chemistry-class-12-unit-04-chapter-04-chemical-kinetics-l-4-16-kicxcenhv8u

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Rate of reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>$\rArr$ Rate of disappearance of reactants</li>
</ul>
<p>or</p>
<ul>
<li>$\rArr$ Rate of appearance of products</li>
</ul>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-04-chemical-kinetics-l-4_16-kicxcenhv8u-01.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ <span style="color:blue">Rate of reaction</span> $\rightarrow$ Rate of reaction in terms of reactants $\rightarrow$ Rate of reaction in terms of products $\rightarrow$ General reaction $\rightarrow$ Stoichiometric coefficients $\rightarrow$ Example of stoichiometric coefficient $\rightarrow$ Reaction $\rightarrow$ Rate of reaction $\rightarrow$ Example $\rightarrow$ Rate of reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Rate of reaction in terms of reactants</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$=-\frac{\Delta[ClO^-]}{\Delta t}$ $=-\frac{\Delta[Br^-]}{\Delta t}$</p>
</li>
<li>
<p>$\frac{\Delta[ClO^-]}{\Delta t}$ $=\frac{c_2 - c_1}{t_3 - t_1}=\frac{-ve}{+ve}=-ve$</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-04-chemical-kinetics-l-4_16-kicxcenhv8u-059-0297.6.jpg"></p>
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<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-04-chemical-kinetics-l-4_16-kicxcenhv8u-021-0087.6.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ Rate of reaction $\rightarrow$ <span style="color:blue">Rate of reaction in terms of reactants</span> $\rightarrow$ Rate of reaction in terms of products $\rightarrow$ General reaction $\rightarrow$ Stoichiometric coefficients $\rightarrow$ Example of stoichiometric coefficient $\rightarrow$ Reaction $\rightarrow$ Rate of reaction $\rightarrow$ Example $\rightarrow$ Rate of reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Rate of reaction in terms of products</B></primary></p>
<hr>
<main>
<div style='float: left; width:65%;font-size:22px;text-align:left'>
<ul>
<li>$=\frac{\Delta[BrO^-]}{[\Delta t]}$ $=\frac{\Delta[Cl^-]}{\Delta t}$ $=\frac{+ve}{+ve}=+ve$</li>
</ul>
</div>
<div style='float: right; width:35%;'>
<p><img alt="alt text" src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/5dcec927-4231-4b1c-1e7b-4257477ec200/public"></p>


</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ Rate of reaction $\rightarrow$ Rate of reaction in terms of reactants $\rightarrow$ <span style="color:blue">Rate of reaction in terms of products</span> $\rightarrow$ General reaction $\rightarrow$ Stoichiometric coefficients $\rightarrow$ Example of stoichiometric coefficient $\rightarrow$ Reaction $\rightarrow$ Rate of reaction $\rightarrow$ Example $\rightarrow$ Rate of reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>General reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p><strong>aA+bB+……$\rarr pP+qQ+….$</strong></p>
</li>
<li>
<p>A,B,C..$\quad$ $\rArr$ reactants</p>
</li>
<li>
<p>a b c $\quad$ $\rArr$ stoichiometric coefficients</p>
</li>
<li>
<p>P,Q,R $\quad$ $\rArr$ products</p>
</li>
<li>
<p>p q r $\quad$ $\rArr$ stoichiometric coefficients</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-04-chemical-kinetics-l-4_16-kicxcenhv8u-02.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ Rate of reaction $\rightarrow$ Rate of reaction in terms of reactants $\rightarrow$ Rate of reaction in terms of products $\rightarrow$ <span style="color:blue">General reaction</span> $\rightarrow$ Stoichiometric coefficients $\rightarrow$ Example of stoichiometric coefficient $\rightarrow$ Reaction $\rightarrow$ Rate of reaction $\rightarrow$ Example $\rightarrow$ Rate of reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>General reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p><strong>For reactants - $\quad$ $\nu$ $\quad$is $\quad$-ve</strong></p>
</li>
<li>
<p><strong>For products - $\quad$ $\nu$ $\quad$is $\quad$+ve</strong></p>
</li>
<li>
<p>$\nu_A$ $\quad$ = $\quad$ -a</p>
</li>
<li>
<p>$\nu_B$ $\quad$ = $\quad$ -b</p>
</li>
<li>
<p>$\nu_p$ $\quad$ = $\quad$ p</p>
</li>
<li>
<p>$\nu_q$ $\quad$ = $\quad$ q</p>
</li>
</ul>
</div>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-04-chemical-kinetics-l-4_16-kicxcenhv8u-098-0577.2.jpg"></p>

