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fa-fw fa-chevron-right divider"></i></li><li><a href="../360/equilibrium.html">Equilibrium</a><i class="fa fa-fw fa-chevron-right divider"></i></li><li><span class="gray">Equilibrium</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/equilibrium/nitrogen_dioxide_at_different_temperatures-1.jpeg" style="width: 160px; height: 127px; float: left;">Understanding how a chemical equilibrium functions is most important. If you can understand that the equilibrium will respond, whenever possible, to oppose any changes that are introduced, then you can work out the answer to any question by thinking it through!</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><strong>dynamic equilibrium*,</strong> homogeneous equilibrium, heterogeneous equilibrium, reaction quotient, equilibrium position, equilibrium constant, backward reaction, forward reaction</p> <div class="tib-flashcard"><a class="show-flashcards btn btn-success btn-xs-block btn-block " data-levels="1" data-mode="" data-topics="614" data-subject-id="7" data-n-flashcards="8" style="text-align:center">Show flashcards</a></div><hr> <div class="panel panel-has-colored-body panel-has-border panel-turquoise"> <div class="panel-heading"><a class="expander" href="#"><span class="fa fa-plus"></span></a> <div> <p>Equilibrium: Understanding Kc and Q</p> </div> </div> <div class="panel-body"> <div class="video-embed vimeo"><iframe allow="accelerometer; autoplay; encrypted-media; gyroscope; picture-in-picture" allowfullscreen="" mozallowfullscreen="" webkitallowfullscreen="" height="420" width="100%" src="https://player.vimeo.com/video/343468974"></iframe></div> </div> <div class="panel-footer"> <div> </div> </div> </div> </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-113" class="dynamic-gallery carousel slide" data-id="113"><div class="carousel-inner" role="listbox"><div class="item active"><a class="fancy" href="../../../std-galleries/7-113/screenshot-2019-06-18-at-164520.png" data-fancybox="gallery-113" title="" data-caption=""><img alt="" src="../../../std-galleries/7-113/screenshot-2019-06-18-at-164520.png"></a></div><div class="item "><a class="fancy" href="../../../std-galleries/7-113/screenshot-2019-06-18-at-164539.png" data-fancybox="gallery-113" title="" data-caption=""><img alt="" src="../../../std-galleries/7-113/screenshot-2019-06-18-at-164539.png"></a></div><div class="item "><a class="fancy" href="../../../std-galleries/7-113/screenshot-2019-06-18-at-164608.png" data-fancybox="gallery-113" title="" data-caption=""><img alt="" src="../../../std-galleries/7-113/screenshot-2019-06-18-at-164608.png"></a></div><div class="item "><a class="fancy" href="../../../std-galleries/7-113/screenshot-2019-06-18-at-164620.png" data-fancybox="gallery-113" title="" data-caption=""><img alt="" src="../../../std-galleries/7-113/screenshot-2019-06-18-at-164620.png"></a></div><div class="item "><a class="fancy" href="../../../std-galleries/7-113/screenshot-2019-06-18-at-164632.png" data-fancybox="gallery-113" title="" data-caption=""><img alt="" src="../../../std-galleries/7-113/screenshot-2019-06-18-at-164632.png"></a></div><div class="item "><a class="fancy" href="../../../std-galleries/7-113/screenshot-2019-06-18-at-164647.png" data-fancybox="gallery-113" title="" data-caption=""><img alt="" src="../../../std-galleries/7-113/screenshot-2019-06-18-at-164647.png"></a></div></div><a class="left carousel-control" href="#carousel-113" role="button" data-slide="prev"><i class="fa fa-fw fa-chevron-left"></i></a><a class="right carousel-control" href="#carousel-113" 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/7-113/screenshot-2019-06-18-at-164520-thumb128.jpg"><li><li data-index="1"><img title="Click to view" src="../../../std-galleries/7-113/screenshot-2019-06-18-at-164539-thumb128.jpg"><li><li data-index="2"><img title="Click to view" src="../../../std-galleries/7-113/screenshot-2019-06-18-at-164608-thumb128.jpg"><li><li data-index="3"><img title="Click to view" src="../../../std-galleries/7-113/screenshot-2019-06-18-at-164620-thumb128.jpg"><li><li data-index="4"><img title="Click to view" src="../../../std-galleries/7-113/screenshot-2019-06-18-at-164632-thumb128.jpg"><li><li data-index="5"><img title="Click to view" src="../../../std-galleries/7-113/screenshot-2019-06-18-at-164647-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="7-144-895"><div class="label label-default q-number">1</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which of the following describes a system at equilibrium?