chemistry-class-12-unit-04-chapter-10-chemical-kinetics-l-10-16-x4iqkved-ve

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Chemical kinetics</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>Hydrolysis of ethylacetate</p>
</li>
<li>
<p>$\rightarrow $ acid catalyzed</p>
</li>
<li>
<p>$\mathrm{CH}_3 \mathrm{COOC}_2 \mathrm{H}_5+\mathrm{H}_2 \mathrm{O} \xrightarrow{\mathrm{H}^{+}} $</p>
</li>
<li>
<p>$\mathrm{CH}_3 \mathrm{COOH}+\mathrm{C}_2 \mathrm{H}_5 \mathrm{OH} $</p>
</li>
<li>
<p>$r=k\left[\mathrm{CH}_3 \mathrm{COOC}_2 \mathrm{H}_5\right]\left[\mathrm{H}_2 \mathrm{O}\right]$</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-10-chemical-kinetics-l-10_16-x4iqkved_ve-035-0188.4.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> <span style="color:blue">Chemical kinetics</span> $\rightarrow$ Example of pseudo order rate equation $\rightarrow$ Initial rate method $\rightarrow$ Experiment $\rightarrow$ $\rightarrow$ Experiment-1 $\rightarrow$ Experiment-2 $\rightarrow$ Experiment-3 $\rightarrow$ Temperature dependence of reaction rates $\rightarrow$ Example $\rightarrow$ Expression arrhenius $\rightarrow$ Origin of chemical kinetics $\rightarrow$ Van't Hoff $\rightarrow$ Reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Example of pseudo order rate equation</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$r=k\left[\mathrm{H}_2 \mathrm{O}\right]\left[\mathrm{CH}_3 \mathrm{COOC}_2 \mathrm{H}_5\right] $</p>
</li>
<li>
<p>$r=k^{\prime}\left[\mathrm{CH}_3 \mathrm{COOC}_2 \mathrm{H}_5\right] $</p>
</li>
<li>
<p>$k^{\prime}=k\left[\mathrm{H}_2 \mathrm{O}\right] $</p>
</li>
<li>
<p>$k^{\prime} \longrightarrow $pseudo-first order rate constant</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-10-chemical-kinetics-l-10_16-x4iqkved_ve-053-0273.6.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-10-chemical-kinetics-l-10_16-x4iqkved_ve-035-0188.4.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Chemical kinetics $\rightarrow$ <span style="color:blue">Example of pseudo order rate equation</span> $\rightarrow$ Initial rate method $\rightarrow$ Experiment $\rightarrow$ $\rightarrow$ Experiment-1 $\rightarrow$ Experiment-2 $\rightarrow$ Experiment-3 $\rightarrow$ Temperature dependence of reaction rates $\rightarrow$ Example $\rightarrow$ Expression arrhenius $\rightarrow$ Origin of chemical kinetics $\rightarrow$ Van't Hoff $\rightarrow$ Reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Example of pseudo order rate equation</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$C_6 H_5 N_2 Cl (aq)+H_2 O(l) $</p>
</li>
<li>
<p>$\rightarrow\left.C_6 H_5 O H\left(aq)\right)+N_2(g)+H C I(aq)\right) $</p>
</li>
<li>
<p>$r= k\left[C_6 H_5 N_2(l)\right]\left[H_2 O\right] $</p>
</li>
<li>
<p>$r= k^{\prime}\left[C_6 H_5 N_2(l)\right. $</p>
</li>
<li>
<p>$k^{\prime}=k\left[H_2 O\right]$</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-10-chemical-kinetics-l-10_16-x4iqkved_ve-079-0400.8.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Chemical kinetics $\rightarrow$ <span style="color:blue">Example of pseudo order rate equation</span> $\rightarrow$ Initial rate method $\rightarrow$ Experiment $\rightarrow$ $\rightarrow$ Experiment-1 $\rightarrow$ Experiment-2 $\rightarrow$ Experiment-3 $\rightarrow$ Temperature dependence of reaction rates $\rightarrow$ Example $\rightarrow$ Expression arrhenius $\rightarrow$ Origin of chemical kinetics $\rightarrow$ Van't Hoff $\rightarrow$ Reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Initial rate method</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$a A+b B \rightarrow P $</p>
</li>
<li>
<p>$r=k[A]^\alpha[B]^\beta$</p>
</li>
<li>
<p>Initial rate $\rightarrow r_0$</p>
</li>
<li>
