chemistry-class-12-unit-04-chapter-06-chemical-kinetics-l-6-16-q1pgfcj4iuo

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-6</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Kinetic analysis of experimental data</B></primary></p>
<hr>
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<div style='float: left; width:60%;font-size:22px;text-align:left'>
<ul>
<li>
<p>Average rate -</p>
</li>
<li>
<p>$Average\hspace{2 mm} rate=-\frac{c_3-c_1}{t_3-t_1}$</p>
</li>
<li>
<p>$=-\frac{\Delta c}{\Delta t}$</p>
</li>
</ul>
</div>
<div style='float: right; width:40%;'>

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</main>
<hr>
<footer style="font-size:18px;"> <span style="color:blue">Kinetic analysis of experimental data</span> $\rightarrow$ Instantaneous rate $\rightarrow$ Initial rate of reaction $\rightarrow$ Key points $\rightarrow$ Dependence of reaction rate on concentration $\rightarrow$ Rate of reaction including 2 reactants, A and B $\rightarrow$ Rate of reaction general reaction $\rightarrow$ Key points $\rightarrow$ Units of rate $\rightarrow$ Meaning of rate expression $\rightarrow$ Units of rate constant $\rightarrow$ Example </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-6</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>By drawing 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 - $r_ {inst}=\frac{d[P]}{dt}$  $P\rArr product$</p>
</li>
</ul>
</div>
<div style='float: right; width:40%;'>


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</main>
<hr>
<footer style="font-size:18px;"> Kinetic analysis of experimental data $\rightarrow$ <span style="color:blue">Instantaneous rate</span> $\rightarrow$ Initial rate of reaction $\rightarrow$ Key points $\rightarrow$ Dependence of reaction rate on concentration $\rightarrow$ Rate of reaction including 2 reactants, A and B $\rightarrow$ Rate of reaction general reaction $\rightarrow$ Key points $\rightarrow$ Units of rate $\rightarrow$ Meaning of rate expression $\rightarrow$ Units of rate constant $\rightarrow$ Example </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-6</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Initial rate of reaction</B></primary></p>
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<div style='float: left; width:100%;font-size:22px;text-align:left'>
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</main>
<hr>
<footer style="font-size:18px;"> Kinetic analysis of experimental data $\rightarrow$ Instantaneous rate $\rightarrow$ <span style="color:blue">Initial rate of reaction</span> $\rightarrow$ Key points $\rightarrow$ Dependence of reaction rate on concentration $\rightarrow$ Rate of reaction including 2 reactants, A and B $\rightarrow$ Rate of reaction general reaction $\rightarrow$ Key points $\rightarrow$ Units of rate $\rightarrow$ Meaning of rate expression $\rightarrow$ Units of rate constant $\rightarrow$ Example </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-6</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 $\rarr$ within 5% of the reaction</p>
</li>
<li>
<p><strong>Except chain reactions</strong></p>
</li>
<li>
<p>The initial rate line or tangent will be the one which is the steepest</p>
</li>
</ul>
</div>
<div style='float: right; width:0%;'>

</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic analysis of experimental data $\rightarrow$ Instantaneous rate $\rightarrow$ Initial rate of reaction $\rightarrow$ <span style="color:blue">Key points</span> $\rightarrow$ Dependence of reaction rate on concentration $\rightarrow$ Rate of reaction including 2 reactants, A and B $\rightarrow$ Rate of reaction general reaction $\rightarrow$ Key points $\rightarrow$ Units of rate $\rightarrow$ Meaning of rate expression $\rightarrow$ Units of rate constant $\rightarrow$ Example </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-6</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Dependence of reaction rate on concentration</B></primary></p>
<hr>
<main>
<div style='float: left; width:65%;font-size:22px;text-align:left'>
<ul>
<li>
<p>The rate of reaction is in some way dependent on the concentration of the reactant remaining</p>
</li>
<li>
<p>Way dependent on the concentration of the reactant remaining</p>
</li>
<li>
<p>rate $\alpha$ $[reactant]^n$ $\dots$(1)</p>
</li>
<li>
<p>n$\rArr$ is a number which states exactly how the rate depends on [reactant]</p>
</li>
</ul>
</div>
<div style='float: right; width:35%;'>



