<p><Success style= "margin-top:16rem;text-align:center;"><B>Chemical kinetics<br>Lecture-8</B></Success></p>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-8</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>$A \rightarrow P$</p> </li> <li> <p>${ rate } = k[A]^0 = k $—(1)</p> </li> <li> <p>$-\frac{d[A]}{d t} = k$—(2)</p> </li> <li> <p>$d[A] = - kdt $ —(3)</p> </li> <li> <p>$\int_{[A]_0}^{[A]_t} d[A]=-\int_0^t k d t \cdots \text { (4) }$</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-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-020-0096.0.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> <span style="color:blue">Zero order reaction</span> $\rightarrow$ Half-life for a zero order reaction $\rightarrow$ First order reaction $\rightarrow$ Half-life for first order reaction $\rightarrow$ Example of first order reaction $\rightarrow$ First order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-8</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:60%;font-size:22px;text-align:left'> <ul> <li> <p>$k$ is a constant and can be kept out side the integral</p> </li> <li> <p>$[A]_t - [A]_0 = - k(t-0)$</p> </li> <li> <p>${[A]_t-[A]_0=-k t} \ $</p> </li> <li> <p>${[A]_t=[A]_0-k t} $—(5)</p> </li> <li> <p>$y=m x+c$</p> </li> <li> <p>If plot of $[A]_t$ versus ’ $t$ ’ is a straight line, then this is the signature of a zero order reaction</p> </li> </ul> </div> <div style='float: right; width:40%;'> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/a1baaa19-7774-49be-dfdb-75a52bdeee00/public" style='width:60%'> </div> </main> <hr> <footer style="font-size:18px;"> <span style="color:blue">Zero order reaction</span> $\rightarrow$ Half-life for a zero order reaction $\rightarrow$ First order reaction $\rightarrow$ Half-life for first order reaction $\rightarrow$ Example of first order reaction $\rightarrow$ First order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-8</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>$[A]<em>0$, $\hspace{2mm}$ $t</em>\frac{1}{2}$ $\rightarrow$ $\frac{1}{2}[A]_0$</p> </li> <li> <p>$[A]_t = [A]_0 - kt \dots (5)$</p> </li> <li> <p>$\frac{1}{2}[A]_t = [A]<em>0 - kt</em>\frac{1}{2} \dots (6)$</p> </li> <li> <p>$kt_{1 / 2} =[A]_0-\frac{1}{2}[A]_0$</p> </li> </ul> </div> <div style='float: right; width:0%;'> <!----> <!----> <!----> <!----> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/a1baaa19-7774-49be-dfdb-75a52bdeee00/public" style='width:70%'> </div> </main> <hr> <footer style="font-size:18px;"> Zero order reaction $\rightarrow$ <span style="color:blue">Half-life for a zero order reaction</span> $\rightarrow$ First order reaction $\rightarrow$ Half-life for first order reaction $\rightarrow$ Example of first order reaction $\rightarrow$ First order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-8</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>$ k t_{1 / 2} =\frac{1}{2}[A]_0 $</p> </li> <li> <p>$t_{1 / 2} =\frac{[A]_0}{2 k} $—(7)</p> </li> <li> <p>Half-life is proportional to the concentration of the reactant</p> </li> <li> <p>Higher concentration</p> </li> <li> <p>Higher, half life</p> </li> </ul> </div> </main> <hr> <footer style="font-size:18px;"> Zero order reaction $\rightarrow$ <span style="color:blue">Half-life for a zero order reaction</span> $\rightarrow$ First order reaction $\rightarrow$ Half-life for first order reaction $\rightarrow$ Example of first order reaction $\rightarrow$ First order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-8</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>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-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-068-0258.0.jpg"> <img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-070-0277.2.jpg"> <img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-073-0301.2.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Zero order reaction $\rightarrow$ <span style="color:blue">Half-life for a zero order reaction</span> $\rightarrow$ First order reaction $\rightarrow$ Half-life for first order reaction $\rightarrow$ Example of first order reaction $\rightarrow$ First order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-8</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>First order reaction</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>$A \rightarrow P $</p> </li> <li> <p>${ rate } = k[A]…(8) $</p> </li> <li> <p>$-\frac{d[A]}{d t}=k[A] \cdots(9)$</p> </li> <li> <p>$\therefore-\frac{d[A]}{[A]} =k d t$</p> </li> <li> <p>$\int_{[A]_0}^{[A_t]}\frac{d[A]}{[A]}$ =-k $\int_0^t d t$</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-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-01.