<p><Success style= "margin-top:16rem;text-align:center;"><B>Chemical kinetics<br> Lecture-9</B></Success></p>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-9</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Second order reactions</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>$A \rarr P$</p> </li> <li> <p>$r=k[A]^2……(1)$</p> </li> <li> <p>$r=-\frac{d[A]}{dt}……(2)$</p> </li> </ul> </div> <div style='float: right; width:0%'> <p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-09-chemical-kinetics-l-9_16-orknwx6u6y0-038-0174.0.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> <span style="color:blue">Second order reactions</span> $\rightarrow$ Slop order reactions $\rightarrow$ Half-life for a second order reaction $\rightarrow$ Genral rate law for 2nd order reaction $\rightarrow$ Second order reaction for differnt reactants $\rightarrow$ Derivation of the integrated rate law $\rightarrow$ Reaction involving several reactants $\rightarrow$ Problem $\rightarrow$ How to solve the question $\rightarrow$ Isolation method $\rightarrow$ Kinetic profile diagram $\rightarrow$ Rate expression $\rightarrow$ Pseudo first order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-9</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Second order reactions</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>$-\frac{d[A]}{dt}=k[A]^2……(3)$</p> </li> <li> <p>$-\frac{d[A]}{[A]^2}=kdt$</p> </li> <li> <p>$\int_{[A]_0}^{[A]_t}$ ${\frac{d[A]}{[A]^2}}$</p> </li> <li> <p>$= - \int_{t=0}^t k d t$</p> </li> </ul> </div> </main> <hr> <footer style="font-size:18px;"> <span style="color:blue">Second order reactions</span> $\rightarrow$ Slop order reactions $\rightarrow$ Half-life for a second order reaction $\rightarrow$ Genral rate law for 2nd order reaction $\rightarrow$ Second order reaction for differnt reactants $\rightarrow$ Derivation of the integrated rate law $\rightarrow$ Reaction involving several reactants $\rightarrow$ Problem $\rightarrow$ How to solve the question $\rightarrow$ Isolation method $\rightarrow$ Kinetic profile diagram $\rightarrow$ Rate expression $\rightarrow$ Pseudo first order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-9</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Second order reactions</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>$-[\frac{1}{[A]_t}-\frac{1}{[A]_0}]=-kt$</p> </li> <li> <p>$\frac{1}{[A]_t}-\frac{1}{[A]_0}=kt$</p> </li> <li> <p>$\frac{1}{[A]_t}=\frac{1}{[A]_0}+kt……(4)$</p> </li> </ul> </div> </main> <hr> <footer style="font-size:18px;"> <span style="color:blue">Second order reactions</span> $\rightarrow$ Slop order reactions $\rightarrow$ Half-life for a second order reaction $\rightarrow$ Genral rate law for 2nd order reaction $\rightarrow$ Second order reaction for differnt reactants $\rightarrow$ Derivation of the integrated rate law $\rightarrow$ Reaction involving several reactants $\rightarrow$ Problem $\rightarrow$ How to solve the question $\rightarrow$ Isolation method $\rightarrow$ Kinetic profile diagram $\rightarrow$ Rate expression $\rightarrow$ Pseudo first order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-9</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Slop order reactions</B></primary></p> <hr> <main> <div style='float: left; width:60%;font-size:22px;text-align:left'> <!--Slope = K --> <!--Intercept: $\frac{1}{[A]_0}$ --> <ul> <li>Plot of $\frac{1}{[A]_t}$ against ’t’ is linear</li> </ul> </div> <div style='float: right; width:40%'> <!----> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/04163702-4c8c-4866-5186-c518d30fc800/public" style='width:70%'> </div> </main> <hr> <footer style="font-size:18px;"> Second order reactions $\rightarrow$ <span style="color:blue">Slop order reactions</span> $\rightarrow$ Half-life for a second order reaction $\rightarrow$ Genral rate law for 2nd order reaction $\rightarrow$ Second order reaction for differnt reactants $\rightarrow$ Derivation of the integrated rate law $\rightarrow$ Reaction involving several reactants $\rightarrow$ Problem $\rightarrow$ How to solve the question $\rightarrow$ Isolation method $\rightarrow$ Kinetic profile diagram $\rightarrow$ Rate expression $\rightarrow$ Pseudo first order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-9</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Half-life for a second order reaction</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>$t_{1/2} \rArr [A]_0 \rarr \frac{1}{2}[A]_0$</p> </li> <li> <p>$\frac{1}{[A]_t}=\frac{1}{[A]_0}+kt……(4)$</p> </li> <li> <p>$\frac{1}{\frac{1}{2}[A]_0} - \frac{1}{[A]_0}$</p> </li> <li> <p>$=kt_{1/2}$</p> </li> </ul> </div> </main> <hr> <footer style="font-size:18px;"> Second order reactions $\rightarrow$ Slop order reactions $\rightarrow$ <span style="color:blue">Half-life for a second order reaction</span> $\rightarrow$ Genral rate law for 2nd order reaction $\rightarrow$ Second order reaction for differnt reactants $\rightarrow$ Derivation of the integrated rate law $\rightarrow$ Reaction involving several reactants $\rightarrow$ Problem $\rightarrow$ How to solve the question $\rightarrow$ Isolation method $\rightarrow$ Kinetic profile diagram $\rightarrow$ Rate expression $\rightarrow$ Pseudo first order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-9</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Half-life for a second order reaction</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>$kt_{1/2}=\frac{2}{[A]_0} - \frac{1}{[A]_0}$</p> </li> <li> <p>$t_{1/2}=\frac{1}{k[A]_0}……(5)$</p> </li> <li> <p>$t_{1/2}=\frac{1}{k[A]_0}$</p> </li> </ul> </div> <div style='float: right; width:0%'> <p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-09-chemical-kinetics-l-9_16-orknwx6u6y0-148-0658.8.jpg"> <img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-09-chemical-kinetics-l-9_16-orknwx6u6y0-164-0744.0.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Second order reactions $\rightarrow$ Slop order reactions $\rightarrow$ <span style="color:blue">Half-life for a second order reaction</span> $\rightarrow$ Genral rate law for 2nd order reaction $\rightarrow$ Second order reaction for differnt reactants $\rightarrow$ Derivation of the integrated rate law $\rightarrow$ Reaction involving several reactants $\rightarrow$ Problem $\rightarrow$ How to solve the question $\rightarrow$ Isolation method $\rightarrow$ Kinetic profile diagram $\rightarrow$ Rate expression $\rightarrow$ Pseudo first order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-9</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Half-life for a second order reaction</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>Half-life is proportional to the reciprocal of concentration</p> </li> <li> <p>Longer the concentration, lesser is the half-life</p> </li> <li> <p>Half-life increases as the reaction proceeds</p> </li> <li> <p><strong>Second order reaction</strong></p> </li> <li> <p>$t_{1/2}\rarr$ Preliminary check</p> </li> </ul> </div> <div style='float: right; width:0%'> <p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-09-chemical-kinetics-l-9_16-orknwx6u6y0-182-0846.0.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Second order reactions $\rightarrow$ Slop order reactions $\rightarrow$ <span style="color:blue">Half-life for a second order reaction</span> $\rightarrow$ Genral rate law for 2nd order reaction $\rightarrow$ Second order reaction for differnt reactants $\rightarrow$ Derivation of the integrated rate law $\rightarrow$ Reaction involving several reactants $\rightarrow$ Problem $\rightarrow$ How to solve the question $\rightarrow$ Isolation method $\rightarrow$ Kinetic profile diagram $\rightarrow$ Rate expression $\rightarrow$ Pseudo first order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-9</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Genral rate law for 2nd order reaction</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>$A \rarr P$</p> </li> <li> <p>$aA \rarr P$</p> </li> <li> <p>$r=-\frac{1}{a} \frac{d[A]}{dt}=k[A]^2$</p> </li> <li> <p><strong>Derive the rate