<p>$r_0=k[A]_0^\alpha[B]_0^\beta \longrightarrow(1)$</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-10-chemical-kinetics-l-10_16-x4iqkved_ve-01.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Chemical kinetics $\rightarrow$ Example of pseudo order rate equation $\rightarrow$ <span style="color:blue">Initial rate method</span> $\rightarrow$ Experiment $\rightarrow$ $\rightarrow$ Experiment-1 $\rightarrow$ Experiment-2 $\rightarrow$ Experiment-3 $\rightarrow$ Temperature dependence of reaction rates $\rightarrow$ Example $\rightarrow$ Expression arrhenius $\rightarrow$ Origin of chemical kinetics $\rightarrow$ Van't Hoff $\rightarrow$ Reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Initial rate method</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>We do a series of experiments!</li>
</ul>
<p>$\qquad \qquad\downarrow$</p>
<ul>
<li>Take the initial concentration of reactant $A$ to be constant in all these experiments</li>
</ul>
<p>$\qquad\qquad\downarrow$</p>
<ul>
<li>$[A]_0$ is a constant</li>
</ul>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-10-chemical-kinetics-l-10_16-x4iqkved_ve-115-0619.2.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Chemical kinetics $\rightarrow$ Example of pseudo order rate equation $\rightarrow$ <span style="color:blue">Initial rate method</span> $\rightarrow$ Experiment $\rightarrow$ $\rightarrow$ Experiment-1 $\rightarrow$ Experiment-2 $\rightarrow$ Experiment-3 $\rightarrow$ Temperature dependence of reaction rates $\rightarrow$ Example $\rightarrow$ Expression arrhenius $\rightarrow$ Origin of chemical kinetics $\rightarrow$ Van't Hoff $\rightarrow$ Reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Initial rate method</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$r_0={k[A]_0^\alpha} [ B]_0^{\beta} \longrightarrow (1) $</p>
</li>
<li>
<p>$r_0=k^{\prime}[B]_0^\beta \longrightarrow  (2)  $</p>
</li>
<li>
<p>$k^{\prime}=k[A]_0^\alpha$(pseudo order rate constant)</p>
</li>
<li>
<p>$[A]_0$ is held constant</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-10-chemical-kinetics-l-10_16-x4iqkved_ve-02.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Chemical kinetics $\rightarrow$ Example of pseudo order rate equation $\rightarrow$ <span style="color:blue">Initial rate method</span> $\rightarrow$ Experiment $\rightarrow$ $\rightarrow$ Experiment-1 $\rightarrow$ Experiment-2 $\rightarrow$ Experiment-3 $\rightarrow$ Temperature dependence of reaction rates $\rightarrow$ Example $\rightarrow$ Expression arrhenius $\rightarrow$ Origin of chemical kinetics $\rightarrow$ Van't Hoff $\rightarrow$ Reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Experiment</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>$ClO^{-}\left(a_{q}\right)+Br^{-}\left(a{q}\right) \rightarrow  Cl^{-}(aq)  +B{r O^{-}(a q)}$</li>
</ul>
<p>$\space$</p>
<table>
<thead>
<tr>
<th>$r_0$ $mol L^{-1}S^{-1}$</th>
<th>$[ClO^-]_0$ $mol L^{-1}$</th>
<th>$[Br^-]_0$ $mol L^{-1}$</th>
<th>Experiments</th>
</tr>
</thead>
<tbody>
<tr>
<td>$3.19 \times 10^{-6}$</td>
<td>$3.23 \times 10^{-3}$</td>
<td>$2.51 \times 10^{-3}$</td>
<td>1</td>
</tr>
<tr>
<td>$5.98 \times 10^{-6}$</td>
<td>$6.07 \times 10^{-3}$</td>
<td>$2.51 \times 10^{-3}$</td>
<td>2</td>
</tr>
<tr>
<td>$9.14 \times 10^{-6}$</td>
<td>$9.25 \times 10^{-3}$</td>
<td>$2.51 \times 10^{-3}$</td>
<td>3</td>
</tr>
</tbody>
</table>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-10-chemical-kinetics-l-10_16-x4iqkved_ve-210-1083.6.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Chemical kinetics $\rightarrow$ Example of pseudo order rate equation $\rightarrow$ Initial rate method $\rightarrow$ <span style="color:blue">Experiment</span> $\rightarrow$ $\rightarrow$ Experiment-1 $\rightarrow$ Experiment-2 $\rightarrow$ Experiment-3 $\rightarrow$ Temperature dependence of reaction rates $\rightarrow$ Example $\rightarrow$ Expression arrhenius $\rightarrow$ Origin of chemical kinetics $\rightarrow$ Van't Hoff $\rightarrow$ Reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Experiment</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$r_0=k\left[\mathrm{ClO^-}\right]_0^\alpha\left[\mathrm{Br}^{-}\right]_0^\beta…. (3)$</p>
