a class="expander" href="#"><span class="fa fa-plus"></span></a> <div> <p>Key concepts</p> </div> </div> <div class="panel-body"> <div> <div class="panel-body"> <div> <p>Ensure you are confident using the terms below and learn the asterisked* definitions</p> <p>rate of reaction, activation energy*, catalyst*, successful collision, Maxwell-Boltzmann distribution, energy profile (energy level diagram)</p> <div class="tib-flashcard"><a class="show-flashcards btn btn-success btn-xs-block btn-block " data-levels="1" data-mode="Normal" data-topics="593" data-subject-id="7" data-n-flashcards="6" style="text-align:center">Show flashcards</a></div><hr> </div> </div> </div> </div> <div class="panel-footer"> <div> </div> </div> </div> <div class="panel panel-yellow panel-has-colored-body"> <div class="panel-heading"><a class="expander" href="#"><span class="fa fa-plus"></span></a> <div> <p>Essentials</p> </div> </div> <div class="panel-body"> <div> <p> The revision cards contain all of the essential content:</p> <div id="carousel-167" class="dynamic-gallery carousel slide" data-id="167"><div class="carousel-inner" role="listbox"><div class="item active"><a class="fancy" href="../../../std-galleries/7-167/screenshot-2020-02-08-at-165137.png" data-fancybox="gallery-167" title="" data-caption=""><img alt="" src="../../../std-galleries/7-167/screenshot-2020-02-08-at-165137.png"></a></div><div class="item "><a class="fancy" href="../../../std-galleries/7-167/screenshot-2020-02-08-at-165158.png" data-fancybox="gallery-167" title="" data-caption=""><img alt="" src="../../../std-galleries/7-167/screenshot-2020-02-08-at-165158.png"></a></div><div class="item "><a class="fancy" 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carousel-control" href="#carousel-167" role="button" data-slide="prev"><i class="fa fa-fw fa-chevron-left"></i></a><a class="right carousel-control" href="#carousel-167" role="button" data-slide="next"><i class="fa fa-fw fa-chevron-right"></i></a></div><ol class="std-carousel-indicators"><li data-index="0"><img title="Click to view" src="../../../std-galleries/7-167/screenshot-2020-02-08-at-165137-thumb128.jpg"><li><li data-index="1"><img title="Click to view" src="../../../std-galleries/7-167/screenshot-2020-02-08-at-165158-thumb128.jpg"><li><li data-index="2"><img title="Click to view" src="../../../std-galleries/7-167/screenshot-2020-02-08-at-165235-thumb128.jpg"><li><li data-index="3"><img title="Click to view" src="../../../std-galleries/7-167/screenshot-2020-02-17-at-193616-thumb128.jpg"><li><li data-index="4"><img title="Click to view" src="../../../std-galleries/7-167/screenshot-2020-02-17-at-193506-thumb128.jpg"><li><li data-index="5"><img title="Click to view" src="../../../std-galleries/7-167/screenshot-2020-02-18-at-084307-thumb128.jpg"><li></li></ol> </div> </div> <div class="panel-footer"> <div> </div> </div> </div> <div class="panel panel-has-colored-body panel-green"> <div class="panel-heading"><a class="expander" href="#"><span class="fa fa-plus"></span></a> <div> <p>Test yourself</p> </div> </div> <div class="panel-body"> <div> <div class="panel-body"> <div> <div class="tib-quiz" data-stats="7-129-892"><div class="label label-default q-number">1</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which of the following is an/are important consideration/s in collision theory when determining the rate of a chemical reaction?</p><p><strong>1: </strong> The frequency of collisions</p><p><strong>2:</strong> The energy of collisions</p><p><strong>3:</strong> The orientation of collisions</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>2 only</span></label> </p><p><label class="radio"> <input type="radio"> <span>2 and 3 only</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>1, 2 and 3</span></label> </p><p><label class="radio"> <input type="radio"> <span>1 and 2 only</span></label> </p></div><div class="q-explanation"><p>Collision theory states that particles must collide with the correct <strong>orientation</strong> and with sufficient <strong>energy </strong>to have a sucessful collision (to overcome the activation energy) and thus react. However, the <strong>frequency </strong>of collisions will also be important in determining the rate of reaction, since a greater number of collisions per unit time will result in a greater number of successful collisions per unit time. Thus '1,2 and 3' is the correct answer.</p></div><div class="actions"><span class="score" data-score="0"></span><button class="btn btn-default btn-sm btn-xs-block text-xs-center check"><i class="fa fa-check-square-o"></i> Check</button></div></div><div class="label label-default q-number">2</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which of the following is <strong>not </strong>likely to be a unit of rate of reaction?