chemistry-class-12-unit-04-chapter-07-chemical-kinetics-l-7-16-ja-sqowih90

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-7</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>
<p>Second order reaction</p>
</li>
<li>
<p>$rate=k[A]^2$</p>
</li>
<li>
<p>$k=\frac{rate}{[A]^2}$ $=\frac{molL^{-1}time^{-1}}{(molL^{-1})^2}$</p>
</li>
<li>
<p>$k = mol^{-1}L \quad time^{-1}$</p>
</li>
<li>
<p>$k = L mol^{-1}time^{-1}$</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-07-chemical-kinetics-l-7_16-ja-sqowih90-022-0056.4.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-07-chemical-kinetics-l-7_16-ja-sqowih90-01.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-07-chemical-kinetics-l-7_16-ja-sqowih90-027-0076.8.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-07-chemical-kinetics-l-7_16-ja-sqowih90-030-0091.2.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> <span style="color:blue">Units of rate constant</span> $\rightarrow$ Example $\rightarrow$ Significance of rate and rate constant $\rightarrow$ Integrated rate laws $\rightarrow$ Zero order reaction $\rightarrow$ Half-life for a zero order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-7</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>
<p>Zero order reaction</p>
</li>
<li>
<p>$rate = k[A]^0$</p>
</li>
<li>
<p>rate = k</p>
</li>
<li>
<p>Unit  of  k = $mol L^{-1} time^{-1}$</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-07-chemical-kinetics-l-7_16-ja-sqowih90-022-0056.4.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-07-chemical-kinetics-l-7_16-ja-sqowih90-01.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-07-chemical-kinetics-l-7_16-ja-sqowih90-027-0076.8.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-07-chemical-kinetics-l-7_16-ja-sqowih90-030-0091.2.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> <span style="color:blue">Units of rate constant</span> $\rightarrow$ Example $\rightarrow$ Significance of rate and rate constant $\rightarrow$ Integrated rate laws $\rightarrow$ Zero order reaction $\rightarrow$ Half-life for a zero order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-7</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><strong>Reaction which is first order w.r.t.</strong></p>
<ul>
<li>
<p>A and first order w.r.t. B , reaction is happening between A and B.</p>
</li>
<li>
<p>Give the rate expression (assume time $\rarr$ minutes)</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-07-chemical-kinetics-l-7_16-ja-sqowih90-038-0110.4.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Units of rate constant $\rightarrow$ <span style="color:blue">Example</span> $\rightarrow$ Significance of rate and rate constant $\rightarrow$ Integrated rate laws $\rightarrow$ Zero order reaction $\rightarrow$ Half-life for a zero order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-7</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>$rate=k[A]^1[B]^1$</p>
</li>
<li>
<p>$rate=k[A][B]$</p>
</li>
<li>
<p>Overall order= 1 + 1 = 2</p>
</li>
<li>
<p>$k=\frac{rate}{[A][B]}$ $=\frac{molL^{-1} min^{-1}}{[molL^{-1}][molL^{-1}]}$</p>
</li>
<li>
<p>$k = L mol^{-1} min^{-1}$</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-07-chemical-kinetics-l-7_16-ja-sqowih90-038-0110.4.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-07-chemical-kinetics-l-7_16-ja-sqowih90-048-0145.2.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Units of rate constant $\rightarrow$ <span style="color:blue">Example</span> $\rightarrow$ Significance of rate and rate constant $\rightarrow$ Integrated rate laws $\rightarrow$ Zero order reaction $\rightarrow$ Half-life for a zero order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-7</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>Reaction between A and B</p>
<ul>
<li>
<p>First order w.r.t. A</p>
</li>
<li>
<p>Second order w.r.t. B</p>
</li>
<li>
<p>$rate=k[A]^1[B]^2$</p>
</li>
<li>
<p>$rate=k[A][B]^2$</p>
</li>
<li>
<p>Overall order= 1 + 2 = 3</p>
</li>
<li>
<p>$k=\frac{rate}{[A][B]^2}$ $=\frac{mol L^{-1} min^{-1}}{(mol L^{-1})(mol L^{-1})^2}$ $=L^2 mol^{-2} min^{-1}$</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-07-chemical-kinetics-l-7_16-ja-sqowih90-02.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Units of rate constant $\rightarrow$ <span style="color:blue">Example</span> $\rightarrow$ Significance of rate and rate constant $\rightarrow$ Integrated rate laws $\rightarrow$ Zero order reaction $\rightarrow$ Half-life for a zero order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-7</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Significance of rate and rate constant</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>Rate will vary with the concentrations of your reactants</p>
</li>
<li>
<p>Rate is not of much use in quantifying reactions or comparing reactions</p>
</li>
<li>
<p>Rate constant is a constant at a given temperature and is independent of the concent reactions of the reactants and can easily be used to quantify and compare reactions</p>
</li>
<li>
<p>If you know the rate constant and the order of the reaction, you can write down the rate expression for that reaction</p>
<ul>
<li>$rate=k[A]^n$</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-07-chemical-kinetics-l-7_16-ja-sqowih90-124-0435.6.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-07-chemical-kinetics-l-7_16-ja-sqowih90-03.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Units of rate constant $\rightarrow$ Example $\rightarrow$ <span style="color:blue">Significance of rate and rate constant</span> $\rightarrow$ Integrated rate laws $\rightarrow$ Zero order reaction $\rightarrow$ Half-life for a zero order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-7</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Integrated rate laws</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p><strong>Half-life</strong></p>
<ul>
<li>
<p>Preliminary check based on the kinetics profile</p>
</li>
<li>
<p>This is the time it takes for the concentration of the  reactant to fall to one-half of its initial value</p>
</li>
<li>
<p>By Wilhelm Ostwald nobel prize in 1909</p>
</li>
</ul>
</li>
</ul>
</div>
<div style='float: right; width:0%;'>