</p><p><strong>1: </strong>The system has no exchange with the surroundings.</p><p><strong>2: </strong>The rate of the forward and backward reactions are equal.</p><p><strong>3: </strong>The concentration of the reactants are the same as the concentration of the products.</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>1 and 3 only</span></label> </p><p><label class="radio"> <input type="radio"> <span>1, 2 and 3</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>2 and 3 only</span></label> </p></div><div class="q-explanation"><p>'1 and 2 only' is the correct answer, since an equilibrium is defined as being closed (1) and having equal rate of reaction in both directions (2), but the concentrations of reactants and products do not need to be the same (3), and rarely are. The third statement might better read 'the concentrations of reactants and products remain <strong>constant'</strong>, which they do, <strong>but not the same as each other</strong>.</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 is the correct equilibrium expression for the equilibrium as given below?</p><p>2SO<sub>2</sub> + O<sub>2</sub> ⇌ 2SO<sub>3</sub></p></div><div class="q-answer"><p><label class="radio"> <input class="c" type="radio"> <span><span class="math-tex">\(K_c = {{[SO_3]^2} \over [SO_2]^2[O_2]}\)</span></span></label> </p><p><label class="radio"> <input type="radio"> <span> <span class="math-tex">\(K_c = {{[SO_2]^2[O_2]} \over [SO_3]^2}\)</span></span></label> </p><p><label class="radio"> <input type="radio"> <span> <span class="math-tex">\(K_c = {{[SO_3]} \over [SO_2][O_2]}\)</span></span></label> </p><p><label class="radio"> <input type="radio"> <span><span class="math-tex">\(K_c = {{[2SO_3]} \over [2SO_2][O_2]}\)</span></span></label> </p></div><div class="q-explanation"><p>The equilibrium constant is defined as being the product of the concentrations of the products (each to the power of the number of moles) over the product of the concentrations of the reactants (each to the power of the number of moles), e.g. for a reaction:</p><p>aA + bB ⇌ cC + dD</p><p><img alt="" height="45" src="../../images/equilibrium/generic-kc.png" width="576"></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>Given the equilibrium for the Haber process N<sub>2(g) </sub>+3H<sub>2(g) </sub>⇌ 2NH<sub>3(g)</sub> and the equilibrium expresssion:</p><p><span class="math-tex">\(K_c = {{[NH_3]^2} \over [N_2][H_2]^3}\)</span></p><p>If K<sub>c</sub> = 0.044 at 200°C what can be said about the position of equilibrium at 200°C?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>The equilibrium lies to the left; there are less reactants than products in the equilibrium mixture.</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>The equilibrium lies to the left; there are more reactants than products in the equilibrium mixture .</span></label> </p><p><label class="radio"> <input type="radio"> <span>The equilibrium lies to the right; there are less reactants than products in the equilibrium mixture.</span></label> </p><p><label class="radio"> <input type="radio"> <span>The equilibrium lies to the right; there are more reactants than products in the equilibrium mixture.</span></label> </p></div><div class="q-explanation"><p>The value of K<sub>c</sub> is 0.044. This number is less than 1, and indicates that the bottom of the fraction is larger than the top. This means that there are more reactants than products in the equilibrium mixture, and this is what 'lies to the left' means.</p><p>Thus the correct answer is 'The equilibrium lies to the left; there are more reactants than products in the equilibrium mixture'.