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>mol dm<sup>–3 </sup> sec<sup>–1</sup></span></label> </p><p><label class="radio"> <input type="radio"> <span>g min<sup>–1</sup></span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>g mol<sup>–1</sup></span></label> </p><p><label class="radio"> <input type="radio"> <span>mol dm<sup>–3 </sup>min<sup>–1</sup></span></label> </p></div><div class="q-explanation"><p>Rate of reaction can be measured in any unit of quantity per unit time. All the answers indicate a quantity changing with time (remember that mol dm<sup>–3</sup> means <em>moles per cubic decimetre</em> and is a unit of concentration and min<sup>–1</sup> means <em>per minute</em>) except 'g mol<sup>–1</sup>' which means <em>grams per mole</em> (the unit of molar mass) and is thus the correct answer.</p></div><div class="actions"><span class="score" data-score="0"></span><button class="btn btn-default btn-sm btn-xs-block text-xs-center check"><i class="fa fa-check-square-o"></i> Check</button></div></div><div class="label label-default q-number">3</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which of the following might be followed in an appropropriate chemical reaction when attempting to measure the rate of reaction?</p><p><strong>1: </strong> The change in colour of reactants</p><p><strong>2:</strong> The change in volume of products</p><p><strong>3:</strong> The change in mass of reactants</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>2 and 3 only</span></label> </p><p><label class="radio"> <input type="radio"> <span>2 only</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>1, 2 and 3</span></label> </p><p><label class="radio"> <input type="radio"> <span>1 and 2 only</span></label> </p></div><div class="q-explanation"><p>'1, 2 and 3' is the correct answer because all these quantities can be measured to follow the rate in an appropriate chemical reaction. e.g. colour of bromine disappearing; volume of hydrogen gas produced; mass decrease as calcium carbonate reacts with acid (and carbon dioxide is given off).</p></div><div class="actions"><span class="score" data-score="0"></span><button class="btn btn-default btn-sm btn-xs-block text-xs-center check"><i class="fa fa-check-square-o"></i> Check</button></div></div><div class="label label-default q-number">4</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which of the following is the <strong>best</strong> definition of activation energy?</p></div><div class="q-answer"><p><label class="radio"> <input class="c" type="radio"> <span>The minimum energy that colliding particles need in order to react.</span></label> </p><p><label class="radio"> <input type="radio"> <span>The enthalpy difference between reactants and products.</span></label> </p><p><label class="radio"> <input type="radio"> <span>The energy needed to break all the bonds in a reactant.</span></label> </p><p><label class="radio"> <input type="radio"> <span>The average kinetic energy of particles.</span></label> </p></div><div class="q-explanation"><p>The correct (best) answer is 'The minimum energy that colliding particles need in order to react.' This is a definition that must be learned. The other answers are incorrect, although activation energy is required to 'break bonds' in reactants (but not necessarilly all bonds). The average kinetic energy of particles is often marked on a <em>Maxwell-Boltzmann</em> curve, and the enthalpy difference between reactants and products is part of the Energetics topic but neither are directly linked to activation energy.</p></div><div class="actions"><span class="score" data-score="0"></span><button class="btn btn-default btn-sm btn-xs-block text-xs-center check"><i class="fa fa-check-square-o"></i> Check</button></div></div><div class="label label-default q-number">5</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which of the following is/are true with respect to the action of a catalyst on a chemical reaction?</p><p><strong>1: </strong> The catalyst lowers the activation energy</p><p><strong>2:</strong> The catalyst is not permanently chemically changed during the reaction</p><p><strong>3:</strong> The catalyst increases the energy of the particle collisions</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>2 only</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>1 and 2 only</span></label> </p><p><label class="radio"> <input type="radio"> <span>1, 2 and 3</span></label> </p><p><label class="radio"> <input type="radio"> <span>1 only</span></label> </p></div><div class="q-explanation"><p>A catalyst increases the rate of a chemical reaction by causing the reaction to follow a different reaction pathway of l<strong>ower activation energy</strong>, and is <strong>not permanently chemically changed during the reaction</strong>. The catalyst does not otherwise affect the energy of the particles (or the position of equilibrium) - it does not increase the collision energy or collision frequency. Thus '1 and 2 only' is the correct answer.