law</strong></p> </li> </ul> </div> </main> <hr> <footer style="font-size:18px;"> Second order reactions $\rightarrow$ Slop order reactions $\rightarrow$ Half-life for a second order reaction $\rightarrow$ <span style="color:blue">Genral rate law for 2nd order reaction</span> $\rightarrow$ Second order reaction for differnt reactants $\rightarrow$ Derivation of the integrated rate law $\rightarrow$ Reaction involving several reactants $\rightarrow$ Problem $\rightarrow$ How to solve the question $\rightarrow$ Isolation method $\rightarrow$ Kinetic profile diagram $\rightarrow$ Rate expression $\rightarrow$ Pseudo first order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-9</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Second order reaction for differnt reactants</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>For second order reaction when reactants are different</p> </li> <li> <p>$A \rarr P$</p> </li> <li> <p>$A+B \rarr P$</p> </li> <li> <p>$r=k[A][B]……(6)$</p> </li> <li> <p>if $[A]=[B]$</p> </li> <li> <p>$r=k[A]^2……(7)$</p> </li> </ul> </div> </main> <hr> <footer style="font-size:18px;"> Second order reactions $\rightarrow$ Slop order reactions $\rightarrow$ Half-life for a second order reaction $\rightarrow$ Genral rate law for 2nd order reaction $\rightarrow$ <span style="color:blue">Second order reaction for differnt reactants</span> $\rightarrow$ Derivation of the integrated rate law $\rightarrow$ Reaction involving several reactants $\rightarrow$ Problem $\rightarrow$ How to solve the question $\rightarrow$ Isolation method $\rightarrow$ Kinetic profile diagram $\rightarrow$ Rate expression $\rightarrow$ Pseudo first order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-9</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Derivation of the integrated rate law</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>If $[A]≠[B]$</p> </li> <li> <p>A+B$\rarr P$</p> </li> <li> <p>$r=k[A][B]$</p> </li> <li> <p>Derive the integrated rate law for a reaction like mentioned above!</p> </li> </ul> </div> <div style='float: right; width:0%'> <p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-09-chemical-kinetics-l-9_16-orknwx6u6y0-227-1087.2.jpg"> <img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-09-chemical-kinetics-l-9_16-orknwx6u6y0-02.jpg"> <img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-09-chemical-kinetics-l-9_16-orknwx6u6y0-277-1299.6.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Second order reactions $\rightarrow$ Slop order reactions $\rightarrow$ Half-life for a second order reaction $\rightarrow$ Genral rate law for 2nd order reaction $\rightarrow$ Second order reaction for differnt reactants $\rightarrow$ <span style="color:blue">Derivation of the integrated rate law</span> $\rightarrow$ Reaction involving several reactants $\rightarrow$ Problem $\rightarrow$ How to solve the question $\rightarrow$ Isolation method $\rightarrow$ Kinetic profile diagram $\rightarrow$ Rate expression $\rightarrow$ Pseudo first order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-9</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Reaction involving several reactants</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>aA + bB $\rarr P……(8)$</p> </li> <li> <p>We need to establish whether the rate equation is-</p> </li> <li> <p>$r=k[A]^{\alpha} [B]^{\beta}……(9)$</p> </li> </ul> </div> <div style='float: right; width:0%'> <p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-09-chemical-kinetics-l-9_16-orknwx6u6y0-314-1455.6.