</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>Given the equilibrium for the Haber process N<sub>2(g) </sub>+3H<sub>2(g) </sub>⇌ 2NH<sub>3(g)</sub> and the equilibrium expresssion:</p><p><span class="math-tex">\(K_c = {{[NH_3]^2} \over [N_2][H_2]^3}\)</span></p><p>If K<sub>c</sub> = 0.044 at 200°C, what will happen to the position of equilibrium and to the value of K<sub>c</sub> if a catalyst (finely divided iron) is added?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>The position of equilibrium will shift right, and the value of K<sub>c</sub> will remain the same.</span></label> </p><p><label class="radio"> <input type="radio"> <span>The position of equilibrium will shift left, and the value of K<sub>c</sub> will decrease.</span></label> </p><p><label class="radio"> <input type="radio"> <span>The position of equilibrium will shift right, and the value of K<sub>c</sub> will increase.</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>The position of equilibrium and the value of K<sub>c</sub> will remain the same.</span></label> </p></div><div class="q-explanation"><p>Remember that K<sub>c</sub> is <strong>constant at constant temperature</strong>. So addition of a catalyst will not affect K<sub>c</sub>.</p><p>Addition of a catalyst will not affect the position of an equilbrium either. It will decrease the time it takes for a reaction to reach equilibrium, because it will speed up the rate of the foward and backward reactions equally, but will not alter the position of the equilibrium when it gets there.</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>Given the equilibrium for the Haber process N<sub>2(g) </sub>+3H<sub>2(g) </sub>⇌ 2NH<sub>3(g)</sub> and the equilibrium expresssion:</p><p><span class="math-tex">\(K_c = {{[NH_3]^2} \over [N_2][H_2]^3}\)</span></p><p>If K<sub>c</sub> = 0.044 at 200°C and ΔH = −92 kJ, what will happen to the value of K<sub>c</sub> if the temperature is increased?</p></div><div class="q-answer"><p><label class="radio"> <input class="c" type="radio"> <span>The value of K<sub>c</sub> will be < 0.044</span></label> </p><p><label class="radio"> <input type="radio"> <span>The value of K<sub>c</sub> will be > 1</span></label> </p><p><label class="radio"> <input type="radio"> <span>The value of K<sub>c </sub>will not change</span></label> </p><p><label class="radio"> <input type="radio"> <span>The value of K<sub>c</sub> will be > 0.044</span></label> </p></div><div class="q-explanation"><p>Increasing temperature will favour the <strong>endothermic </strong>direction, which is the reverse direction in this case (a negative ΔH indicates an exothermic forward reaction). The equilibrium will shift to the left to give a greater proportion of reactants. A greater proportion of reactants will make the bottom of the fraction greater and will therefore reduce the value of K<sub>c</sub>.</p><p>The value of K<sub>c</sub> will be < 0.044.</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 is the best description of Q, the reaction quotient?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>Q is always different in value to K<sub>c</sub></span></label> </p><p><label class="radio"> <input type="radio"> <span>Q is the number of moles of reactant over moles of product in the stoichiometric equation. </span></label> </p><p><label class="radio"> <input type="radio"> <span>Q is identical to K<sub>c</sub></span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>Q is the same as the K<sub>c</sub> expression, but not necessarilly with equilibrium concentration values.</span></label> </p></div><div class="q-explanation"><p>The correct answer is 'Q is the same as the K<sub>c</sub> expression, but not necessarilly with equilibrium concentration values'.</p><p>Q is useful when a reaction is thrown out of equilibrium e.g.</p><p>A + B ⇌ C</p><p><span class="math-tex">\(K_c = {{[C]} \over [A][B]}\)</span> at equilibrium, and</p><p><span class="math-tex">\(Q = {{[C]} \over [A][B]}\)</span></p><p>The reaction is at equilibrium (K<sub>c</sub> = Q), and then more A is added: The reaction is suddenly thrown out of equilibrium and now Q will be smaller than K<sub>c</sub> (since [A] has increased and it is on the bottom of the fraction). The equilibrium will now shift to the right, decreasing the amount of A (and B) and increasing the amount of C, until Q once more equals the value of K<sub>c</sub>. Equilibrium is re-attained.