</p></div><div class="actions"><span class="score" data-score="0"></span><button class="btn btn-default btn-sm btn-xs-block text-xs-center check"><i class="fa fa-check-square-o"></i> Check</button></div></div><div class="label label-default q-number">6</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which of the following is the <strong>best </strong>explanation for why increasing temperature increases rate of reaction?</p></div><div class="q-answer"><p><label class="radio"> <input class="c" type="radio"> <span>Particles move faster, collide more often and collide with greater energy.</span></label> </p><p><label class="radio"> <input type="radio"> <span>The collision frequency of particles is greater.</span></label> </p><p><label class="radio"> <input type="radio"> <span>Particles move faster and collide more often.</span></label> </p><p><label class="radio"> <input type="radio"> <span>Particles have greater kinetic energy.</span></label> </p></div><div class="q-explanation"><p>All these answers are correct statements, but 'Particles move faster, collide more often and collide with greater energy' is the correct (best) answer since it covers all the important points: Increasing temperature causes particles to have greater kinetic energy (move faster), increases the collision frequency (collide more often) and also causes collisions to have greater energy (because the particles are striking each other at higher speeds). This results in a greater proportion of collisions that can overcome the activation energy per unit time, and thus a greater rate of reaction.</p></div><div class="actions"><span class="score" data-score="0"></span><button class="btn btn-default btn-sm btn-xs-block text-xs-center check"><i class="fa fa-check-square-o"></i> Check</button></div></div><div class="label label-default q-number">7</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which of the following is the correct explanation for why increasing surface area increases rate of reaction?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>Particles collide with greater energy.</span></label> </p><p><label class="radio"> <input type="radio"> <span>Particles of lower energy are able to react.</span></label> </p><p><label class="radio"> <input type="radio"> <span>Particles move faster and collide more often.</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>A greater number of particles are exposed so there are a greater number of collisions per unit time.</span></label> </p></div><div class="q-explanation"><p>Increasing surface area does not increase the energy of the particles or of the collisions, nor does it alter the activation energy to allow particles of lower energy to react. So the correct answer is 'A greater number of particles are exposed so there are a greater number of collisions per unit time.' Increasing surface area increases the collision frequency (particles collide more often). This results in a greater number of <em>successful</em> collisions per unit time, and thus a greater rate of reaction.</p></div><div class="actions"><span class="score" data-score="0"></span><button class="btn btn-default btn-sm btn-xs-block text-xs-center check"><i class="fa fa-check-square-o"></i> Check</button></div></div><div class="label label-default q-number">8</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which word is missing from the sentence below?</p><p>Increasing the .................................. may increase the rate of a chemical reaction because having a greater number of particles in the same volume increases the collision frequency of the particles so there will be more successful collisions per second.</p></div><div class="q-answer"><p><label class="radio"> <input class="c" type="radio"> <span>Concentration</span></label> </p><p><label class="radio"> <input type="radio"> <span>Temperature</span></label> </p><p><label class="radio"> <input type="radio"> <span>Volume</span></label> </p><p><label class="radio"> <input type="radio"> Activation energy<span></span></label> </p></div><div class="q-explanation"><p>The correct answer is 'concentration'. Increasing volume will lower concentration and may have the opposite effect (lower rate). Increasing temperature will increase the rate, but will not increase the number of particles in the same volume. Increasing activation energy would decrease the rate as fewer particles would have the minimum energy needed to react.