</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ Rate of reaction $\rightarrow$ Rate of reaction in terms of reactants $\rightarrow$ Rate of reaction in terms of products $\rightarrow$ <span style="color:blue">General reaction</span> $\rightarrow$ Stoichiometric coefficients $\rightarrow$ Example of stoichiometric coefficient $\rightarrow$ Reaction $\rightarrow$ Rate of reaction $\rightarrow$ Example $\rightarrow$ Rate of reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>General reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$aA+bB \rarr pP+qQ$</p>
</li>
<li>
<p>Degree of advancement of a reaction $\rightarrow$ $\xi$</p>
</li>
<li>
<p>$n_i=n_i^0 + \nu_i \xi……(1)$</p>
</li>
<li>
<p>$n_i$ number of moles of no chemical species i</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-04-chemical-kinetics-l-4_16-kicxcenhv8u-04.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ Rate of reaction $\rightarrow$ Rate of reaction in terms of reactants $\rightarrow$ Rate of reaction in terms of products $\rightarrow$ <span style="color:blue">General reaction</span> $\rightarrow$ Stoichiometric coefficients $\rightarrow$ Example of stoichiometric coefficient $\rightarrow$ Reaction $\rightarrow$ Rate of reaction $\rightarrow$ Example $\rightarrow$ Rate of reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>General reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$n_i^0=$ the number of moles of the chemical species  ‘i’ when $\xi= \leftarrow$ degree of advancement 0</p>
</li>
<li>
<p>$\nu_i$ stoichiometric coefficients</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-04-chemical-kinetics-l-4_16-kicxcenhv8u-162-0928.8.jpg"></p>

</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ Rate of reaction $\rightarrow$ Rate of reaction in terms of reactants $\rightarrow$ Rate of reaction in terms of products $\rightarrow$ <span style="color:blue">General reaction</span> $\rightarrow$ Stoichiometric coefficients $\rightarrow$ Example of stoichiometric coefficient $\rightarrow$ Reaction $\rightarrow$ Rate of reaction $\rightarrow$ Example $\rightarrow$ Rate of reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>General reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$n_i=n^0_i + \nu_i \xi……(1)$</p>
</li>
<li>
<p><strong>Differentiate (1) with respect to time</strong></p>
</li>
<li>
<p>$\frac{dn_i}{dt}$= $\frac{dn_i^0}{dt}+\frac{d(\nu_i \xi)}{dt}……(2)$</p>
</li>
<li>
<p><strong>Because $n_i^0$ is a constant , hence $\frac{dn_i^0}{dt}= 0$</strong></p>
</li>
<li>
<p>$\frac{d(\nu_i \xi)}{dt}=\nu_i \frac{d\xi}{dt}$</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-04-chemical-kinetics-l-4_16-kicxcenhv8u-05.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ Rate of reaction $\rightarrow$ Rate of reaction in terms of reactants $\rightarrow$ Rate of reaction in terms of products $\rightarrow$ <span style="color:blue">General reaction</span> $\rightarrow$ Stoichiometric coefficients $\rightarrow$ Example of stoichiometric coefficient $\rightarrow$ Reaction $\rightarrow$ Rate of reaction $\rightarrow$ Example $\rightarrow$ Rate of reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>General reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$\frac{dn_i}{dt}=\nu_i \frac{d\xi}{dt}$</p>
</li>
<li>
<p>$\frac{d\xi}{dt}=\frac{1}{\nu_i}\frac{dni}{dt}$…….(3)</p>
</li>
<li>
<p>Rate of advancement of the reaction $\rightarrow$ rate of the reaction</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-04-chemical-kinetics-l-4_16-kicxcenhv8u-239-1353.6.jpg"></p>

