chemistry-class-12-unit-04-chapter-11-chemical-kinetics-l-11-16-alfbsjxt9l4

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-11</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>
<p>Reaction rates depend upon temperature</p>
<ul>
<li>Increase in temperature in general leads to increase in the rate of a reaction</li>
</ul>
</li>
</ul>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-11-chemical-kinetics-l-11_16-alfbsjxt9l4-017-0054.0.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> <span style="color:blue">Temperature dependence of reaction rates</span> $\rightarrow$ Arrhenius equation $\rightarrow$ Van't Hoff equation $\rightarrow$ Arrhenius importance $\rightarrow$ Inversion of cane sugar $\rightarrow$ Reaction Coordinate $\rightarrow$ Relation between H and U $\rightarrow$ Gas-phase reactions $\rightarrow$ Important point $\rightarrow$ Maxwell and boltzmann distribution curve $\rightarrow$ Fraction of molecules vs kinetic energy curve </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-11</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Arrhenius equation</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>k = A$e^{-Ea/RT} \cdots$ 1(a)</p>
</li>
<li>
<p>k = A exp ($\frac{-E_a}{RT}$) $\cdots$ 1(b)</p>
</li>
</ul>
<ul>
<li>
<p>Where-</p>
<ul>
<li>
<p>A - Pre-exponential factor or frequency factor or arrhenius factor</p>
</li>
<li>
<p>$E_a$ - Activation energy arrhenius activation energy</p>
</li>
<li>
<p>k - rate constant</p>
</li>
<li>
<p>R - gas constant</p>
</li>
</ul>
</li>
</ul>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-11-chemical-kinetics-l-11_16-alfbsjxt9l4-026-0111.6.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-11-chemical-kinetics-l-11_16-alfbsjxt9l4-037-0142.8.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Temperature dependence of reaction rates $\rightarrow$ <span style="color:blue">Arrhenius equation</span> $\rightarrow$ Van't Hoff equation $\rightarrow$ Arrhenius importance $\rightarrow$ Inversion of cane sugar $\rightarrow$ Reaction Coordinate $\rightarrow$ Relation between H and U $\rightarrow$ Gas-phase reactions $\rightarrow$ Important point $\rightarrow$ Maxwell and boltzmann distribution curve $\rightarrow$ Fraction of molecules vs kinetic energy curve </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-11</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Van’t Hoff equation</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$(\frac{∂ lnKc}{∂T})_p=\frac{\Delta U^o}{RT^2}……(2)$</p>
</li>
<li>
<p>$K_c=\frac{k_1}{k_{-1}}$</p>
</li>
<li>
<p>$\frac{d ln^{k_1/k_{-1}}}{dt}=\frac{\Delta U^o}{RT^2}$</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-11-chemical-kinetics-l-11_16-alfbsjxt9l4-01.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Temperature dependence of reaction rates $\rightarrow$ <span style="color:blue">Arrhenius equation</span> $\rightarrow$ Van't Hoff equation $\rightarrow$ Arrhenius importance $\rightarrow$ Inversion of cane sugar $\rightarrow$ Reaction Coordinate $\rightarrow$ Relation between H and U $\rightarrow$ Gas-phase reactions $\rightarrow$ Important point $\rightarrow$ Maxwell and boltzmann distribution curve $\rightarrow$ Fraction of molecules vs kinetic energy curve </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-11</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Van’t Hoff equation</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>Van’t hoft argued$\rarr k_1$ and $k_{-1}$ will be influenced by 2 different</p>
</li>
<li>
<p>Energy factors : $E_1$ and $E_{-1}$</p>
</li>
</ul>
<ul>
<li>
<p>$\frac{d (ln k_1)}{dT}=\frac{E_1}{RT^2}$</p>
</li>
<li>
<p>$\frac{d (ln k_{-1})}{dT}=\frac{E_{-1}}{RT^2}$</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-11-chemical-kinetics-l-11_16-alfbsjxt9l4-090-0384.0.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Temperature dependence of reaction rates $\rightarrow$ Arrhenius equation $\rightarrow$ <span style="color:blue">Van't Hoff equation</span> $\rightarrow$ Arrhenius importance $\rightarrow$ Inversion of cane sugar $\rightarrow$ Reaction Coordinate $\rightarrow$ Relation between H and U $\rightarrow$ Gas-phase reactions $\rightarrow$ Important point $\rightarrow$ Maxwell and boltzmann distribution curve $\rightarrow$ Fraction of molecules vs kinetic energy curve </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-11</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Van’t Hoff equation</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$E_1 - E_2=\Delta U^o $</p>
</li>
<li>
<p>$\frac{d (lnk)} {dT}=\frac{E}{RT^2}$</p>
</li>
<li>
<p>ln k $\hspace{2mm}$ = $\hspace{2mm}$constant$-\frac{E}{RT}$</p>
</li>
<li>