</p></div><div class="actions"><span class="score" data-score="0"></span><button class="btn btn-default btn-sm btn-xs-block text-xs-center check"><i class="fa fa-check-square-o"></i> Check</button></div></div><div class="label label-default q-number">9</div><div class="exercise shadow-bottom"><div class="q-question"><p>For a chemical reaction, which of the differences in energy below represents the activation energy of the reverse reaction?</p><p><img alt="" height="372" src="../../images/chemical-kinetics/ea-diagram.png" width="291"></p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>B</span></label> </p><p><label class="radio"> <input type="radio"> <span>C minus B<span lang="EN-US" style="font-size:12.0pt;font-family:Cambria;
mso-ascii-theme-font:minor-latin;mso-fareast-font-family:"ＭＳ 明朝";mso-fareast-theme-font:
minor-fareast;mso-hansi-theme-font:minor-latin;mso-bidi-font-family:"Times New Roman";
mso-bidi-theme-font:minor-bidi;mso-ansi-language:EN-US;mso-fareast-language:
EN-US;mso-bidi-language:AR-SA"></span></span></label> </p><p><label class="radio"> <input type="radio"> <span>A</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>C</span></label> </p></div><div class="q-explanation"><p>C is the activation energy of the reverse reaction and is the correct answer. A is the activation energy of the forward reaction; B is the difference in enthalpy between reactants and products; C minus B would be equal to A (activation energy in the forward direction).</p></div><div class="actions"><span class="score" data-score="0"></span><button class="btn btn-default btn-sm btn-xs-block text-xs-center check"><i class="fa fa-check-square-o"></i> Check</button></div></div><div class="label label-default q-number">10</div><div class="exercise shadow-bottom"><div class="q-question"><p>The diagram below represents a Maxwell-Boltzmann energy distribution.</p><p><img alt="" height="259" src="../../images/chemical-kinetics/maxwell-boltzmann.png" width="376"></p><p>If the temperature is increased, which of the following correctly describe how the distribution should be redrawn?</p><p><strong>1: </strong> The distribution should flatten out</p><p><strong>2:</strong> The peak of the distribution should drop lower</p><p><strong>3:</strong> The peak of the distribution should move to the right</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>1 and 2 only</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>1, 2 and 3</span></label> </p><p><label class="radio"> <input type="radio"> <span>2 only</span></label> </p><p><label class="radio"> <input type="radio"> <span>2 and 3 only</span></label> </p></div><div class="q-explanation"><p>If the temperature is increased particles will gain kinetic energy, but the number of particles will remain the same. Thus all three (1,2 and 3) correctly describe how the distribtuion should be redrawn as exemplified in red here:</p><p><img alt="" height="254" src="../../images/chemical-kinetics/maxwell-boltzmann2.png" width="378"></p></div><div class="actions"><span class="score" data-score="0"></span><button class="btn btn-default btn-sm btn-xs-block text-xs-center check"><i class="fa fa-check-square-o"></i> Check</button></div></div><div class="totals"><span class="score"></span><button class="btn btn-success btn-block text-center check-total"><i class="fa fa-check-square-o"></i> Check</button></div></div><hr> </div> </div> </div> </div> <div class="panel-footer"> <div> </div> </div> </div> <div class="panel panel-has-colored-body panel-default"> <div class="panel-heading"><a class="expander" href="#"><span class="fa fa-plus"></span></a> <div> <p>Exam-style questions</p> </div> </div> <div class="panel-body"> <div> <h4>Paper 1</h4> <h5>Core (SL&HL): <a href="../2712/kinetics-core-sl-and-hl-paper-1-questions.html" title="Kinetics core (SL and HL) paper 1 questions">Kinetics core (SL and HL) paper 1 questions</a></h5> <h5>AHL (HL only): <a href="../2721/kinetics-ahl-hl-only-paper-1-questions.html" title="Kinetics AHL (HL only) paper 1 questions">Kinetics AHL (HL only) paper 1 questions</a></h5> <h4>Paper 2</h4> <h5>Core (SL&HL): <a href="../2719/kinetics-core-sl-hl-paper-2-questions.html" title="Kinetics core (SL & HL) paper 2 questions">Kinetics core (SL & HL) paper 2 questions</a></h5> <h5>AHL (HL only): <a href="../2720/kinetics-ahl-hl-only-paper-2-questions.html" title="Kinetics AHL (HL only) paper 2 questions">Kinetics AHL (HL only) paper 2 questions</a></h5> </div> </div> <div class="panel-footer"> <div> </div> </div> </div> <div class="page-container panel-self-assessment" data-id="892"> <div