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</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic analysis of experimental data $\rightarrow$ Instantaneous rate $\rightarrow$ Initial rate of reaction $\rightarrow$ Key points $\rightarrow$ <span style="color:blue">Dependence of reaction rate on concentration</span> $\rightarrow$ Rate of reaction including 2 reactants, A and B $\rightarrow$ Rate of reaction general reaction $\rightarrow$ Key points $\rightarrow$ Units of rate $\rightarrow$ Meaning of rate expression $\rightarrow$ Units of rate constant $\rightarrow$ Example </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-6</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Dependence of reaction rate on concentration</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>Where n = order of the reaction rate = $k[reactant]^n$ $\dots$(2)</p>
</li>
<li>
<p>k is the constant of proportionality rate constant</p>
</li>
<li>
<p>If, n = 1 , first order reaction</p>
</li>
<li>
<p>n = 2 , second order reaction</p>
</li>
<li>
<p>n = 3 , third order reaction</p>
</li>
<li>
<p>n = 0, zero order reaction</p>
</li>
<li>
<p>n = 3/2 , fractional order</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-06-chemical-kinetics-l-6_16-q1pgfcj4iuo-192-0777.6.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-06-chemical-kinetics-l-6_16-q1pgfcj4iuo-203-0872.4.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic analysis of experimental data $\rightarrow$ Instantaneous rate $\rightarrow$ Initial rate of reaction $\rightarrow$ Key points $\rightarrow$ <span style="color:blue">Dependence of reaction rate on concentration</span> $\rightarrow$ Rate of reaction including 2 reactants, A and B $\rightarrow$ Rate of reaction general reaction $\rightarrow$ Key points $\rightarrow$ Units of rate $\rightarrow$ Meaning of rate expression $\rightarrow$ Units of rate constant $\rightarrow$ Example </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-6</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Rate of reaction including 2 reactants, A and B</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>Rate = $K[A]^2[B]\dots(4)$</p>
</li>
<li>
<p>Second order with respect to A</p>
</li>
<li>
<p>First order with respect to B</p>
</li>
<li>
<p>Total order = 2+1 = 3</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-06-chemical-kinetics-l-6_16-q1pgfcj4iuo-273-1112.4.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-06-chemical-kinetics-l-6_16-q1pgfcj4iuo-305-1233.6.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic analysis of experimental data $\rightarrow$ Instantaneous rate $\rightarrow$ Initial rate of reaction $\rightarrow$ Key points $\rightarrow$ Dependence of reaction rate on concentration $\rightarrow$ <span style="color:blue">Rate of reaction including 2 reactants, A and B</span> $\rightarrow$ Rate of reaction general reaction $\rightarrow$ Key points $\rightarrow$ Units of rate $\rightarrow$ Meaning of rate expression $\rightarrow$ Units of rate constant $\rightarrow$ Example </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-6</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>One concentration form for each reactant</p>
</li>
<li>
<p>Each concentration term is raised to a particular power - $\alpha , \beta , \gamma…$</p>
</li>
<li>
<p>Kinetic analysis -</p>
</li>
<li>
<p>Find the value of $\alpha , \beta , \gamma…$</p>
</li>
<li>
<p>k rate constant at a certain 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-06-chemical-kinetics-l-6_16-q1pgfcj4iuo-02.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic analysis of experimental data $\rightarrow$ Instantaneous rate $\rightarrow$ Initial rate of reaction $\rightarrow$ Key points $\rightarrow$ Dependence of reaction rate on concentration $\rightarrow$ Rate of reaction including 2 reactants, A and B $\rightarrow$ Rate of reaction general reaction $\rightarrow$ <span style="color:blue">Key points</span> $\rightarrow$ Units of rate $\rightarrow$ Meaning of rate expression $\rightarrow$ Units of rate constant $\rightarrow$ Example </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-6</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Units of rate</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>For gaseous reactions</li>
</ul>
<p>$\frac{atm}{time}$ $\hspace{2mm}$ atm $time^{-1}$</p>
<p>If time is in seconds</p>
<p>$Ms^{-1}$ or $molL^{-1}s^{-1}$ or $atm s^{-1}$</p>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-06-chemical-kinetics-l-6_16-q1pgfcj4iuo-03.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-06-chemical-kinetics-l-6_16-q1pgfcj4iuo-528-2095.199.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic analysis of experimental data $\rightarrow$ Instantaneous rate $\rightarrow$ Initial rate of reaction $\rightarrow$ Key points $\rightarrow$ Dependence of reaction rate on concentration $\rightarrow$ Rate of reaction including 2 reactants, A and B $\rightarrow$ Rate of reaction general reaction $\rightarrow$ Key points $\rightarrow$ <span style="color:blue">Units of rate</span> $\rightarrow$ Meaning of rate expression $\rightarrow$ Units of rate constant $\rightarrow$ Example </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-6</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Meaning of rate expression</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>$rate=k[A]$ $\quad$  first order reaction</li>
