chemistry-class-12-unit-04-chapter-13-chemical-kinetics-l-13-16-t1j-w8q-ugg

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-13</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Recap</B></primary></p>
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<li>$E_a=137 kJ mol^{-1}$</li>
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<li>If we change temperature from 420 k to 430 k (10 k change), by what factor will rate increase?</li>
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<footer style="font-size:18px;"> <span style="color:blue">Recap</span> $\rightarrow$ Example $\rightarrow$ Closer look at chemical reactions $\rightarrow$ Reaction mechanism $\rightarrow$ Types of reactions $\rightarrow$ Elementary reactions $\rightarrow$ Complex reaction $\rightarrow$ Reaction coordinate $\rightarrow$ Vertical axis $\rightarrow$ Horizontal axis </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-13</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Recap</B></primary></p>
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<li>As we know</li>
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<p>$ln k_2-ln k_1=[ln A-\frac{E_a}{RT_2}]-[ln A-\frac{E_a}{RT_1}]$</p>
</li>
<li>
<p>$ln\frac{k_2}{k_1}=\frac{E_a}{R}[\frac{1}{T_1}-\frac{1}{T_2}]……(7)$</p>
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<footer style="font-size:18px;"> <span style="color:blue">Recap</span> $\rightarrow$ Example $\rightarrow$ Closer look at chemical reactions $\rightarrow$ Reaction mechanism $\rightarrow$ Types of reactions $\rightarrow$ Elementary reactions $\rightarrow$ Complex reaction $\rightarrow$ Reaction coordinate $\rightarrow$ Vertical axis $\rightarrow$ Horizontal axis </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-13</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Example</B></primary></p>
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<li>
<p>ln$ \frac{k_2}{k_1}$ = $\frac{Ea}{R}[\frac{1}{T_1}-\frac{1}{T_2}]$</p>
</li>
<li>
<p>ln$\frac{k_2}{k_1}$ = $\frac{137×10^3 Jmol^{-1}}{8.314 Jk^{-1}mol^{-1}}[\frac{1}{420k} - \frac{1}{430k}]$</p>
</li>
<li>
<p>ln$\frac{k_2}{k_1}$ = $\frac{137×10^3 Jmol^{-1}}{8.314 Jk^{-1}mol^{-1}}[\frac{430-420}{420×430}]k^{-1}$</p>
</li>
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<hr>
<footer style="font-size:18px;"> Recap $\rightarrow$ <span style="color:blue">Example</span> $\rightarrow$ Closer look at chemical reactions $\rightarrow$ Reaction mechanism $\rightarrow$ Types of reactions $\rightarrow$ Elementary reactions $\rightarrow$ Complex reaction $\rightarrow$ Reaction coordinate $\rightarrow$ Vertical axis $\rightarrow$ Horizontal axis </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-13</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Closer look at chemical reactions</B></primary></p>
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<ul>
<li>$A + B \rarr P$</li>
</ul>
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<li>
<p>Does the reaction occur in a single step ? or Does it involve multiple steps ?</p>
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<li>
<p>Which bonds are broken ?</p>
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<p>Which bonds are being formed ?</p>
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<p>Does the bond making and bond breaking happen at the same time ?</p>
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<p>What energy changes are involved in the reactions ?</p>
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</ul>
<p>$\qquad\qquad\downarrow$</p>
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<li><strong>Reaction mechanism</strong></li>
</ul>
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<hr>
<footer style="font-size:18px;"> Recap $\rightarrow$ Example $\rightarrow$ <span style="color:blue">Closer look at chemical reactions</span> $\rightarrow$ Reaction mechanism $\rightarrow$ Types of reactions $\rightarrow$ Elementary reactions $\rightarrow$ Complex reaction $\rightarrow$ Reaction coordinate $\rightarrow$ Vertical axis $\rightarrow$ Horizontal axis </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-13</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Reaction mechanism</B></primary></p>
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<li>
<p>It is the molecular description of how the reactants are being converted to products</p>
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<p>It is a proposed way of reactants going to products</p>
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<p><strong>Experiments</strong></p>
</li>
</ul>
<ol>
<li>
<p>Vary concentrations</p>
</li>
<li>
<p>Vary temperature</p>
</li>
</ol>
<ul>
<li>
<p>$CH_3CH_2Br(aq)+O^-H(aq)\rarr CH_3CH_2OH(aq)+Br^-(aq)……(1)$</p>
</li>