</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ Rate of reaction $\rightarrow$ Rate of reaction in terms of reactants $\rightarrow$ Rate of reaction in terms of products $\rightarrow$ <span style="color:blue">General reaction</span> $\rightarrow$ Stoichiometric coefficients $\rightarrow$ Example of stoichiometric coefficient $\rightarrow$ Reaction $\rightarrow$ Rate of reaction $\rightarrow$ Example $\rightarrow$ Rate of reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>General reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p><strong>$aA+bB \rarr pP+qQ$</strong></p>
</li>
<li>
<p>$n_i=n^0_i + \nu_i \xi……(1)$</p>
</li>
<li>
<p>$i \rarr A$</p>
</li>
<li>
<p>$n_A=n_A^0+\nu_A \xi$</p>
</li>
<li>
<p>$n_A=n^0_A - a \xi$</p>
</li>
<li>
<p>$\frac{dn_A}{dt}=\frac{dn_A^0}{dt} + \frac{d(-a \xi)}{dt}$</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-04-chemical-kinetics-l-4_16-kicxcenhv8u-252-1450.8.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-04-chemical-kinetics-l-4_16-kicxcenhv8u-261-1520.4.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ Rate of reaction $\rightarrow$ Rate of reaction in terms of reactants $\rightarrow$ Rate of reaction in terms of products $\rightarrow$ <span style="color:blue">General reaction</span> $\rightarrow$ Stoichiometric coefficients $\rightarrow$ Example of stoichiometric coefficient $\rightarrow$ Reaction $\rightarrow$ Rate of reaction $\rightarrow$ Example $\rightarrow$ Rate of reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>General reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p><strong>General reaction</strong></p>
</li>
<li>
<p>$\frac{dn_A}{dt}=-a\frac{d\xi}{dt}$</p>
</li>
<li>
<p>$\frac{d\xi}{dt}=-\frac{1}{a}\frac{dn_A}{dt}$</p>
</li>
<li>
<p>Rate of reaction in terms of the change in the number of moles of ‘A’</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-04-chemical-kinetics-l-4_16-kicxcenhv8u-06.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ Rate of reaction $\rightarrow$ Rate of reaction in terms of reactants $\rightarrow$ Rate of reaction in terms of products $\rightarrow$ <span style="color:blue">General reaction</span> $\rightarrow$ Stoichiometric coefficients $\rightarrow$ Example of stoichiometric coefficient $\rightarrow$ Reaction $\rightarrow$ Rate of reaction $\rightarrow$ Example $\rightarrow$ Rate of reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>General reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p><strong>$i\rarr B$</strong></p>
</li>
<li>
<p>$n_B=n^0_B + \nu_B \xi$</p>
</li>
<li>
<p>$n_B=n^0_B - b \xi$</p>
</li>
<li>
<p>$\frac{dn_B}{dt}=\frac{dn^0_B}{dt} + \frac{d(-b \xi)}{dt}$</p>
</li>
<li>
<p>$\frac{dn_B}{dt}=-b\frac{d\xi}{dt}$</p>
</li>
<li>
<p>$\frac{d\xi}{dt}=-\frac{1}{b} \frac{dn_B}{dt}$</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-04-chemical-kinetics-l-4_16-kicxcenhv8u-07.jpg"></p>

</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ Rate of reaction $\rightarrow$ Rate of reaction in terms of reactants $\rightarrow$ Rate of reaction in terms of products $\rightarrow$ <span style="color:blue">General reaction</span> $\rightarrow$ Stoichiometric coefficients $\rightarrow$ Example of stoichiometric coefficient $\rightarrow$ Reaction $\rightarrow$ Rate of reaction $\rightarrow$ Example $\rightarrow$ Rate of reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>General reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p><strong>$aA+bB \rarr pP+qQ$</strong></p>
</li>
<li>
<p><strong>$i\rarr P$</strong></p>
</li>
<li>
<p>$n_p=n^0_P+ \nu_P \xi$</p>
</li>
<li>
<p>$n_p=n^0_P+ p \xi$</p>
</li>
<li>
<p>$\frac{dn_P}{dt}$=$\frac{dn^0_P}{dt}+\frac{d(P\xi)}{dt}$</p>
</li>
<li>
<p>$\frac{dn_P}{dt}=P\frac{d\xi}{dt}$ $∴ \frac{d\xi}{dt}=\frac{1}{P}\frac{dn_P}{dt}$</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-04-chemical-kinetics-l-4_16-kicxcenhv8u-08.jpg"></p>