<p>k = A$e^{-Ea/RT}$</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-11-chemical-kinetics-l-11_16-alfbsjxt9l4-117-0486.0.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-11-chemical-kinetics-l-11_16-alfbsjxt9l4-090-0384.0.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Temperature dependence of reaction rates $\rightarrow$ Arrhenius equation $\rightarrow$ <span style="color:blue">Van't Hoff equation</span> $\rightarrow$ Arrhenius importance $\rightarrow$ Inversion of cane sugar $\rightarrow$ Reaction Coordinate $\rightarrow$ Relation between H and U $\rightarrow$ Gas-phase reactions $\rightarrow$ Important point $\rightarrow$ Maxwell and boltzmann distribution curve $\rightarrow$ Fraction of molecules vs kinetic energy curve </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-11</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Arrhenius importance</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>This is a general concept of how reactions occur</p>
<ul>
<li>An equilibrium is established between ’normal’ and ‘active’ reactant molecules</li>
</ul>
</li>
</ul>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-11-chemical-kinetics-l-11_16-alfbsjxt9l4-172-0748.8.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-11-chemical-kinetics-l-11_16-alfbsjxt9l4-117-0486.0.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Temperature dependence of reaction rates $\rightarrow$ Arrhenius equation $\rightarrow$ Van't Hoff equation $\rightarrow$ <span style="color:blue">Arrhenius importance</span> $\rightarrow$ Inversion of cane sugar $\rightarrow$ Reaction Coordinate $\rightarrow$ Relation between H and U $\rightarrow$ Gas-phase reactions $\rightarrow$ Important point $\rightarrow$ Maxwell and boltzmann distribution curve $\rightarrow$ Fraction of molecules vs kinetic energy curve </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-11</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Inversion of cane sugar</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>Inversion was not brought about by a simple cane sugar molecule but a substance he mentioned as active cane sugar molecule</p>
</li>
<li>
<p>Rate of reaction</p>
<p>$\quad \quad \downarrow$ proportional</p>
</li>
</ul>
<ul>
<li>Active cane sugar molecules</li>
</ul>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-11-chemical-kinetics-l-11_16-alfbsjxt9l4-208-0940.8.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-11-chemical-kinetics-l-11_16-alfbsjxt9l4-212-0980.4.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Temperature dependence of reaction rates $\rightarrow$ Arrhenius equation $\rightarrow$ Van't Hoff equation $\rightarrow$ Arrhenius importance $\rightarrow$ <span style="color:blue">Inversion of cane sugar</span> $\rightarrow$ Reaction Coordinate $\rightarrow$ Relation between H and U $\rightarrow$ Gas-phase reactions $\rightarrow$ Important point $\rightarrow$ Maxwell and boltzmann distribution curve $\rightarrow$ Fraction of molecules vs kinetic energy curve </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-11</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Relation between H and U</B></primary></p>
<hr>
<main>
<div style='float: left; width:60%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$H = U + PV$</p>
</li>
<li>
<p>$\Delta H=\Delta U + \Delta(PV)$</p>
</li>
<li>
<p>$\Delta H=\Delta U + P\Delta V + V\Delta P$</p>
</li>
<li>
<p>$\frac{d(lnK_c)}{dt};(\frac{\partial (InK_c)}{\partial T})_p$</p>
</li>
</ul>
</div>
<div style='float: right; width:40%;'>
<img src ="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/932c5eb1-0228-4eb5-2e4c-c5a47b873700/public" style='width:90%;'>


</div>
</main>
<hr>
<footer style="font-size:18px;"> Temperature dependence of reaction rates $\rightarrow$ Arrhenius equation $\rightarrow$ Van't Hoff equation $\rightarrow$ Arrhenius importance $\rightarrow$ Inversion of cane sugar $\rightarrow$ Reaction Coordinate $\rightarrow$ <span style="color:blue">Relation between H and U</span> $\rightarrow$ Gas-phase reactions $\rightarrow$ Important point $\rightarrow$ Maxwell and boltzmann distribution curve $\rightarrow$ Fraction of molecules vs kinetic energy curve </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-11</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Relation between H and U</B></primary></p>
<hr>
<main>
<div style='float: left; width:60%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$\Delta H=\Delta U + P\Delta V + V\Delta P$</p>
</li>
<li>
<p>at constant pressure, $\Delta P=0$</p>
</li>
<li>
<p>$\Delta H=\Delta U + P \Delta V$</p>
</li>
<li>
<p>For reactions in solids & solutions,$\Delta V≈0$</p>
</li>
<li>
<p>$\Delta H=\Delta U$</p>
</li>
</ul>
</div>
<div style='float: right; width:40%;'>
<img src ="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/932c5eb1-0228-4eb5-2e4c-c5a47b873700/public" style='width:100%;'>


</div>
</main>
<hr>
<footer style="font-size:18px;"> Temperature dependence of reaction rates $\rightarrow$ Arrhenius equation $\rightarrow$ Van't Hoff equation $\rightarrow$ Arrhenius importance $\rightarrow$ Inversion of cane sugar $\rightarrow$ Reaction Coordinate $\rightarrow$ <span style="color:blue">Relation between H and U</span> $\rightarrow$ Gas-phase reactions $\rightarrow$ Important point $\rightarrow$ Maxwell and boltzmann distribution curve $\rightarrow$ Fraction of molecules vs kinetic energy curve </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-11</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Gas-phase reactions</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$P\Delta V = \Delta nRT$</p>