</li>
<li>
<p>$r_0={k\left[\mathrm{Br}^-\right]_0^\beta}\left[\mathrm{ClO}^{-}\right]_0^\alpha $</p>
</li>
<li>
<p>$r_0=k^{\prime}\left[\mathrm{ClO}^{-}\right]_0^\alpha…. (4)$</p>
</li>
<li>
<p>$r=k\left[\mathrm{ClO}^{-}\right][\mathrm{Br}^-] \cdots \text { (5) } $</p>
</li>
</ul>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Chemical kinetics $\rightarrow$ Example of pseudo order rate equation $\rightarrow$ Initial rate method $\rightarrow$ <span style="color:blue">Experiment</span> $\rightarrow$ $\rightarrow$ Experiment-1 $\rightarrow$ Experiment-2 $\rightarrow$ Experiment-3 $\rightarrow$ Temperature dependence of reaction rates $\rightarrow$ Example $\rightarrow$ Expression arrhenius $\rightarrow$ Origin of chemical kinetics $\rightarrow$ Van't Hoff $\rightarrow$ Reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Experiment</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$r_0=k^{\prime}\left[\mathrm{ClO}^{-}\right]_0^\alpha \cdots \text { (4) } $</p>
</li>
<li>
<p>$\frac{r_0}{[\mathrm{ClO}-]_0^\alpha}=k^{\prime} $</p>
</li>
<li>
<p>$\text { if } \alpha=1 \quad \frac{r_0}{\left[\mathrm{ClO} ^{-}\right]_0}=k^{\prime} \cdots \text { (6) }$</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-10-chemical-kinetics-l-10_16-x4iqkved_ve-235-1182.0.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-10-chemical-kinetics-l-10_16-x4iqkved_ve-03.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-10-chemical-kinetics-l-10_16-x4iqkved_ve-210-1083.6.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Chemical kinetics $\rightarrow$ Example of pseudo order rate equation $\rightarrow$ Initial rate method $\rightarrow$ <span style="color:blue">Experiment</span> $\rightarrow$ $\rightarrow$ Experiment-1 $\rightarrow$ Experiment-2 $\rightarrow$ Experiment-3 $\rightarrow$ Temperature dependence of reaction rates $\rightarrow$ Example $\rightarrow$ Expression arrhenius $\rightarrow$ Origin of chemical kinetics $\rightarrow$ Van't Hoff $\rightarrow$ Reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Experiment-1</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$r_0=3.19 \times 10^{-6} \mathrm{mol} L^{-1} \mathrm{~s}^{-1} $</p>
</li>
<li>
<p>${\left[\mathrm{ClO}^{-}\right]_0=3.23 \times 10^{-3} \mathrm{mol}L^{-1}} $</p>
</li>
<li>
<p>$\frac{r_0}{\left[\mathrm{ClO^-}\right]_0}=\frac{3.19 \times 10^{-6} \mathrm{mol}L^{-1} \mathrm{~s}^{-1}}{3.23 \times 10^{-3} \mathrm{mol}L^{-1}}$</p>
</li>
<li>
<p>$={9.88 \times 10^{-4} \mathrm{S}^{-1}}=k^{\prime} $</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-10-chemical-kinetics-l-10_16-x4iqkved_ve-299-1498.8.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-10-chemical-kinetics-l-10_16-x4iqkved_ve-296-1484.4.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Chemical kinetics $\rightarrow$ Example of pseudo order rate equation $\rightarrow$ Initial rate method $\rightarrow$ Experiment $\rightarrow$ $\rightarrow$ <span style="color:blue">Experiment-1</span> $\rightarrow$ Experiment-2 $\rightarrow$ Experiment-3 $\rightarrow$ Temperature dependence of reaction rates $\rightarrow$ Example $\rightarrow$ Expression arrhenius $\rightarrow$ Origin of chemical kinetics $\rightarrow$ Van't Hoff $\rightarrow$ Reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Experiment-2</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$r_0=5.98 \times 10^{-6} \mathrm{mol} L^{-1} \mathrm{~s}^{-1} $</p>
</li>
<li>
<p>${\left[\mathrm{ClO}^{-}\right]_0=6.07 \times 10^{-3} \mathrm{mol}L^{-1}} $</p>
</li>
<li>
