chemistry-class-12-unit-04-chapter-05-chemical-kinetics-l-5-16-qgiyys7-clm

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-5</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>$CH_3CHO(g) \rightarrow$ $CH_4(g)+ CO(g)$</p>
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<li>
<p>$n^o_{CH_3CHO}$ $ \quad \quad \quad$ $0$ $\quad \quad \quad \quad$ $0$</p>
</li>
<li>
<p>$n^o_{CH_3CHO}-\xi$ $\quad \quad$ $\xi$ $\quad\quad\quad\quad \xi$</p>
</li>
<li>
<p><strong>Example</strong>-</p>
</li>
<li>
<p>$CH_3CHO (g) \rightarrow$ $CH_4 (g)+ CO (g)$</p>
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<li>
<p>The rate of this reaction can be followed by measuring the pressure in the system at constant volume and temperature</p>
</li>
</ul>
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<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-05-chemical-kinetics-l-5_16-qgiyys7-clm-027-0104.4.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-05-chemical-kinetics-l-5_16-qgiyys7-clm-27.jpg"></p>
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<footer style="font-size:18px;"> <span style="color:blue">Rate of reaction</span> $\rightarrow$ Assume ideal gas behaviour of the gases $\rightarrow$ Expression of the total pressure $\rightarrow$ Kinetic analysis of experimental data $\rightarrow$ Kinetic reaction profile $\rightarrow$ Instantaneous rate $\rightarrow$ Initial rate of reaction $\rightarrow$ Key points $\rightarrow$ Dependence of reaction rate on concentration </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-5</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Assume ideal gas behaviour of the gases</B></primary></p>
<hr>
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<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$n_{CH_4} =\xi$ $\quad [n^o_{CH_4} = 0]$</p>
</li>
<li>
<p>$n_{CO} = n^o_{CO} + v_i$ $\xi$</p>
</li>
<li>
<p>$n_{CO} = 0$ + $\xi$</p>
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<li>
<p>$n_{CO}$ =$\xi$</p>
</li>
</ul>
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<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-05-chemical-kinetics-l-5_16-qgiyys7-clm-032-0117.6.jpg"></p>
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<hr>
<footer style="font-size:18px;"> Rate of reaction $\rightarrow$ <span style="color:blue">Assume ideal gas behaviour of the gases</span> $\rightarrow$ Expression of the total pressure $\rightarrow$ Kinetic analysis of experimental data $\rightarrow$ Kinetic reaction profile $\rightarrow$ Instantaneous rate $\rightarrow$ Initial rate of reaction $\rightarrow$ Key points $\rightarrow$ Dependence of reaction rate on concentration </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-5</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Expression of the total pressure</B></primary></p>
<hr>
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<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p><strong>Initial number of moles</strong></p>
</li>
<li>
<p>$n^o_{CH_3CHO} = n^0$</p>
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<li>
<p><strong>Total pressure</strong> $=P_{CH_3CHO} + P_{CH_4} + P_{CO}$</p>
</li>
<li>
<p>ideal  gas $PV = n RT$</p>
</li>
<li>
<p>$P_{CH_3CHO} = (n^o-\xi)$ $\frac{RT}{V}$</p>
</li>
<li>
<p>$ P_{CH_4}$ = $\xi$ $\frac{RT}{V}$</p>
</li>
<li>
<p>$P_{CO}$ = $\xi$ $\frac{RT}{V}$</p>
</li>
</ul>
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<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-05-chemical-kinetics-l-5_16-qgiyys7-clm-074-0265.2.jpg"></p>
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<hr>
<footer style="font-size:18px;"> Rate of reaction $\rightarrow$ Assume ideal gas behaviour of the gases $\rightarrow$ <span style="color:blue">Expression of the total pressure</span> $\rightarrow$ Kinetic analysis of experimental data $\rightarrow$ Kinetic reaction profile $\rightarrow$ Instantaneous rate $\rightarrow$ Initial rate of reaction $\rightarrow$ Key points $\rightarrow$ Dependence of reaction rate on concentration </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-5</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Expression of the total pressure</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p><strong>Go for expression of the total pressure</strong></p>
</li>
<li>
<p>$P_{total}$ = $P_{CH_3CHO} + P_{CH_4} + P_{CO} $</p>
</li>
<li>
<p>$P = [(n^0-\xi)+ \xi + \xi] \frac{R T}{V}$</p>
</li>
<li>
<p>$p = (n^o + \xi) \frac{R T}{V}$</p>
</li>
<li>
<p>$p = \frac{n^o R T}{V}+ \frac{\xi R T}{V}$</p>
</li>
<li>
<p>$n^o$ was the initial number of moles</p>
</li>
<li>
<p>$\frac{n^o R T}{V} \rightarrow$ initial pressure $P^o $</p>
</li>
</ul>
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<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-05-chemical-kinetics-l-5_16-qgiyys7-clm-01.jpg"></p>