class="panel-heading">MY PROGRESS</div> <div class="panel-body understanding-rate"> <div class="msg"></div> <label 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}</style><div id="modal-periodic-table" class="modal fade" tabindex="-1" role="dialog"> <div class="modal-dialog modal-lg" role="document" style="width: 90vw;"> <div class="modal-content"> <div class="modal-header"> <h4 class="modal-title">Periodic table</h4> <button type="button" class="close" data-dismiss="modal" aria-label="Close"> <span aria-hidden="true">×</span> </button> </div> <div class="modal-body"> <img src="../../../img/periodic-table/periodic-table-2020.png" style="max-width: 1400px; height: auto"> </div> <div class="modal-footer"> <button type="button" class="btn btn-default btn-xs-block m-xs-0 pull-right" data-dismiss="modal" aria-hidden="true"> Close </button> </div> </div> </div></div> <div id="fc-viewer" class="modal fade modal-flashcard" tabindex="-1" role="dialog"><div class="modal-dialog" role="document"><div class="modal-content"><div class="modal-header" style="background-color: #fafafa;"><div class="row" style="width: 100%;"><div class="col-md-12 tags-heading"><div style="display: flex; justify-content: space-between; align-items: center;"><p id="fc-viewer-info" style="width: 80%;"></p><button type="button" class="close" data-dismiss="modal" aria-label="Close"><span aria-hidden="true">×</span></button></div></div></div></div><div id="flashcard-body" class="modal-body"><div class="row" style="margin: 0;"><div class="col-md-8 fc-viewer-main"><div class="fc-viewer-inner"><div id="fc-viewer-main-front"><div class="fc-viewer-content"></div><span class="mark-favorite" style="position: absolute; top: 10px; right: 10px; font-size: 22px;"><i class="fa fa-lg fa-star-o"></i></span><span id="issue-report" class="issue-report hidden-xs hidden-sm" title="Report a problem"><i class="fa fa-fw fa-lg fa-exclamation-circle" style="font-size: 1.5em;"></i> </span> </div><div id="fc-viewer-main-back" class="reverse-flashcard green-bg"><div class="fc-viewer-content"></div><span class="mark-favorite" style="position: absolute; top: 10px; right: 10px; font-size: 22px;"><i class="fa fa-lg fa-star-o"></i></span></div></div></div><div class="col-md-4 fc-viewer-controls"><div class="fc-viewer-controls-middle"> <div class="fc-viewer-controls-middle-inner fc-back"><div class="fc-viewer-controls-answers mt-xs-0 mx-xs-0"><button id="right-answer" class="btn btn-success text-center btn-block" title="Mark this flashcard as CORRECT"><i class="fa fa-check"></i> Correct</button><button id="wrong-answer" class="btn text-center bg-red btn-block" title="Mark this flashcard as INCORRECT"><i class="fa fa-remove"></i> Incorrect</button></div><table class="table stats"><tr><td>Times flipped</td><td id="fc-viewer-tflipped" class="text-right">0</td></tr><tr><td>Marked as <em>correct</em></td><td id="fc-viewer-right" class="text-right">0</td></tr><tr><td>Marked as <em>incorrect</em></td><td id="fc-viewer-wrong" class="text-right">0</td></tr></table><a href="#" class="btn btn-default btn-sm btn-block text-center reset-stats hidden-xs hidden-sm" title="Reset stats for this flashcard" style="margin: 10px 0;"><i class="fa fa-undo"></i> Reset</a> <div class="fc-notes-container hidden-xs hidden-sm"><textarea class="form-control notes fc-back card-notes" rows="4" placeholder="Write your own notes here..." style="resize: none;">
</textarea><a href="#" class="btn btn-default btn-sm btn-block text-center save-notes" title="Save personal notes for this flashcard" style="margin-bottom: 10px;"><i class="fa fa-pencil"></i> Save notes</a> </div><div class="fc-viewer-actions-sm hidden-md hidden-lg"><button type="button" class="btn btn-sm btn-xs-block reset-stats"><i class="fa fa-fw fa-undo"></i>Reset</button> <button type="button" class="btn btn-sm btn-xs-block" data-toggle="modal" data-target="#card-notes-sm-modal"><i class="fa fa-fw fa-pencil"></i>Notes</button><button type="button" class="btn btn-sm btn-xs-block" data-toggle="modal" data-target="#report-problem-sm-modal"><i class="fa fa-fw fa-exclamation-circle"></i>Report error</button></div> </div></div><div class="fc-viewer-controls-bottom hidden-xs hidden-sm"><div class="fc-move"> <button class="btn bg-turquoise text-center disabled" rel="prev" title="Previous flashcard"><i class="fa fa-fw fa-chevron-left"></i>Prev</button><button class="btn bg-turquoise text-center disabled" rel="next" title="Next flashcard">Next<i class="fa fa-fw fa-chevron-right"></i></button></div><div class="fc-actions"><button class="btn btn-default btn-block text-center shuffle"><i class="fa fa-random"></i> Shuffle</button><div class="fc-progress"><div class="progress"><div