<p>$\frac{r_0}{\left[\mathrm{ClO^-}\right]_0}=\frac{5.98 \times 10^{-6} \mathrm{mol}L^{-1} \mathrm{~s}^{-1}}{6.07 \times 10^{-3} \mathrm{mol}L^{-1}} $</p>
</li>
<li>
<p>$={9.85 \times 10^{-4} \mathrm{s}^{-1}}=k^{\prime} $</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-10-chemical-kinetics-l-10_16-x4iqkved_ve-319-1596.0.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Chemical kinetics $\rightarrow$ Example of pseudo order rate equation $\rightarrow$ Initial rate method $\rightarrow$ Experiment $\rightarrow$ $\rightarrow$ Experiment-1 $\rightarrow$ <span style="color:blue">Experiment-2</span> $\rightarrow$ Experiment-3 $\rightarrow$ Temperature dependence of reaction rates $\rightarrow$ Example $\rightarrow$ Expression arrhenius $\rightarrow$ Origin of chemical kinetics $\rightarrow$ Van't Hoff $\rightarrow$ Reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Experiment-3</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$r_0=9.14 \times 10^{-6} \mathrm{mol} L^{-1} \mathrm{~s}^{-1} $</p>
</li>
<li>
<p>${\left[\mathrm{ClO}^{-}\right]_0=9.25 \times 10^{-3} \mathrm{mol}L^{-1}} $</p>
</li>
<li>
<p>$\frac{r_0}{\left[\mathrm{ClO^-}\right]_0}={9.88 \times 10^{-4} \mathrm{~s}^{-1}}$</p>
</li>
<li>
<p>$=k^{\prime} $</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-10-chemical-kinetics-l-10_16-x4iqkved_ve-337-1653.6.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Chemical kinetics $\rightarrow$ Example of pseudo order rate equation $\rightarrow$ Initial rate method $\rightarrow$ Experiment $\rightarrow$ $\rightarrow$ Experiment-1 $\rightarrow$ Experiment-2 $\rightarrow$ <span style="color:blue">Experiment-3</span> $\rightarrow$ Temperature dependence of reaction rates $\rightarrow$ Example $\rightarrow$ Expression arrhenius $\rightarrow$ Origin of chemical kinetics $\rightarrow$ Van't Hoff $\rightarrow$ Reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Temperature dependence of reaction rates</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>Reaction rates depend upon temperature</li>
</ul>
<p>$\quad\downarrow$</p>
<ul>
<li>Increase in temperature in general leads to increase in the rate of a reaction</li>
</ul>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-10-chemical-kinetics-l-10_16-x4iqkved_ve-04.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Chemical kinetics $\rightarrow$ Example of pseudo order rate equation $\rightarrow$ Initial rate method $\rightarrow$ Experiment $\rightarrow$ $\rightarrow$ Experiment-1 $\rightarrow$ Experiment-2 $\rightarrow$ Experiment-3 $\rightarrow$ <span style="color:blue">Temperature dependence of reaction rates</span> $\rightarrow$ Example $\rightarrow$ Expression arrhenius $\rightarrow$ Origin of chemical kinetics $\rightarrow$ Van't Hoff $\rightarrow$ Reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Example</B></primary></p>
<hr>
<main>
<div style='float: left; width:60%;font-size:22px;text-align:left'>
<ul>
<li>$CH_3 I + C_2H_5 O^- \rightarrow C_2 H_5 O CH_3 + I^-$</li>
</ul>
</div>
<div style='float: right; width:40%;'>
<img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/122c290d-532b-4102-bdaf-c0267c99eb00/public" width="80%" >

</div>
</main>
<hr>
<footer style="font-size:18px;"> Chemical kinetics $\rightarrow$ Example of pseudo order rate equation $\rightarrow$ Initial rate method $\rightarrow$ Experiment $\rightarrow$ $\rightarrow$ Experiment-1 $\rightarrow$ Experiment-2 $\rightarrow$ Experiment-3 $\rightarrow$ Temperature dependence of reaction rates $\rightarrow$ <span style="color:blue">Example</span> $\rightarrow$ Expression arrhenius $\rightarrow$ Origin of chemical kinetics $\rightarrow$ Van't Hoff $\rightarrow$ Reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Expression arrhenius</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$k=A e^{-E_a / R T} \cdots 1 a $</p>
</li>