</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ Rate of reaction $\rightarrow$ Rate of reaction in terms of reactants $\rightarrow$ Rate of reaction in terms of products $\rightarrow$ <span style="color:blue">General reaction</span> $\rightarrow$ Stoichiometric coefficients $\rightarrow$ Example of stoichiometric coefficient $\rightarrow$ Reaction $\rightarrow$ Rate of reaction $\rightarrow$ Example $\rightarrow$ Rate of reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>General reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$\frac{d\xi}{dt}$ $=-\frac{1}{a}\frac{dn_A}{dt}=-\frac{1}{b}\frac{dn_B}{dt}$*</p>
</li>
<li>
<p>$=\frac{1}{p}\frac{Qn_p}{dt}=\frac{1}{q}\frac{dn_Q}{dt}$</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-04-chemical-kinetics-l-4_16-kicxcenhv8u-366-2102.4.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ Rate of reaction $\rightarrow$ Rate of reaction in terms of reactants $\rightarrow$ Rate of reaction in terms of products $\rightarrow$ <span style="color:blue">General reaction</span> $\rightarrow$ Stoichiometric coefficients $\rightarrow$ Example of stoichiometric coefficient $\rightarrow$ Reaction $\rightarrow$ Rate of reaction $\rightarrow$ Example $\rightarrow$ Rate of reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Stoichiometric coefficients</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>The stoichiometric coefficients is always positive</li>
</ul>
<p><strong>Reactant</strong> $\quad$ : $\quad$ Put a ‘-ve’ sign</p>
<p>$\qquad\qquad\quad$ before the coefficient</p>
<p><strong>Product</strong> $\quad$ : $\quad$ Put a ‘+ve’ sign</p>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-04-chemical-kinetics-l-4_16-kicxcenhv8u-388-2193.6.jpg"></p>

</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ Rate of reaction $\rightarrow$ Rate of reaction in terms of reactants $\rightarrow$ Rate of reaction in terms of products $\rightarrow$ General reaction $\rightarrow$ <span style="color:blue">Stoichiometric coefficients</span> $\rightarrow$ Example of stoichiometric coefficient $\rightarrow$ Reaction $\rightarrow$ Rate of reaction $\rightarrow$ Example $\rightarrow$ Rate of reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Example of stoichiometric coefficient</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$2N_2O_5\rarr4NO_2 + O_2$</p>
</li>
<li>
<p>$\frac{d\xi}{dt}$ $=-\frac{1}{2}\frac{dn_{N_2 O_5}}{dt}$ $=\frac{1}{4} \frac{dn_{NO_2}}{dt} =\frac{dn_{O_2}}{dt}$</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-04-chemical-kinetics-l-4_16-kicxcenhv8u-431-2437.2.jpg"></p>