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Second order reactions $\rightarrow$ Slop order reactions $\rightarrow$ Half-life for a second order reaction $\rightarrow$ Genral rate law for 2nd order reaction $\rightarrow$ Second order reaction for differnt reactants $\rightarrow$ Derivation of the integrated rate law $\rightarrow$ <span style="color:blue">Reaction involving several reactants</span> $\rightarrow$ Problem $\rightarrow$ How to solve the question $\rightarrow$ Isolation method $\rightarrow$ Kinetic profile diagram $\rightarrow$ Rate expression $\rightarrow$ Pseudo first order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-9</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Problem</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p><strong>Problem</strong>- Rate of reaction now depends on the concentration of both the reactants</p> </li> <li> <p><strong>Solution</strong>- Difficult to disentangle the effect of one reactant from the other</p> </li> </ul> </div> <div style='float: right; width:0%'> <p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-09-chemical-kinetics-l-9_16-orknwx6u6y0-03.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Second order reactions $\rightarrow$ Slop order reactions $\rightarrow$ Half-life for a second order reaction $\rightarrow$ Genral rate law for 2nd order reaction $\rightarrow$ Second order reaction for differnt reactants $\rightarrow$ Derivation of the integrated rate law $\rightarrow$ Reaction involving several reactants $\rightarrow$ <span style="color:blue">Problem</span> $\rightarrow$ How to solve the question $\rightarrow$ Isolation method $\rightarrow$ Kinetic profile diagram $\rightarrow$ Rate expression $\rightarrow$ Pseudo first order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-9</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>How to solve the question</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>We arrange our experimental conditions in such a way that data analysis will be simplified.</p> </li> <li> <p><strong>Two ways</strong></p> </li> <li> <p>Isolation method</p> </li> <li> <p>Initial Rate method</p> </li> </ul> </div> <div style='float: right; width:0%'> <p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-09-chemical-kinetics-l-9_16-orknwx6u6y0-355-1651.2.jpg"> <img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-09-chemical-kinetics-l-9_16-orknwx6u6y0-370-1695.6.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Second order reactions $\rightarrow$ Slop order reactions $\rightarrow$ Half-life for a second order reaction $\rightarrow$ Genral rate law for 2nd order reaction $\rightarrow$ Second order reaction for differnt reactants $\rightarrow$ Derivation of the integrated rate law $\rightarrow$ Reaction involving several reactants $\rightarrow$ Problem $\rightarrow$ <span style="color:blue">How to solve the question</span> $\rightarrow$ Isolation method $\rightarrow$ Kinetic profile diagram $\rightarrow$ Rate expression $\rightarrow$ Pseudo first order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-9</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Isolation method</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>aA + bB$\rarr P$</p> </li> <li> <p>$ClO^-(aq)+ Br^-(aq) \rarr BrO^-(aq)+Cl^-(aq)……(9)$</p> </li> </ul> </div> <div style='float: right; width:0%'> <p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-09-chemical-kinetics-l-9_16-orknwx6u6y0-400-1810.8.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Second order reactions $\rightarrow$ Slop order reactions $\rightarrow$ Half-life for a second order reaction $\rightarrow$ Genral rate law for 2nd order reaction $\rightarrow$ Second order reaction for differnt reactants $\rightarrow$ Derivation of the integrated rate law $\rightarrow$ Reaction involving several reactants $\rightarrow$ Problem $\rightarrow$ How to solve the question $\rightarrow$ <span style="color:blue">Isolation method</span> $\rightarrow$ Kinetic profile diagram $\rightarrow$ Rate expression $\rightarrow$ Pseudo first order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-9</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Isolation method</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>A Plausible rate equation</p> </li> <li> <p>$r=k[ClO^-]^\alpha [Br^-]^\beta……(10)$</p> </li> <li> <p>Let $[ClO^-] =0.1 molL^{-1}$</p> </li> <li> <p>$[Br^-]=2.0×10^{-3} molL^{-1}$</p> </li> <li> <p>$[ClO^-]»[Br^-]$</p> </li> </ul> </div> </main> <hr> <footer style="font-size:18px;"> Second order reactions $\rightarrow$ Slop order reactions $\rightarrow$ Half-life for a second order reaction $\rightarrow$ Genral rate law for 2nd order reaction $\rightarrow$ Second order reaction for differnt reactants $\rightarrow$ Derivation of the integrated rate law $\rightarrow$ Reaction involving several reactants $\rightarrow$ Problem $\rightarrow$ How to solve the question $\rightarrow$ <span style="color:blue">Isolation method</span> $\rightarrow$ Kinetic profile diagram $\rightarrow$ Rate expression $\rightarrow$ Pseudo first order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-9</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Isolation method</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>$ClO^-$ is in excess</p> </li> <li> <p>$\frac{[ClO^-]}{[Br^-]}$</p> </li> <li> <p>$=\frac{0.1 molL^{-1}}{2.0×10^{-3}molL^{-1}}$ = 50</p> </li> <li> <p>$[ClO^-]$ is in fifty-fold excess</p> </li> </ul> </div> <div style='float: right; width:0%'> <p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-09-chemical-kinetics-l-9_16-orknwx6u6y0-421-1916.4.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Second order reactions $\rightarrow$ Slop order reactions $\rightarrow$ Half-life for a second order reaction $\rightarrow$ Genral rate law for 2nd order reaction $\rightarrow$ Second order reaction for differnt reactants $\rightarrow$ Derivation of the integrated rate law $\rightarrow$ Reaction involving several reactants $\rightarrow$ Problem $\rightarrow$ How to solve the question $\rightarrow$ <span style="color:blue">Isolation method</span> $\rightarrow$ Kinetic profile diagram $\rightarrow$ Rate expression $\rightarrow$ Pseudo first order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-9</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Kinetic profile diagram</B></primary></p> <hr> <main> <div style='float: left; width:60%;font-size:22px;text-align:left'> <ul> <li> <p>For hypochloride</p> </li> <li> <p>For bromide</p> </li> <li> <p>$ClO^-$ is being consumed to a very little extent</p> </li> <li> <p>$[ClO^-]$ can be treated to be constant</p> </li> <li> <p>$Br^-$ ion is almost fully consumed!</p> </li> </ul> </div> <div style='float: right; width:40%'> <!----> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/237b648e-84c8-49e9-46c6-8beddb938900/public" style='width:70%'> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/df649641-29d3-4aeb-0b9d-5a181e97c400/public" style='width:60%'> </div> </main> <hr> <footer style="font-size:18px;"> Second order reactions $\rightarrow$ Slop order reactions $\rightarrow$ Half-life for a second order reaction $\rightarrow$ Genral rate law for 2nd order reaction $\rightarrow$ Second order reaction for differnt reactants $\rightarrow$ Derivation of the integrated rate law $\rightarrow$ Reaction involving several reactants $\rightarrow$ Problem $\rightarrow$ How to solve the question $\rightarrow$ Isolation method $\rightarrow$ <span style="color:blue">Kinetic profile diagram</span> $\rightarrow$ Rate expression $\rightarrow$ Pseudo first order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-9</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Kinetic profile diagram</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>$[ClO^-]$ Has essentially remained constant throughout the reaction</p> </li> <li> <p>$[ClO^-]≈[ClO^-]_0$</p> </li> </ul> <!--$[ClO^-]$ Has shown very little change--> <!--$Br^-$ Is almost fully consumed!--> </div> </main> <hr> <footer style="font-size:18px;"> Second order reactions $\rightarrow$ Slop order reactions $\rightarrow$ Half-life for a second order reaction $\rightarrow$ Genral rate law for 2nd order reaction $\rightarrow$ Second order reaction for differnt reactants $\rightarrow$ Derivation of the integrated rate law $\rightarrow$ Reaction involving several reactants $\rightarrow$ Problem $\rightarrow$ How to solve the question $\rightarrow$ Isolation method $\rightarrow$ <span style="color:blue">Kinetic profile diagram</span> $\rightarrow$ Rate expression $\rightarrow$ Pseudo first