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Zero order reaction $\rightarrow$ Half-life for a zero order reaction $\rightarrow$ <span style="color:blue">First order reaction</span> $\rightarrow$ Half-life for first order reaction $\rightarrow$ Example of first order reaction $\rightarrow$ First order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-8</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>First order reaction</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>$\ln [A]_t-\ln [A]_0=-k t$….(10)</p> </li> <li> <p>$\ln [A]_t=\ln [A]_0-k t$…. (11)</p> </li> <li> <p>$\ln \frac{[A]_t}{[A]_0}$ = -k t…. (12)</p> </li> <li> <p>$\frac{[A]_t}{[A]_0}$ =$e^{-k t}$….(13)</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-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-154-0580.8.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Zero order reaction $\rightarrow$ Half-life for a zero order reaction $\rightarrow$ <span style="color:blue">First order reaction</span> $\rightarrow$ Half-life for first order reaction $\rightarrow$ Example of first order reaction $\rightarrow$ First order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-8</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>First order reaction</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>$[A]_t=[A]_0 e^{-k t}\ $ ,</p> </li> <li> <p>$[A]_t=[A]_0 \exp (-k t)$…(14)</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-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-194-0733.2.jpg"> <img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-154-0580.8.jpg"> <img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-073-0301.2.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Zero order reaction $\rightarrow$ Half-life for a zero order reaction $\rightarrow$ <span style="color:blue">First order reaction</span> $\rightarrow$ Half-life for first order reaction $\rightarrow$ Example of first order reaction $\rightarrow$ First order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-8</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>First order reaction</B></primary></p> <hr> <main> <div style='float: left; width:60%;font-size:22px;text-align:left'> <ul> <li> <p>$\ln [A]_t=ln [A]_0-k t \cdots(11)$</p> </li> <li> <p>If the experimental data fit first order kinetics, then the plot of $\ ln [A]_t$ versus time will be a straight line that is linear</p> </li> </ul> </div> <div style='float: right; width:40%;'> <!----> <!----> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/7f060bcb-d93d-4b63-4b3f-6b31dc65a700/public" style='width:70%'> </div> </main> <hr> <footer style="font-size:18px;"> Zero order reaction $\rightarrow$ Half-life for a zero order reaction $\rightarrow$ <span style="color:blue">First order reaction</span> $\rightarrow$ Half-life for first order reaction $\rightarrow$ Example of first order reaction $\rightarrow$ First order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-8</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Half-life for first order reaction</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>$t_\frac{1}{2}$ $\Rightarrow$ $\frac{1}{2}[A]_0$</p> </li> <li> <p>$\ln \frac{[A]_t}{[A]_0}=-k t$…(12)</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-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-281-1117.2.jpg"> <img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-154-0580.8.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Zero order reaction $\rightarrow$ Half-life for a zero order reaction $\rightarrow$ First order reaction $\rightarrow$ <span style="color:blue">Half-life for first order reaction</span> $\rightarrow$ Example of first order reaction $\rightarrow$ First order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-8</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Half-life for first order reaction</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>At $\quad t_{1 / 2} \quad \ln \frac{[A_{t\frac {1}{2}}]}{[A_0]}$=$-k t_{1 / 2}$ …..(15)</p> </li> <li> <p>$\ln\frac{\frac{1}{2}[A]_0}{[A]_0} = -kt\frac{1}{2 }$</p> </li> <li> <p>$\ln \frac{1}{2}$ = $-k t_{1 / 2}$ …. (16)</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-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-307-1222.8.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Zero order reaction $\rightarrow$ Half-life for a zero order reaction $\rightarrow$ First order reaction $\rightarrow$ <span style="color:blue">Half-life for first order reaction</span> $\rightarrow$ Example of first order reaction $\rightarrow$ First order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-8</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Half-life for first order reaction</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>$t_{1 / 2}=\frac{\ln 2}{k} $…..(17)</p> </li> <li> <p>$ t_{1 / 2}=\frac{0.693}{k}$…..