<img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/c4cf076f-3b4e-4db2-496c-010a7ef59e00/public" style='width:70%'>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Units of rate constant $\rightarrow$ Example $\rightarrow$ Significance of rate and rate constant $\rightarrow$ <span style="color:blue">Integrated rate laws</span> $\rightarrow$ Zero order reaction $\rightarrow$ Half-life for a zero order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-7</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Integrated rate laws</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$[A]_0 \rarr$ initial value of the reactant</p>
</li>
<li>
<p>$t_{1/2} \rarr$ half-life</p>
</li>
<li>
<p>$t_{1/2}(1) \rarr$ first half-life</p>
</li>
<li>
<p>$t_{1/2}(2)\rarr$ second half-life</p>
</li>
<li>
<p>$t_{1/2}(3)\rarr$ third half-life</p>
</li>
</ul>
</div>
<div style='float: right; width:0%;'>

<img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/8de2955c-60a9-4a83-8507-e9b4ee216900/public" style='width:70%'>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Units of rate constant $\rightarrow$ Example $\rightarrow$ Significance of rate and rate constant $\rightarrow$ <span style="color:blue">Integrated rate laws</span> $\rightarrow$ Zero order reaction $\rightarrow$ Half-life for a zero order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-7</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Zero order reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$A\rarr P$</p>
</li>
<li>
<p>$\text{rate}=k[A]^0=k \dots (1)$</p>
</li>
<li>
<p>$\frac{d[A]}{dt}=k\dots (2)$</p>
</li>
<li>
<p>$d[A]=-kdt\dots (3)$</p>
</li>
<li>
<p>$\int_{[A]_0}^{[A]_t} d[A]=-\int_0^t k d t \dots(4)$</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-07-chemical-kinetics-l-7_16-ja-sqowih90-06ab.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Units of rate constant $\rightarrow$ Example $\rightarrow$ Significance of rate and rate constant $\rightarrow$ Integrated rate laws $\rightarrow$ <span style="color:blue">Zero order reaction</span> $\rightarrow$ Half-life for a zero order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-7</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Zero order reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>$[A]_t=[A]_0-kt$</li>
</ul>
<ul>
<li>If plot of $[A]_t$ versus ’t’ is a straight line, then this is the signature of a zero order reaction</li>
</ul>
</div>
<div style='float: right; width:0%;'>


<img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/2c77a91c-fb6b-48ab-4976-ec6c04fbd000/public" style='width:70%'>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Units of rate constant $\rightarrow$ Example $\rightarrow$ Significance of rate and rate constant $\rightarrow$ Integrated rate laws $\rightarrow$ <span style="color:blue">Zero order reaction</span> $\rightarrow$ Half-life for a zero order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-7</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Half-life for a zero order reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$[A]<em>0$ $\hspace{2mm}$ $t</em>\frac{1}{2}$ $\rightarrow$ $\frac{1[A]_0}{2}$</p>
</li>
<li>
<p>$[A]_t=[A]_0 -kt \dots(5)$</p>
</li>
<li>
<p>$\frac{1}{2}[A]_0=[A]_0 -kt \dots(6)$</p>
</li>
<li>
<p>$kt_{1/2}=[A]_0-\frac{1}{2}[A]_0$</p>
</li>
<li>
<p>$kt_{1/2}=\frac{1}{2}[A]_0$</p>
</li>
<li>
<p>$t_{1/2}=\frac{[A]_0}{2k} \dots(7)$</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-07-chemical-kinetics-l-7_16-ja-sqowih90-632-2696.4.jpg"></p>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-07-chemical-kinetics-l-7_16-ja-sqowih90-661-2808.0.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Units of rate constant $\rightarrow$ Example $\rightarrow$ Significance of rate and rate constant $\rightarrow$ Integrated rate laws $\rightarrow$ Zero order reaction $\rightarrow$ <span style="color:blue">Half-life for a zero order reaction</span> </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-7</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Half-life for a zero order reaction</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>Half-life is proportional to the concentration of the reactant</p>
</li>
<li>
<p>Higher concentartion</p>
</li>
<li>
<p>Higher Half-life</p>
</li>
<li>
<p>As a reaction proceeds then the half-life also decreases</p>
</li>
<li>
<p>Half-life being used as a preliminary check</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-07-chemical-kinetics-l-7_16-ja-sqowih90-693-3003.6.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-07-chemical-kinetics-l-7_16-ja-sqowih90-661-2808.0.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Units of rate constant $\rightarrow$ Example $\rightarrow$ Significance of rate and rate constant $\rightarrow$ Integrated rate laws $\rightarrow$ Zero order reaction $\rightarrow$ <span style="color:blue">Half-life for a zero order reaction</span> </footer>