</li>
<li>
<p>$\Delta H =\Delta U = \Delta nRT$</p>
</li>
<li>
<p>$\Delta n$ = Change in number of moles</p>
</li>
<li>
<p>if $\Delta n = 0, then \hspace{3mm}\Delta H=\Delta U$</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-11-chemical-kinetics-l-11_16-alfbsjxt9l4-422-1764.0.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Temperature dependence of reaction rates $\rightarrow$ Arrhenius equation $\rightarrow$ Van't Hoff equation $\rightarrow$ Arrhenius importance $\rightarrow$ Inversion of cane sugar $\rightarrow$ Reaction Coordinate $\rightarrow$ Relation between H and U $\rightarrow$ <span style="color:blue">Gas-phase reactions</span> $\rightarrow$ Important point $\rightarrow$ Maxwell and boltzmann distribution curve $\rightarrow$ Fraction of molecules vs kinetic energy curve </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-11</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Important point</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>Suppose there  is a system having 1 mole of gaseous reactants</li>
</ul>
<ul>
<li>1 $mole=6.023×10^{23}$ molecules</li>
</ul>
<ul>
<li>At a certain temperature, all molecules in the system do not have the same kinetic energy</li>
</ul>
<ul>
<li>
<p>A distribution of kinetic energies exist in the system</p>
<p>$\quad \quad \quad \quad \quad \downarrow$</p>
</li>
</ul>
<ul>
<li>Distribution depends on temperature</li>
</ul>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-11-chemical-kinetics-l-11_16-alfbsjxt9l4-02.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Temperature dependence of reaction rates $\rightarrow$ Arrhenius equation $\rightarrow$ Van't Hoff equation $\rightarrow$ Arrhenius importance $\rightarrow$ Inversion of cane sugar $\rightarrow$ Reaction Coordinate $\rightarrow$ Relation between H and U $\rightarrow$ Gas-phase reactions $\rightarrow$ <span style="color:blue">Important point</span> $\rightarrow$ Maxwell and boltzmann distribution curve $\rightarrow$ Fraction of molecules vs kinetic energy curve </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-11</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Maxwell and boltzmann distribution curve</B></primary></p>
<hr>
<main>
<div style='float: left; width:60%;font-size:22px;text-align:left'>
<ul>
<li>
<p>Total number of molecules is N</p>
</li>
<li>
<p>Fraction = $\frac{N_E}{N}$</p>
</li>
<li>
<p>$N_E$ is the number of molecules having kinetic energy E</p>
</li>
<li>
<p>Peak of distribution $\rarr$ most probable kinetic energy</p>
</li>
</ul>
</div>
<div style='float: right; width:40%;'>
<img src ="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/4351a025-bf97-4445-7e75-e22287930700/public" style='width:100%;'>


</div>
</main>
<hr>
<footer style="font-size:18px;"> Temperature dependence of reaction rates $\rightarrow$ Arrhenius equation $\rightarrow$ Van't Hoff equation $\rightarrow$ Arrhenius importance $\rightarrow$ Inversion of cane sugar $\rightarrow$ Reaction Coordinate $\rightarrow$ Relation between H and U $\rightarrow$ Gas-phase reactions $\rightarrow$ Important point $\rightarrow$ <span style="color:blue">Maxwell and boltzmann distribution curve</span> $\rightarrow$ Fraction of molecules vs kinetic energy curve </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-11</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Fraction of molecules vs kinetic energy curve</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li><strong>As temperature is increased</strong></li>
</ul>
<ul>
<li>
<p>The distribution becomes broader</p>
</li>
<li>
<p>The peak of distribution shifts to higher value of kinetic Energy</p>
</li>
<li>
<p>The shaded portion which shows the fraction of molecules having energy more than Ea and area of shaded portion increases as the temperature is increased</p>
</li>
<li>
<p>Fraction of molecules having excess energy is energy in excess of Ea is given by  $e^{-E_a/RT}$</p>
<p>$\quad \quad \downarrow$</p>
</li>
</ul>
<ul>
<li>$k=Ae^{-Ea/RT}$</li>
</ul>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-11-chemical-kinetics-l-11_16-alfbsjxt9l4-710-3142.8.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Temperature dependence of reaction rates $\rightarrow$ Arrhenius equation $\rightarrow$ Van't Hoff equation $\rightarrow$ Arrhenius importance $\rightarrow$ Inversion of cane sugar $\rightarrow$ Reaction Coordinate $\rightarrow$ Relation between H and U $\rightarrow$ Gas-phase reactions $\rightarrow$ Important point $\rightarrow$ Maxwell and boltzmann distribution curve $\rightarrow$ <span style="color:blue">Fraction of molecules vs kinetic energy curve</span> </footer>