(18)</p> </li> <li> <p>The half-life for a first order reaction is independent of the concentration of the reactant</p> </li> <li> <p>$t_{1 / 2}$ takes the same value no matter what the extent of reaction is</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-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-02.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Zero order reaction $\rightarrow$ Half-life for a zero order reaction $\rightarrow$ First order reaction $\rightarrow$ <span style="color:blue">Half-life for first order reaction</span> $\rightarrow$ Example of first order reaction $\rightarrow$ First order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-8</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Example of first order reaction</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>$2N_2 O_5(g)\rightarrow 4NO_2(g)+\mathrm{O}_2(\mathrm{g})$</p> </li> <li> <p>$ rate = k[\mathrm{N}_2{O}_5]$</p> </li> <li> <p>$\mathrm { rate } = -\frac{1}{2} \frac {{d}[\mathrm{N}_2 \mathrm{O}_5]}{ d t}$</p> </li> <li> <p>$= - \frac{1}{2} \frac {{d}[\mathrm{N}_2 \mathrm{O}_5]}{ d t}$</p> </li> <li> <p>$-\frac{1}{2} \frac{d\left[\mathrm{N}_2 \mathrm{O}_5\right]}{d t}=k\left[\mathrm{N}_2{O}_5\right]$——-(19)</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-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-391-1665.6.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Zero order reaction $\rightarrow$ Half-life for a zero order reaction $\rightarrow$ First order reaction $\rightarrow$ Half-life for first order reaction $\rightarrow$ <span style="color:blue">Example of first order reaction</span> $\rightarrow$ First order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-8</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Example of first order reaction</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <!--$\ln \left[\mathrm{N}_2 \mathrm{O}_5\right]_t-\ln \left[\mathrm{N}_2 \mathrm{O}_5\right]_0=-2$kt--> <ul> <li> <p>$ {\int_{[N_2 O_5]}^{[N_2 O_5]} \frac {d[N_2 O_5]}{[N_2 O_5]}} $</p> </li> <li> <p>$=-\int_{t=0}^t 2 k d t$</p> </li> <li> <p>$\ln \left[\mathrm{N}_2 \mathrm{O}_5\right]_t-\ln \left[\mathrm{N}_2 \mathrm{O}_5\right]_0=-2 R t$</p> </li> <li> <p>$\ln \left[\mathrm{N}_2 \mathrm{O}_5\right]_t=\ln \left[\mathrm{N}_2 \mathrm{O}_5\right]_0-2 k t\ldots (20)$</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-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-436-1881.6.jpg"> <img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-154-0580.8.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Zero order reaction $\rightarrow$ Half-life for a zero order reaction $\rightarrow$ First order reaction $\rightarrow$ Half-life for first order reaction $\rightarrow$ <span style="color:blue">Example of first order reaction</span> $\rightarrow$ First order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-8</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>Example of first order reaction</B></primary></p> <hr> <main> <div style='float: left; width:100%;'> <!--Intercept $=\ln \left[\mathrm{N}_2 \mathrm{O}_5\right]_0$--> <!--slope $=-2 k$--> <!--$k=\frac{\text { slope }}{-2}$--> <!--$\ 2 \mathrm{N}_2 \mathrm{O}_5(\mathrm{g})\rightarrow 4 \mathrm{NO}_2(\mathrm{g}]+\mathrm{O}_2(\mathrm{g}] \$--> <!--$rate =k\[\mathrm{N}_2 \mathrm{O}_5]\ $--> <!--$rate =-\frac{1}{2}\frac{d\left[\mathrm{N}_2 \mathrm{O}_5\right)}{dt} \$--> <!--$=-\frac{1}{2}\frac{d\left[\mathrm{N}_2 \mathrm{O}_5\right)}{dt} \$--> <!----> <!----> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/12c8eca4-8bf6-443d-928f-d79ca4ecd300/public" style='width:40%'> </div> </main> <hr> <footer style="font-size:18px;"> Zero order reaction $\rightarrow$ Half-life for a zero order reaction $\rightarrow$ First order reaction $\rightarrow$ Half-life for first order reaction $\rightarrow$ <span style="color:blue">Example of first order reaction</span> $\rightarrow$ First order reaction </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-8</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>First order reaction</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p><strong>To generalise-</strong></p> </li> <li> <p>$ 2 A \rightarrow P$</p> </li> <li> <p>$a A \rightarrow P$</p> </li> <li> <p>$\text { rate }=-\frac{1}{a} \frac{d[A]}{d t}=k[A]$</p> </li> <li> <p>$\ln [A]_{t}=\ln [A]_0-a k t$ …(21)</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-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-03.jpg"> <img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-551.