order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-9</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Rate expression</B></primary></p> <hr> <main> <div style='float: left; width:60%;font-size:22px;text-align:left'> <ul> <li> <p>$r=k[ClO^-]^\alpha [Br^-]^\beta……(10)$</p> </li> <li> <p>$r=k[ClO^-]^\alpha_0 [Br^-]^\beta……(11)$</p> </li> <li> <p>Where $k[ClO^-]^\alpha_0$ is effectively a constant</p> </li> <li> <p>$r=k^{’}[Br^-]^\beta……(12)$</p> </li> <li> <p>$k^{’}=k[ClO^-]^{\alpha}_0……(13)$</p> </li> <li> <p>Where $r=k^{’}[Br^-]^\beta$ is Depending only on $[Br^-]$</p> </li> <li> <p>Kinetics contribution of $[Br^-]$ has been isolated</p> </li> </ul> </div> <div style='float: right; width:40%'> <!----> <!----> <!----> <!----> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/422d1721-5cc8-48c7-c835-eeebf603af00/public" style='width:60%'> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/49198afe-6696-4010-9069-2fca164e8e00/public" style='width:60%'> </div> </main> <hr> <footer style="font-size:18px;"> Second order reactions $\rightarrow$ Slop order reactions $\rightarrow$ Half-life for a second order reaction $\rightarrow$ Genral rate law for 2nd order reaction $\rightarrow$ Second order reaction for differnt reactants $\rightarrow$ Derivation of the integrated rate law $\rightarrow$ Reaction involving several reactants $\rightarrow$ Problem $\rightarrow$ How to solve the question $\rightarrow$ Isolation method $\rightarrow$ Kinetic profile diagram $\rightarrow$ <span style="color:blue">Rate expression</span> $\rightarrow$ Pseudo first order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-9</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Pseudo first order reaction</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>$r=k^{’}[Br^-]^\beta……(13)$</p> </li> <li> <p>Experimentally $\rarr \beta=1$</p> </li> <li> <p>$r=k{’}[Br^-]^{1}$</p> </li> <li> <p>$r=k^{’}[Br^-]……(14)$</p> </li> <li> <p>Keeping $[ClO]^-$ in large excess</p> </li> </ul> </div> <div style='float: right; width:0%'> <p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-09-chemical-kinetics-l-9_16-orknwx6u6y0-06.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Second order reactions $\rightarrow$ Slop order reactions $\rightarrow$ Half-life for a second order reaction $\rightarrow$ Genral rate law for 2nd order reaction $\rightarrow$ Second order reaction for differnt reactants $\rightarrow$ Derivation of the integrated rate law $\rightarrow$ Reaction involving several reactants $\rightarrow$ Problem $\rightarrow$ How to solve the question $\rightarrow$ Isolation method $\rightarrow$ Kinetic profile diagram $\rightarrow$ Rate expression $\rightarrow$ <span style="color:blue">Pseudo first order reaction</span> </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-9</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Pseudo first order reaction</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>$[Br^-]»[ClO^-]$</p> </li> <li> <p>$r=k[ClO^-]^\alpha [Br^-]^\beta_0$</p> </li> <li> <p>$r=\underbrace{k[Br^-]^\beta_0}_{k’’} [ClO^-]^\alpha$</p> </li> <li> <p>$r=k"[ClO^-]^\alpha……(15)$</p> </li> <li> <p>$\alpha$=1</p> </li> <li> <p>$r=k[ClO^-][Br^-]……(16)$</p> </li> </ul> </div> <div style='float: right; width:0%'> <p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-09-chemical-kinetics-l-9_16-orknwx6u6y0-661-3201.6.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Second order reactions $\rightarrow$ Slop order reactions $\rightarrow$ Half-life for a second order reaction $\rightarrow$ Genral rate law for 2nd order reaction $\rightarrow$ Second order reaction for differnt reactants $\rightarrow$ Derivation of the integrated rate law $\rightarrow$ Reaction involving several reactants $\rightarrow$ Problem $\rightarrow$ How to solve the question $\rightarrow$ Isolation method $\rightarrow$ Kinetic profile diagram $\rightarrow$ Rate expression $\rightarrow$ <span style="color:blue">Pseudo first order reaction</span> </footer>

<p><Success style= "margin-top:16rem;text-align:center;"><B>Thank you</B></Success></p>