</ul>
<ul>
<li>If [A] is increased by a factor of 2 , then the rate also increased by a factor of 2</li>
<li>If [A] is increased by a factor of 6 , rate is also increased by the factor of 6</li>
</ul>
<ul>
<li>$rate = k[A]^2$ $\quad$ second order reaction</li>
</ul>
<ul>
<li>If concentration of A is increased by a factor of 2 , then rate is increased by a factor of $2^2 = 4$</li>
<li>If concentration of A is increased by a factor of 6 , the rate is increased by a factor of $6^2 = 36$</li>
</ul>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-06-chemical-kinetics-l-6_16-q1pgfcj4iuo-04.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-06-chemical-kinetics-l-6_16-q1pgfcj4iuo-568-2256.0.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-06-chemical-kinetics-l-6_16-q1pgfcj4iuo-591-2395.2.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic analysis of experimental data $\rightarrow$ Instantaneous rate $\rightarrow$ Initial rate of reaction $\rightarrow$ Key points $\rightarrow$ Dependence of reaction rate on concentration $\rightarrow$ Rate of reaction including 2 reactants, A and B $\rightarrow$ Rate of reaction general reaction $\rightarrow$ Key points $\rightarrow$ Units of rate $\rightarrow$ <span style="color:blue">Meaning of rate expression</span> $\rightarrow$ Units of rate constant $\rightarrow$ Example </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-6</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Units of rate constant</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>First order reaction</li>
</ul>
<ul>
<li>rate = k[A]</li>
<li>$k = \frac{rate}{[A]}=\frac{rate}{molL^{-1}}$</li>
<li>$k = \frac{rate}{[A]}$ $=\frac{molL^{-1}time^{-1}}{molL^{-1}}$</li>
<li>$k = time^{-1}$</li>
<li>$k = s^{-1};min^{-1};h^{-1}$</li>
</ul>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-06-chemical-kinetics-l-6_16-q1pgfcj4iuo-05.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-06-chemical-kinetics-l-6_16-q1pgfcj4iuo-651-2647.2.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-06-chemical-kinetics-l-6_16-q1pgfcj4iuo-667-2707.2.jpg">
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</main>
<hr>
<footer style="font-size:18px;"> Kinetic analysis of experimental data $\rightarrow$ Instantaneous rate $\rightarrow$ Initial rate of reaction $\rightarrow$ Key points $\rightarrow$ Dependence of reaction rate on concentration $\rightarrow$ Rate of reaction including 2 reactants, A and B $\rightarrow$ Rate of reaction general reaction $\rightarrow$ Key points $\rightarrow$ Units of rate $\rightarrow$ Meaning of rate expression $\rightarrow$ <span style="color:blue">Units of rate constant</span> $\rightarrow$ Example </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-6</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Units of rate constant</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>Second order reaction</li>
</ul>
<ul>
<li>$rate = k[A]^2$</li>
<li>$k = \frac{rate}{[A]^2}$ $ = \frac{molL^{-1}time^{-1}}{(molL^{-1})^2}$</li>
<li>$ = mol^{-1}Ltime^{-1} = L mol^{-1}time^{-1}$</li>
</ul>
<ul>
<li>Zero order reaction</li>
</ul>
<ul>
<li>$rate = k[A]^o$</li>
<li>rate = k</li>
<li>unit  of  k = $molL^{-1} time^{-1}$</li>
</ul>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-06-chemical-kinetics-l-6_16-q1pgfcj4iuo-740-2960.4.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic analysis of experimental data $\rightarrow$ Instantaneous rate $\rightarrow$ Initial rate of reaction $\rightarrow$ Key points $\rightarrow$ Dependence of reaction rate on concentration $\rightarrow$ Rate of reaction including 2 reactants, A and B $\rightarrow$ Rate of reaction general reaction $\rightarrow$ Key points $\rightarrow$ Units of rate $\rightarrow$ Meaning of rate expression $\rightarrow$ <span style="color:blue">Units of rate constant</span> $\rightarrow$ Example </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-6</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>$rate = k[A][B]$</p>
</li>
<li>
<p>overall order = 1+1 = 2</p>
</li>
<li>
<p>$k=\frac{rate}{[A][B]}$ $=\frac{molL^{-1} min^{-1}}{[molL^{-1}][molL^{-1}]} = L mol^{-1} min^{-1}$</p>
</li>
</ul>
</p>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-06-chemical-kinetics-l-6_16-q1pgfcj4iuo-771-3106.8.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-06-chemical-kinetics-l-6_16-q1pgfcj4iuo-804-3252.0.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Kinetic analysis of experimental data $\rightarrow$ Instantaneous rate $\rightarrow$ Initial rate of reaction $\rightarrow$ Key points $\rightarrow$ Dependence of reaction rate on concentration $\rightarrow$ Rate of reaction including 2 reactants, A and B $\rightarrow$ Rate of reaction general reaction $\rightarrow$ Key points $\rightarrow$ Units of rate $\rightarrow$ Meaning of rate expression $\rightarrow$ Units of rate constant $\rightarrow$ <span style="color:blue">Example</span> </footer>