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</main>
<hr>
<footer style="font-size:18px;"> Rate of reaction $\rightarrow$ Assume ideal gas behaviour of the gases $\rightarrow$ <span style="color:blue">Expression of the total pressure</span> $\rightarrow$ Kinetic analysis of experimental data $\rightarrow$ Kinetic reaction profile $\rightarrow$ Instantaneous rate $\rightarrow$ Initial rate of reaction $\rightarrow$ Key points $\rightarrow$ Dependence of reaction rate on concentration </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-5</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Expression of the total pressure</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$P = P^o + \frac {\xi RT}{V}$</p>
</li>
<li>
<p>$\frac{dP}{dt} = \frac{dP^o}{dt} + \frac{d}{dt} [\xi \frac{RT}{V}] $</p>
</li>
<li>
<p>$\frac{dP}{dt} = \frac{RT}{V} \frac{d\xi}{dt}$</p>
</li>
<li>
<p>$\frac{dP}{dt} = \frac{RT}{V} \frac{d \xi}{dt}$</p>
</li>
<li>
<p>$\frac{1}{V} \frac{d \xi}{dt} = \frac{1}{RT} \frac{dP}{dt}$</p>
</li>
</ul>
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<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-05-chemical-kinetics-l-5_16-qgiyys7-clm-144-0556.8.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-05-chemical-kinetics-l-5_16-qgiyys7-clm-165-0690.0.jpg"></p>
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<hr>
<footer style="font-size:18px;"> Rate of reaction $\rightarrow$ Assume ideal gas behaviour of the gases $\rightarrow$ <span style="color:blue">Expression of the total pressure</span> $\rightarrow$ Kinetic analysis of experimental data $\rightarrow$ Kinetic reaction profile $\rightarrow$ Instantaneous rate $\rightarrow$ Initial rate of reaction $\rightarrow$ Key points $\rightarrow$ Dependence of reaction rate on concentration </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-5</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Instantaneous rate</B></primary></p>
<hr>
<main>
<div style='float: left; width:60%;font-size:22px;text-align:left'>
<ul>
<li>
<p>Bydrawing a catalyst a tangent at that instant or that time point,$t_1$</p>
</li>
<li>
<p>Take the slope of the tangent</p>
</li>
<li>
<p>For products:$r_{(inst)}= \frac{d[P]}{dt}$</p>
</li>
</ul>
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<img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/e41ae8ea-22fb-4747-8f54-8e8b7f89a800/public" width="80%">


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<hr>
<footer style="font-size:18px;"> Rate of reaction $\rightarrow$ Assume ideal gas behaviour of the gases $\rightarrow$ Expression of the total pressure $\rightarrow$ Kinetic analysis of experimental data $\rightarrow$ Kinetic reaction profile $\rightarrow$ <span style="color:blue">Instantaneous rate</span> $\rightarrow$ Initial rate of reaction $\rightarrow$ Key points $\rightarrow$ Dependence of reaction rate on concentration </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-5</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Key points</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>It is preferred to do the initial rate calculation based on product appearance</p>
</li>
<li>
<p>Initial rate calculation has to be done very close to the starting point of the reaction $\rightarrow $ within 5% of the reaction</p>
</li>
<li>
<p>Except chain reactions the initial rate line or tangent will be the one which is the steepest</p>
</li>
</ul>
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<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-05-chemical-kinetics-l-5_16-qgiyys7-clm-469-2344.8.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Rate of reaction $\rightarrow$ Assume ideal gas behaviour of the gases $\rightarrow$ Expression of the total pressure $\rightarrow$ Kinetic analysis of experimental data $\rightarrow$ Kinetic reaction profile $\rightarrow$ Instantaneous rate $\rightarrow$ Initial rate of reaction $\rightarrow$ <span style="color:blue">Key points</span> $\rightarrow$ Dependence of reaction rate on concentration </footer>