</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ Rate of reaction $\rightarrow$ Rate of reaction in terms of reactants $\rightarrow$ Rate of reaction in terms of products $\rightarrow$ General reaction $\rightarrow$ Stoichiometric coefficients $\rightarrow$ <span style="color:blue">Example of stoichiometric coefficient</span> $\rightarrow$ Reaction $\rightarrow$ Rate of reaction $\rightarrow$ Example $\rightarrow$ Rate of reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</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>Since most of the reactions are done under constant volume conditions , then</p>
</li>
<li>
<p>from-(1) $\rarr n_i=n^0_i + \nu_i \xi……(1)$</p>
</li>
<li>
<p>$\frac{d\xi}{dt}=\frac{1}{\nu_i}\frac{dn_i}{dt}……(3)$</p>
</li>
<li>
<p>$\frac{1}{V}\quad \frac{d\xi}{dt}$ $=\frac{1}{V}\quad \frac{1}{\nu_i}\frac{dn_i}{dt}$</p>
</li>
<li>
<p>V(volume) is 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-04-chemical-kinetics-l-4_16-kicxcenhv8u-458-2604.0.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ Rate of reaction $\rightarrow$ Rate of reaction in terms of reactants $\rightarrow$ Rate of reaction in terms of products $\rightarrow$ General reaction $\rightarrow$ Stoichiometric coefficients $\rightarrow$ Example of stoichiometric coefficient $\rightarrow$ <span style="color:blue">Reaction</span> $\rightarrow$ Rate of reaction $\rightarrow$ Example $\rightarrow$ Rate of reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Rate of reaction</B></primary></p>
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<li>
<p>$\frac{d(\xi V)}{dt}$ $=\frac{1}{\nu_i}\frac{d(n_i/V)}{dt}$</p>
</li>
<li>
<p>$\frac{d(\xi /V)}{dt}$ $=\frac{1}{\nu_i}\frac{d[i]}{dt}……(4)$</p>
</li>
<li>
<p>[i] $\rArr$ concentration of species ‘i’</p>
</li>
</ul>
<p>(rate of reaction)</p>
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<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-04-chemical-kinetics-l-4_16-kicxcenhv8u-10.jpg"></p>
</div>
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<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ Rate of reaction $\rightarrow$ Rate of reaction in terms of reactants $\rightarrow$ Rate of reaction in terms of products $\rightarrow$ General reaction $\rightarrow$ Stoichiometric coefficients $\rightarrow$ Example of stoichiometric coefficient $\rightarrow$ Reaction $\rightarrow$ <span style="color:blue">Rate of reaction</span> $\rightarrow$ Example $\rightarrow$ Rate of reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Example</B></primary></p>
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<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$CH_3CHO(g) \rarr CH_4(g)+CO(g)$</p>
</li>
<li>
<p>The rate of this reaction can be followed by measuring the pressure in the system of constant volume and temperature</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-04-chemical-kinetics-l-4_16-kicxcenhv8u-531-2942.4.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ Rate of reaction $\rightarrow$ Rate of reaction in terms of reactants $\rightarrow$ Rate of reaction in terms of products $\rightarrow$ General reaction $\rightarrow$ Stoichiometric coefficients $\rightarrow$ Example of stoichiometric coefficient $\rightarrow$ Reaction $\rightarrow$ Rate of reaction $\rightarrow$ <span style="color:blue">Example</span> $\rightarrow$ Rate of reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</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:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>Assume ideal gas behaviour of the gases</p>
</li>
<li>
<p>$CH_3CHO(g) \rarr CH_4(g)+CO(g)$</p>
</li>
</ul>
<p>Initial $\quad$ $n^0_{CH_3CHO} \quad\quad 0  \quad\quad\quad\quad 0$</p>
<p>$n^0_{CH_3CHO}-\xi \quad \quad \quad \quad\xi \quad \quad \quad\quad \xi $</p>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-04-chemical-kinetics-l-4_16-kicxcenhv8u-564-3092.4.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ Rate of reaction $\rightarrow$ Rate of reaction in terms of reactants $\rightarrow$ Rate of reaction in terms of products $\rightarrow$ General reaction $\rightarrow$ Stoichiometric coefficients $\rightarrow$ Example of stoichiometric coefficient $\rightarrow$ Reaction $\rightarrow$ Rate of reaction $\rightarrow$ <span style="color:blue">Example</span> $\rightarrow$ Rate of reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Rate of reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$n_{CH_3CHO}=n^0_{CH_3CHO}+\nu_i\xi$</p>
</li>
<li>
<p>$n_{CH_3CHO}=n^0_{CH_3CHO}-\xi$</p>
</li>
<li>
<p>$n_{CH_4}=n^0_{CH_4}+\nu_i \xi$</p>
</li>
<li>
<p>$n_{CH_4}=n^0_{CH_4}+\xi$</p>
</li>
<li>
<p>$n_{CH_4}=\xi \hspace{3 mm}[n^0_{CH_4=0}]$</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-04-chemical-kinetics-l-4_16-kicxcenhv8u-11.jpg"></p>

</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ Rate of reaction $\rightarrow$ Rate of reaction in terms of reactants $\rightarrow$ Rate of reaction in terms of products $\rightarrow$ General reaction $\rightarrow$ Stoichiometric coefficients $\rightarrow$ Example of stoichiometric coefficient $\rightarrow$ Reaction $\rightarrow$ Rate of reaction $\rightarrow$ Example $\rightarrow$ <span style="color:blue">Rate of reaction</span> </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-4</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Rate of reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$n_{CO}=n^0_{CO}(=0) + \nu_i \xi (+1)$</p>
</li>
<li>
<p>$n_{CO}=0+\xi$</p>
</li>
<li>
<p>$n_{CO}=\xi$</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-04-chemical-kinetics-l-4_16-kicxcenhv8u-630-3379.2.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic reaction profile $\rightarrow$ Rate of reaction $\rightarrow$ Rate of reaction in terms of reactants $\rightarrow$ Rate of reaction in terms of products $\rightarrow$ General reaction $\rightarrow$ Stoichiometric coefficients $\rightarrow$ Example of stoichiometric coefficient $\rightarrow$ Reaction $\rightarrow$ Rate of reaction $\rightarrow$ Example $\rightarrow$ <span style="color:blue">Rate of reaction</span> </footer>