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Zero order reaction $\rightarrow$ Half-life for a zero order reaction $\rightarrow$ First order reaction $\rightarrow$ Half-life for first order reaction $\rightarrow$ Example of first order reaction $\rightarrow$ <span style="color:blue">First order reaction</span> </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-8</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>First order reaction</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p><strong>Relaxation time $(\tau)$ $\rightarrow tau$</strong></p> </li> <li> <p>$[A]_0 \rightarrow \frac{1}{e}[A]_0$</p> </li> <li> <p>Relaxation time</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-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-526-2263.2.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Zero order reaction $\rightarrow$ Half-life for a zero order reaction $\rightarrow$ First order reaction $\rightarrow$ Half-life for first order reaction $\rightarrow$ Example of first order reaction $\rightarrow$ <span style="color:blue">First order reaction</span> </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-8</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>First order reaction</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>${[A]_{t=\tau}=0.368[A]_0}$</p> </li> <li> <p>${[A]_{t=\tau}=0.368[A]_0}$</p> </li> <li> <p>at $t=\tau$ (relaxation time)</p> </li> <li> <p>Reaction has gone to 63.2%</p> </li> <li> <p>Completion and still has 36.8% to go</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-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-04.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Zero order reaction $\rightarrow$ Half-life for a zero order reaction $\rightarrow$ First order reaction $\rightarrow$ Half-life for first order reaction $\rightarrow$ Example of first order reaction $\rightarrow$ <span style="color:blue">First order reaction</span> </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-8</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>First order reaction</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>${[A]_t } =[A]_0 e^{-k t} \cdots \text { (14) }$</p> </li> <li> <p>$t=\tau$ $\quad \frac{1}{e}[A]_0 =[A]_0 e^{-k t}$</p> </li> <li> <p>$\frac{1}{e} = e^{-k t}$</p> </li> <li> <p>$e^{-1} = e^{-k t}$</p> </li> <li> <p>$e^{-1} = e^{-k \tau}$…22</p> </li> <li> <p>$e^{1}$ = $e^{(k\tau)}$</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-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-624-2635.2.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Zero order reaction $\rightarrow$ Half-life for a zero order reaction $\rightarrow$ First order reaction $\rightarrow$ Half-life for first order reaction $\rightarrow$ Example of first order reaction $\rightarrow$ <span style="color:blue">First order reaction</span> </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-8</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>First order reaction</B></primary></p> <hr> <main> <div style='float: left; width:100%;font-size:22px;text-align:left'> <ul> <li> <p>ln e = k $\tau$</p> </li> <li> <p>k $\tau$ = 1</p> </li> <li> <p>$\tau$ = $\frac{1}{k} \quad \ldots(23)$</p> </li> <li> <p>Relaxation times are only applicable for first order or pseudo first order 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-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-624-2635.2.jpg"> <img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-04-chapter-08-chemical-kinetics-l-8_16-cwg_y3w_b_k-618-2620.8.jpg"></p> </div> </main> <hr> <footer style="font-size:18px;"> Zero order reaction $\rightarrow$ Half-life for a zero order reaction $\rightarrow$ First order reaction $\rightarrow$ Half-life for first order reaction $\rightarrow$ Example of first order reaction $\rightarrow$ <span style="color:blue">First order reaction</span> </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Chemical kinetics Lecture-8</B></Success></p> <p><primary style="float:center;text-align:center;font-size:24px;"> <B>First order reaction</B></primary></p> <hr> <main> <div style='float: left; width:60%;font-size:22px;text-align:left'> <ul> <li> <p>${[A]_t=[A]_0 e^{-k t}}$</p> </li> <li> <p>$t_{1 / 2}=\frac{0.693}{k}$</p> </li> </ul> <!--$\{[A]_t } =[A]_0 e^{-k t} \cdots \text { (14) }\$--> <!--$t=\tau$ $\quad \frac{1}{e}[A]_0 =[A]_0 e^{-k t}\$--> <!--$\frac{1}{e} = e^{-k t}$--> <!--$e^{-1} = e^{-k t}$--> <!--$e^{-1} = e^{-k t}\$....22--> </div> <div style='float: right; width:40%;'> <!----> <!----> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/81f4019b-e193-4e58-1b9c-3ee8a443c300/public" style='width:80%'> </div> </main> <hr> <footer style="font-size:18px;"> Zero order reaction $\rightarrow$ Half-life for a zero order reaction $\rightarrow$ First order reaction $\rightarrow$ Half-life for first order reaction $\rightarrow$ Example of first order reaction $\rightarrow$ <span style="color:blue">First order reaction</span> </footer>

<p><Success style= "margin-top:16rem;text-align:center;"><B>Thank you</B></Success></p>