<li>
<p>$k=A \exp \left(-E_a / R T\right) \cdots 1 b \longrightarrow$ Arrhenius equation</p>
</li>
<li>
<p>$k=A_{e^{-}} E_a / R T$</p>
</li>
<li>
<p>A : pre-exponential factor or frequency factor or Arrhenius factor</p>
</li>
<li>
<p>Ea : Activation Energy Arrhenius Activation Energy</p>
</li>
<li>
<p>$k$ : rate constant</p>
</li>
<li>
<p>$R$ : gas constant</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-10-chemical-kinetics-l-10_16-x4iqkved_ve-449-2334.0.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-10-chemical-kinetics-l-10_16-x4iqkved_ve-466-2460.0.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Chemical kinetics $\rightarrow$ Example of pseudo order rate equation $\rightarrow$ Initial rate method $\rightarrow$ Experiment $\rightarrow$ $\rightarrow$ Experiment-1 $\rightarrow$ Experiment-2 $\rightarrow$ Experiment-3 $\rightarrow$ Temperature dependence of reaction rates $\rightarrow$ Example $\rightarrow$ <span style="color:blue">Expression arrhenius</span> $\rightarrow$ Origin of chemical kinetics $\rightarrow$ Van't Hoff $\rightarrow$ Reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Origin of chemical kinetics</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>1850 - 1910 $\longrightarrow$ A lot of work being done to understand the temperature dependence</p>
</li>
<li>
<p>1904 $\longrightarrow$ Ostwald</p>
</li>
<li>
<p>Temperature dependence of reaction rates is “one of the darkest chapters in chemical mechanics”.</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-10-chemical-kinetics-l-10_16-x4iqkved_ve-05.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Chemical kinetics $\rightarrow$ Example of pseudo order rate equation $\rightarrow$ Initial rate method $\rightarrow$ Experiment $\rightarrow$ $\rightarrow$ Experiment-1 $\rightarrow$ Experiment-2 $\rightarrow$ Experiment-3 $\rightarrow$ Temperature dependence of reaction rates $\rightarrow$ Example $\rightarrow$ Expression arrhenius $\rightarrow$ <span style="color:blue">Origin of chemical kinetics</span> $\rightarrow$ Van't Hoff $\rightarrow$ Reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Van’t Hoff</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$\left(\frac{\partial \ln K c}{\partial T}\right)_p=\frac{\Delta U^0}{R T^2}….(2)$</p>
</li>
<li>
<p>$K_c$ : concentration equilibrium constant</p>
</li>
<li>
<p>$\Delta U^{\circ}$ : standard internal energy change</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-10-chemical-kinetics-l-10_16-x4iqkved_ve-539-2782.8.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Chemical kinetics $\rightarrow$ Example of pseudo order rate equation $\rightarrow$ Initial rate method $\rightarrow$ Experiment $\rightarrow$ $\rightarrow$ Experiment-1 $\rightarrow$ Experiment-2 $\rightarrow$ Experiment-3 $\rightarrow$ Temperature dependence of reaction rates $\rightarrow$ Example $\rightarrow$ Expression arrhenius $\rightarrow$ Origin of chemical kinetics $\rightarrow$ <span style="color:blue">Van't Hoff</span> $\rightarrow$ Reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p><strong>Reaction</strong></p>
</li>
<li>
<p>$A+B \xrightleftharpoons [{k_{-1}}]{k_1} P+Q $</p>
</li>
<li>
<p>$r_{\text {forward }}=k_1[A][B] $</p>
</li>
<li>
<p>$r_{\text {backward }}=k_{-1}[P][Q]$</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-10-chemical-kinetics-l-10_16-x4iqkved_ve-555-2860.8.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Chemical kinetics $\rightarrow$ Example of pseudo order rate equation $\rightarrow$ Initial rate method $\rightarrow$ Experiment $\rightarrow$ $\rightarrow$ Experiment-1 $\rightarrow$ Experiment-2 $\rightarrow$ Experiment-3 $\rightarrow$ Temperature dependence of reaction rates $\rightarrow$ Example $\rightarrow$ Expression arrhenius $\rightarrow$ Origin of chemical kinetics $\rightarrow$ Van't Hoff $\rightarrow$ <span style="color:blue">Reaction</span> </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>At equilibrium</p>