class="progress-bar"></div></div><div class="text-right"><span class="fc-viewer-results-counter"></span></div></div></div></div><div class="fc-close-sm hidden-md hidden-lg"><button id="fc-xs-close" type="button" class="btn btn-default btn-block text-center" data-dismiss="modal" aria-label="Close">Close</button> <hr class="thin"> <div class="fc-actions" style="width: 100%;"> <button class="btn btn-default btn-block text-center shuffle"> <i class="fa fa-random"></i> Shuffle </button><div class="fc-progress"><div class="progress"><div class="progress-bar"></div></div><div class="text-right"><span class="fc-viewer-results-counter hidden-md hidden-lg"></span></div></div> </div></div></div></div></div><div class="modal-footer"><div id="report-error-container" class="report-problem"><div class="row"><div class="col-md-8"><div class="msg"></div><div class="form-group"><label>Report a problem for flashcard <span class="fc-viewer-id"></span></label><textarea class="form-control issue-description" cols="4"></textarea></div><button type="button" class="btn btn-primary pull-right send-report disabled"><i class="fa fa-paper-plane"></i>Send</button><button id="close-send-report" type="button" class="btn btn-default" style="margin-left: 0;">Close</button></div></div></div></div></div></div></div><div id="card-notes-sm-modal" class="modal fade overlay-modal" tabindex="-1" role="dialog"><div class="modal-dialog modal-sm" role="document"><div class="modal-content"><div class="modal-header p-xs-3"><h4 class="modal-title text-center my-xs-2">Notes</h4></div><div class="modal-body p-xs-3"><textarea class="form-control notes fc-back card-notes p-xs-3" rows="8" style="resize: none;">
</textarea></div><div class="modal-footer p-xs-3"><button type="button" class="btn btn-sm btn-primary btn-xs-block save-notes"><i class="fa fa-fw fa-pencil"></i>Save</button><button type="button" class="btn btn-sm btn-default btn-xs-block mx-xs-0" data-dismiss="modal" aria-label="Close">Close</button></div></div></div></div><div id="report-problem-sm-modal" class="modal fade overlay-modal report-problem" tabindex="-1" role="dialog"><div class="modal-dialog modal-sm" role="document"><div class="modal-content"><div class="modal-header p-xs-3"><h4 class="modal-title text-center my-xs-2">Report a problem for flashcard <span class="fc-viewer-id"></span></h4></div><div class="modal-body p-xs-3"><div class="msg"></div><div class="form-group mb-xs-0"><textarea class="form-control issue-description p-xs-3" rows="8"></textarea></div></div><div class="modal-footer p-xs-3"><button type="button" class="btn btn-sm btn-primary text-center btn-xs-block mb-xs-3 disabled send-report"><i class="fa fa-fw fa-paper-plane"></i>Send</button><button type="button" class="btn btn-sm btn-default text-center btn-xs-block mx-xs-0" data-dismiss="modal" aria-label="Close">Close</button></div></div></div></div> <div id="fcgame-viewer" class="modal fade modal-flashcard" tabindex="-1" role="dialog"> <div class="modal-dialog modal-lg modal-dialog-fcgame" role="document"> <div class="modal-content mc-flashcard modal-content-fcgame"> <div class="modal-header" style="background-color: #fafafa;"> <div class="row text-center" style="width: 100%;"> <div class="col-md-12"> <div style="display: flex; justify-content: space-between; align-items: center;"> <div class="text-left"> Your time: <span class="chronometer c-mobile" id="chronometer">00:00:</span> <span class="chronometer msec c-mobile" id="chronometer-msec">000</span> <br> Your best time: <span class="chronometer c-mobile" id="best-record"></span> </div> <button type="button" class="close" data-dismiss="modal" aria-label="Close"> <span aria-hidden="true">×</span> </button> </div> </div> </div> </div> <div id="fcgame-body" class=" modal-body modal-body-fcgame"> <div class="row-fluid"> <div class="col-lg-12 col-md-12 col-sm-12 fc-content" id="fc-content" style="padding: 15px;"></div> </div> </div> <div id="end-game" style="display: none;"> <div class="col-lg-10 col-lg-offset-1 col-md-10 col-md-offset-1 col-sm-10 col-sm-offset-1 result shadow-bottom"> <div id="end-game-dismiss"></div> <div id="end-game-results"></div> <div id="show-percent" style="margin-bottom: 30px;font-size: 16px;"></div> </div> <div id="end-game-fc" class="col-lg-12"></div> </div> <div id="start-game" class="col-lg-12 col-md-12 col-sm-12 centered"> <div style="width: 200px;"> <button class="btn btn-success btn-xs-block" id="play-game" style="display: block; width: 100%; margin: 10px 0;">Start</button> <button class="btn btn-default btn-xs-block" id="cancel-game" style="display: block; width: 100%; margin: 10px 0;">Cancel</button> </div> </div> <div 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