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<h2 class="hd hd-2 unit-title">Lecture 2.2</h2>
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<h2 class="hd hd-2 unit-title">Reference Summary</h2>
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<h3><b> Free Energy (ΔG) </b></h3>
<p> ΔG = ΔH - TΔS <br />H = Enthalpy <br />S = Entropy <br />T= Temperature </p>
<br />
<h3><b> Exergonic Reactions </b></h3>
<p>Exergonic reactions release energy, so that <b> ΔG < 0 </b> and the reaction is spontaneous. </p>
<img src = '/assets/courseware/v1/f4653831666b150a25291763c55b0659/asset-v1:OCW+Pre-7.01+1T2020+type@asset+block/g1.png' alt="This image depicts a conceptual graph. The graph is titled Exergonic Reaction. The y axis label is Free Energy. The x axis label is Course of Reaction. There is one curve plotted on the graph that extends from a plateau at the top left of the plot and then curves down to a plateau at the bottom right of the plot. The value of the curve at the top left is labeled Reactants. The value of the curve at the bottom right is labeled Products. Finally, the value of the Energy Released, or delta G, is labeled as the difference between the value labeled Reactants and the value labeled Products."> <br />
<br />
<h3><b> Endergonic Reactions </b></h3>
<p>Endergonic reactions require energy to proceed, so that <b> ΔG > 0 </b> and the reaction is non-spontaneous. </p>
<img src = '/assets/courseware/v1/c0f179a92df3aff994954a0d921bebe0/asset-v1:OCW+Pre-7.01+1T2020+type@asset+block/g2.png' alt = "This image depicts a conceptual graph. The graph is titled Endergonic Reaction. The y axis label is Free Energy. The x axis label is Course of Reaction. There is one curve plotted on the graph that extends from a plateau at the bottom left of the plot and then curves up to a plateau at the top right of the plot. The value of the curve at the bottom left is labeled Reactants. The value of the curve at the top right is labeled Products. Finally, the value of the Energy Released, or delta G, is labeled as the difference between the value labeled Reactants and the value labeled Products."> <br />
<br />
<h3><b> Equilibrium </b></h3>
<p> If <b> ΔG = 0</b>, the reaction is at equilibrium such that the rate fo the forward reaction = the rate of the backwards reaction. </p> <br />
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<h2 class="hd hd-2 unit-title">Exercise 1 (Understanding Free Energy)</h2>
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<p> The following questions concern Reactions 1, 2, and 3 that are shown below with their ΔG values. </p>
<br />
<p><b>Reaction 1: </b> A → B, ΔG < 0 </p>
<p><b>Reaction 2: </b> A → B, ΔG > 0 </p>
<p><b>Reaction 3: </b> A → B, ΔG = 0 </p>
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<p>Which reaction will proceed spontaneously? Select the best answer.</p>
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<i> (Hint: &#916;G will be negative) </i>
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<p>For which reaction does &#916;H = T&#916;S? Select the best answer.</p>
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<i> (Hint: It will be at equilibrium) </i>
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<h2 class="hd hd-2 unit-title">Exercise 2 (Evaluating Reactions)</h2>
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<p> The following questions concern Reactions A - F, which are shown here with their ΔG values. </p>
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<table class="chart" summary="A chart of the Reactions A through F and their corresponding delta G values." label="Three columns. The first column gives the reaction letter, A, B, C, D, E, or F. The second column gives the chemical formula of the reaction. Each compound is followed by an abbreviation for that compound's state of matter in parentheses. The third column gives the reaction's delta G value in units of kilojoules per mole.">
<tr>
<td scope="col" style="text-align:center; border: 1px solid black;" width="30">
<strong>Reaction</strong>
</td>
<td scope="col" style="text-align:center; border: 1px solid black;" width="90">
<strong>Chemical Formula</strong></td>
<td scope="col" style="text-align:center; border: 1px solid black;" width="120">
<strong>ΔG</strong></td>
</tr>
<tr>
<td scope="row" style="text-align:center; border: 1px solid black;">A</td>
<td scope="row" style="text-align:center; border: 1px solid black;">2 Mg (<em>s</em>) + O<sub>2</sub> (<em>g</em>) → 2 MgO (<em>s</em>)</td>
<td scope="row" style="text-align:center; border: 1px solid black;">ΔG = -1137 kJ/mol</td>
</tr>
<tr>
<td scope="row" style="text-align:center; border: 1px solid black;">B</td>
<td scope="row" style="text-align:center; border: 1px solid black;">NH<sub>3</sub> (<em>g</em>) + HCl (<em>g</em>) → NH<sub>4</sub>Cl (<em>s</em>)</td>
<td scope="row" style="text-align:center; border: 1px solid black;">ΔG = -91.1 kJ/mol</td>
</tr>
<tr>
<td scope="row" style="text-align:center; border: 1px solid black;">C</td>
<td scope="row" style="text-align:center; border: 1px solid black;">AgCl (<em>s</em>) → Ag<sup>+</sup> (<em>aq</em>) + Cl<sup>-</sup> (<em>aq</em>)</td>
<td scope="row" style="text-align:center; border: 1px solid black;">ΔG = 55.6 kJ/mol</td>
</tr>
<tr>
<td scope="row" style="text-align:center; border: 1px solid black;">D</td>
<td scope="row" style="text-align:center; border: 1px solid black;">2 H<sub>2</sub> (<em>g</em>) + O<sub>2</sub>(<em>g</em>) → 2 H<sub>2</sub>O (<em>g</em>)</td>
<td scope="row" style="text-align:center; border: 1px solid black;">ΔG = 456 kJ/mol</td>
</tr>
<tr>
<td scope="row" style="text-align:center; border: 1px solid black;">E</td>
<td scope="row" style="text-align:center; border: 1px solid black;">C (<em>s</em>) + H<sub>2</sub>O (<em>l</em>) → CO(<em>g</em>) + H<sub>2</sub> (<em>g</em>)</td>
<td scope="row" style="text-align:center; border: 1px solid black;">ΔG = 90.8 kJ/mol</td>
</tr>
<tr>
<td scope="row" style="text-align:center; border: 1px solid black;">F</td>
<td scope="row" style="text-align:center; border: 1px solid black;">CH<sub>4</sub> (<em>g</em>) + 2 O<sub>2</sub> (<em>g</em>) → CO<sub>2</sub>(<em>g</em>) + 2 H<sub>2</sub>O (<em>l</em>)</td>
<td scope="row" style="text-align:center; border: 1px solid black;">ΔG = -820 kJ/mol</td>
</tr>
</table>
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<p>Check the boxes for all of the <b> exergonic </b> reactions.</p>
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Question 2
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<p>Which reaction requires the most energy? <br/>Select the best answer.</p>
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<button type="button" class="btn btn-default btn-small notification-btn review-btn sr">Review</button>
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