</li>
<li>
<p>$r_{\text {forward }} =r_{\text {backward }} $</p>
</li>
<li>
<p>$k_1[A][B] =k_{-1}[P][Q] …..(3)$</p>
</li>
<li>
<p>$\frac{[P][Q]}{[A][B]} =K_C=\frac{k_1}{k_{-1}}……(4)$</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-10-chemical-kinetics-l-10_16-x4iqkved_ve-587-2986.8.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Chemical kinetics $\rightarrow$ Example of pseudo order rate equation $\rightarrow$ Initial rate method $\rightarrow$ Experiment $\rightarrow$ $\rightarrow$ Experiment-1 $\rightarrow$ Experiment-2 $\rightarrow$ Experiment-3 $\rightarrow$ Temperature dependence of reaction rates $\rightarrow$ Example $\rightarrow$ Expression arrhenius $\rightarrow$ Origin of chemical kinetics $\rightarrow$ Van't Hoff $\rightarrow$ <span style="color:blue">Reaction</span> </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$\frac{d ln K_c}{d T} =\frac{\Delta U^0}{R T^2} \cdots \text { (2) } $</p>
</li>
<li>
<p>$K_c =\frac{K_1}{K_{-1}} \cdots \text { (4) }$</p>
</li>
</ul>
<p>using (4) in (2) we have</p>
<ul>
<li>$\frac{d \ln \left(k_1 / k_{-1}\right)}{d T}=\frac{\Delta U^0}{R T^2}$</li>
</ul>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-10-chemical-kinetics-l-10_16-x4iqkved_ve-06.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Chemical kinetics $\rightarrow$ Example of pseudo order rate equation $\rightarrow$ Initial rate method $\rightarrow$ Experiment $\rightarrow$ $\rightarrow$ Experiment-1 $\rightarrow$ Experiment-2 $\rightarrow$ Experiment-3 $\rightarrow$ Temperature dependence of reaction rates $\rightarrow$ Example $\rightarrow$ Expression arrhenius $\rightarrow$ Origin of chemical kinetics $\rightarrow$ Van't Hoff $\rightarrow$ <span style="color:blue">Reaction</span> </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$\frac{d \ln k_1}{d T}-\frac{d \ln k_{-1}}{d T}=\frac{\Delta U^0}{R T^2} \cdots(5) $</p>
</li>
<li>
<p>$\frac{d \ln k_1}{d T}=\frac{E_1}{R T^2} \cdots(6) $</p>
</li>
<li>
<p>$\frac{d \ln k_{-1}}{d T}=\frac{E_{-1}}{R T^2} \cdots \text { (7) }$</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-10-chemical-kinetics-l-10_16-x4iqkved_ve-07.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Chemical kinetics $\rightarrow$ Example of pseudo order rate equation $\rightarrow$ Initial rate method $\rightarrow$ Experiment $\rightarrow$ $\rightarrow$ Experiment-1 $\rightarrow$ Experiment-2 $\rightarrow$ Experiment-3 $\rightarrow$ Temperature dependence of reaction rates $\rightarrow$ Example $\rightarrow$ Expression arrhenius $\rightarrow$ Origin of chemical kinetics $\rightarrow$ Van't Hoff $\rightarrow$ <span style="color:blue">Reaction</span> </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-10</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$\Delta U^0 =E_1-E_{-1} \cdots(8) $</p>
</li>
<li>
<p>$\frac{d \ln k}{d T} =\frac{E}{R T^2} \cdots(9) $</p>
</li>
<li>
<p>$\ln k =\text { constant } - \frac {E}{RT}$</p>
</li>
<li>
<p>$k =A e^{-E / R T}$</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-10-chemical-kinetics-l-10_16-x4iqkved_ve-641-3249.6.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-10-chemical-kinetics-l-10_16-x4iqkved_ve-07.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Chemical kinetics $\rightarrow$ Example of pseudo order rate equation $\rightarrow$ Initial rate method $\rightarrow$ Experiment $\rightarrow$ $\rightarrow$ Experiment-1 $\rightarrow$ Experiment-2 $\rightarrow$ Experiment-3 $\rightarrow$ Temperature dependence of reaction rates $\rightarrow$ Example $\rightarrow$ Expression arrhenius $\rightarrow$ Origin of chemical kinetics $\rightarrow$ Van't Hoff $\rightarrow$ <span style="color:blue">Reaction</span> </footer>