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<p>It is a single step reaction</p>
</li>
</ul>
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<hr>
<footer style="font-size:18px;"> Recap $\rightarrow$ Example $\rightarrow$ Closer look at chemical reactions $\rightarrow$ <span style="color:blue">Reaction mechanism</span> $\rightarrow$ Types of reactions $\rightarrow$ Elementary reactions $\rightarrow$ Complex reaction $\rightarrow$ Reaction coordinate $\rightarrow$ Vertical axis $\rightarrow$ Horizontal axis </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-13</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Elementary reactions</B></primary></p>
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<li>
<p>An elementary reaction is a single step reaction with a single transition state and no intermediates</p>
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<p>Single step reactions are also known as elementary reactions</p>
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<p>Balanced chemical equation conveys the one-step nature of the process</p>
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</ul>
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<hr>
<footer style="font-size:18px;"> Recap $\rightarrow$ Example $\rightarrow$ Closer look at chemical reactions $\rightarrow$ Reaction mechanism $\rightarrow$ Types of reactions $\rightarrow$ <span style="color:blue">Elementary reactions</span> $\rightarrow$ Complex reaction $\rightarrow$ Reaction coordinate $\rightarrow$ Vertical axis $\rightarrow$ Horizontal axis </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-13</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Elementary reactions</B></primary></p>
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<li>
<p><strong>Example</strong></p>
</li>
<li>
<p>$r=k[CH_3CH_2Br][OH^-]$</p>
</li>
<li>
<p>It gives molecularity of a reaction</p>
</li>
<li>
<p>$CH_3CH_2Br(aq)+O^-H(ag)\rarr CH_3CH_2OH(aq)+Br^-(aq)……(1)$</p>
</li>
<li>
<p>$C_6H_5CH_2Cl(aq)+OH^-(aq)\rarr C_6H_5CH_2OH(aq)+Cl^-(aq)……(2)$</p>
</li>
<li>
<p>$C_6H_5CH_2Cl\rarr C_6H_5CH_2^+ + Cl^-……(3)$</p>
</li>
<li>
<p>$C_6H_5CH_2^+ + OH^- \rarr C_6H_5CH_2OH……(4)$</p>
</li>
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<hr>
<footer style="font-size:18px;"> Recap $\rightarrow$ Example $\rightarrow$ Closer look at chemical reactions $\rightarrow$ Reaction mechanism $\rightarrow$ Types of reactions $\rightarrow$ <span style="color:blue">Elementary reactions</span> $\rightarrow$ Complex reaction $\rightarrow$ Reaction coordinate $\rightarrow$ Vertical axis $\rightarrow$ Horizontal axis </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-13</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Complex reaction</B></primary></p>
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<li>
<p>A reacton which proceeds by more than one step is known as a composite reaction or a complex reaction</p>
</li>
<li>
<p>For a composite reaction, the number and nature of the steps in the mechanism cannot be deduced from stoichiometry</p>
</li>
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<li>$C_6H_5CH_2^+ \rarr $ Intermediate</li>
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<li>
<p>Formed in one step and is being used up in another</p>
</li>
<li>
<p>Hence, the corresponding reaction mechanism for these reactions is known as composite reaction mechanism or complex reaction mechanism</p>
</li>
</ul>
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<hr>
<footer style="font-size:18px;"> Recap $\rightarrow$ Example $\rightarrow$ Closer look at chemical reactions $\rightarrow$ Reaction mechanism $\rightarrow$ Types of reactions $\rightarrow$ Elementary reactions $\rightarrow$ <span style="color:blue">Complex reaction</span> $\rightarrow$ Reaction coordinate $\rightarrow$ Vertical axis $\rightarrow$ Horizontal axis </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-13</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Horizontal axis</B></primary></p>
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<li>
<p><strong>Reaction coordinate</strong></p>
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<p>Path the system takes</p>
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<p>Summaries the collection of motions, such as changes in interanomic distance and bond angles that are directly involved in the promotion of products</p>
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<hr>
<footer style="font-size:18px;"> Recap $\rightarrow$ Example $\rightarrow$ Closer look at chemical reactions $\rightarrow$ Reaction mechanism $\rightarrow$ Types of reactions $\rightarrow$ Elementary reactions $\rightarrow$ Complex reaction $\rightarrow$ Reaction coordinate $\rightarrow$ Vertical axis $\rightarrow$ <span style="color:blue">Horizontal axis</span> </footer>