</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>Consider the reaction given below at equilibrium:</p><p>N<sub>2</sub>O<sub>4(g) </sub>⇌ 2NO<sub>2(g)</sub></p><p>If more N<sub>2</sub>O<sub>4</sub> gas is pumped into the container, what will happen to the value of Q, the reaction quotient?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>Q will remain the same.</span></label> </p><p><label class="radio"> <input type="radio"> <span>Q will initially increase; the equilibrium will then shift causing Q to decrease again until Q = K<sub>c</sub></span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>Q will initially decrease; the equilibrium will then shift causing Q to increase again until Q = K<sub>c</sub></span></label> </p><p><label class="radio"> <input type="radio"> <span>Q will initially decrease; the equilibrium will<sub> </sub>not shift, and Q ≠ K<sub>c</sub></span></label> </p></div><div class="q-explanation"><p>The correct answer is 'Q will initially decrease; the equilibrium will then shift causing Q to increase again until Q = K<sub>c</sub>'.</p><p><span class="math-tex">\(K_c = {{[NO_2]^2} \over [N_2O_4]}\)</span> ; this is also the expression for Q.</p><p>The reaction is at equilibrium (K<sub>c</sub> = Q), and then more N<sub>2</sub>O<sub>4</sub> is pumped in: The reaction is suddenly thrown out of equilibrium and now Q will be smaller than K<sub>c</sub> (since [N<sub>2</sub>O<sub>4</sub>] has increased and it is on the bottom of the fraction). The equilibrium will now shift to the right, decreasing the amount of N<sub>2</sub>O<sub>4</sub> and increasing the amount of NO<sub>2</sub>, until Q once more equals the value of K<sub>c</sub>. Equilibrium is re-attained.</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>Given the equilibrium for the Haber process N<sub>2(g) </sub>+3H<sub>2(g) </sub>⇌ 2NH<sub>3(g)</sub> and the equilibrium expresssion:</p><p><span class="math-tex">\(K_c = {{[NH_3]^2} \over [N_2][H_2]^3}\)</span></p><p>If K<sub>c</sub> = 0.044 at 200°C what will happen to the position of equilibrium and to the value of K<sub>c</sub> if the pressure is increased (by reducing the total volume)?</p></div><div class="q-answer"><p><label class="radio"> <input class="c" type="radio"> <span>The position of equilibrium will shift right, and the value of K<sub>c</sub> will remain the same.</span></label> </p><p><label class="radio"> <input type="radio"> <span>The position of equilibrium and the value of K<sub>c</sub> will remain the same.</span></label> </p><p><label class="radio"> <input type="radio"> <span>The position of equilibrium will shift left, value of K<sub>c</sub> will increase.</span></label> </p><p><label class="radio"> <input type="radio"> <span>The position of equilibrium will shift right, and the value of K<sub>c</sub> will increase.</span></label> </p></div><div class="q-explanation"><p>Remember that K<sub>c</sub> is <strong>constant at constant temperature</strong>.</p><p>The value of K<sub>c</sub> will therefore remain as 0.044 when the volume decrease causes an increase in pressure, but the increase in pressure will favour the side of the equilibrium with fewest moles of gas (2 moles of the right) so the equilibrium will shift right.</p><p>Decreasing the volume (and thus increasing total pressure) causes the concentration values to each increase. There are more concentration terms on the bottom than the top of the fraction, so the bottom becomes bigger; decreasing the volume throws the reaction out of equilibrium and Q becomes smaller than K<sub>c</sub>. Thus the equilibrium shifts to increase the top of the fraction (more ammonia, NH<sub>3</sub>); that is a shift to the right, until Q once more equals K<sub>c</sub> (0.044).</p><p><span class="math-tex">\(Q = {{[NH_3]^2} \over [N_2][H_2]^3}\)</span></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 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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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