chemistry-class-12-unit-03-chapter-03-electro-chemistry-l-3-6-9oy6z-5nf-s

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemisrty Lecture 3</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Example of galvanic cell</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$Cu(s)+2Ag^+ (aq) \rightarrow Cu^{2+}(aq) + 2Ag(s)$</p>
</li>
<li>
<p>Cathode (RHE) reduction $2Ag^+(aq) + 2e \rightarrow 2Ag(s) \Rightarrow Ag^+(aq)/Ag(s)$</p>
</li>
<li>
<p>Anode (LHE) Oxidation $Cu(s) \rightarrow Cu^{2+}(aq)+2e \Rightarrow Cu/Cu^{2+}(aq)$</p>
</li>
<li>
<p>$Cu | Cu^{2+}(aq)$ | | $Ag^+ (aq) | Ag(s)$</p>
</li>
<li>
<p>$Cu | Cu^{2+}(aq) \rightarrow LHE \rightarrow Oxidation$</p>
</li>
<li>
<p>$Ag^+ (aq) | Ag(s) \rightarrow RHE \rightarrow Reduction$</p>
</li>
<li>
<p>$E_{cell} = \phi_R - \phi_L = \phi_{Ag^+/Ag} - \phi_{Cu^{2+}/Cu}$</p>
</li>
</ul>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-03-chapter-03-electro-chemistry-l-3_6-9oy6z_5nf_s-01.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Electrochemistry $\rightarrow$ <span style="color:blue">Example of galvanic cell</span> $\rightarrow$ Daniell cell $\rightarrow$ Representation of cell $\rightarrow$ Use of SHE to calculate half-cell potential $\rightarrow$ Example $\rightarrow$ Standard electrode potential at 298 k $\rightarrow$ Daniell cell </footer>

1bd

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemisrty Lecture 3</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Daniell cell</B></primary></p>
<hr>
<main>
<div style='float: left; width:70%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$Zn(S)|ZnSO_4(C=1)$ | |  $CuSO_4(C=1)|Cu$</p>
</li>
<li>
<p>Measurement of half-cell potential</p>
</li>
<li>
<p>Standard hydrogen electrode</p>
</li>
<li>
<p>$Pt(s) | H_2(g)(P=1bar)|H^+(aq,1M)$</p>
</li>
<li>
<p>$\phi = 0$ at all T</p>
</li>
</ul>
</div>
<div style='float: right; width:30%;'>
<img src ="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/79e5a1b4-5373-40bf-db48-0a8f5fb56600/public" style='width:100%;'>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Electrochemistry $\rightarrow$ Example of galvanic cell $\rightarrow$ <span style="color:blue">Daniell cell</span> $\rightarrow$ Representation of cell $\rightarrow$ Use of SHE to calculate half-cell potential $\rightarrow$ Example $\rightarrow$ Standard electrode potential at 298 k $\rightarrow$ Daniell cell </footer>

1bd

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemisrty Lecture 3</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Daniell cell</B></primary></p>
<hr>
<main>
<div style='float: left; width:70%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$H^+(aq) + e \rightarrow \frac{1}{2} H_2(g,1bar)$</p>
</li>
<li>
<p>$E = \phi_R - \phi_L$</p>
</li>
<li>
<p>$E=\phi_{Ag^+/Ag}-\phi_{Cu^{+2}/Cu}$</p>
</li>
<li>
<p>$E_{cell} = \phi_R - \phi_L = \phi_{Ag^+/Ag}-\phi_{Cu^{2+}/Cu}$</p>
</li>
</ul>
</div>
<div style='float: right; width:30%;'>
<img src ="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/79e5a1b4-5373-40bf-db48-0a8f5fb56600/public" style='width:100%;'>


</div>
</main>
<hr>
<footer style="font-size:18px;"> Electrochemistry $\rightarrow$ Example of galvanic cell $\rightarrow$ <span style="color:blue">Daniell cell</span> $\rightarrow$ Representation of cell $\rightarrow$ Use of SHE to calculate half-cell potential $\rightarrow$ Example $\rightarrow$ Standard electrode potential at 298 k $\rightarrow$ Daniell cell </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemisrty Lecture 3</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Representation of cell</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>SHE $\quad \quad $ ||  $\quad$ 2nd Half cell</p>
</li>
<li>
<p>$\quad \darr \quad \quad\quad \quad \quad \quad \darr$</p>
</li>
<li>
<p>Anode $\qquad \quad \quad$ Cathode</p>
</li>
<li>
<p>LHE $\qquad \quad \quad\quad$ RHE</p>
</li>
<li>
<p>$LHE \rightarrow H^+(aq) + e \rightarrow \frac{1}{2}H_2 (g,1bar)$</p>
</li>
<li>
<p>$RHE \rightarrow$ reduction potential of the RH half cell</p>
</li>
</ul>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Electrochemistry $\rightarrow$ Example of galvanic cell $\rightarrow$ Daniell cell $\rightarrow$ <span style="color:blue">Representation of cell</span> $\rightarrow$ Use of SHE to calculate half-cell potential $\rightarrow$ Example $\rightarrow$ Standard electrode potential at 298 k $\rightarrow$ Daniell cell </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemisrty Lecture 3</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Representation of cell</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>Concentration of the redox active substances/electrolyte in set at unity</p>
</li>
<li>
<p>Cell potential /Cell EMF = standard electrode potential or, standard reduction potential of the half cell</p>
</li>
<li>
<p>$E^{\phi} = \phi_R^{\phi} - \phi_L ^{\phi}$</p>
</li>
<li>
<p>$E^{\phi} = \phi_R ^{\phi}$</p>
</li>
<li>
<p>If ${\phi_L ^{\phi} }$ will be zero</p>
</li>
</ul>
</div>
<div style='float: right; width:00%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-03-chapter-03-electro-chemistry-l-3_6-9oy6z_5nf_s-03.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Electrochemistry $\rightarrow$ Example of galvanic cell $\rightarrow$ Daniell cell $\rightarrow$ <span style="color:blue">Representation of cell</span> $\rightarrow$ Use of SHE to calculate half-cell potential $\rightarrow$ Example $\rightarrow$ Standard electrode potential at 298 k $\rightarrow$ Daniell cell </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemisrty Lecture 3</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Use of SHE to calculate half-cell potential</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$E_{cell} ^{\phi} = \phi_R = 0.34V$</p>
</li>
<li>
<p>$Cu^{2+} (aq,1M) + 2e^- \rightarrow Cu^0 (S)$</p>
</li>
<li>
<p>$\Delta G^0=-nFE^0$</p>
</li>
<li>
<p>$\Delta G^0 < 0$</p>
</li>
</ul>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-03-chapter-03-electro-chemistry-l-3_6-9oy6z_5nf_s-04.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Electrochemistry $\rightarrow$ Example of galvanic cell $\rightarrow$ Daniell cell $\rightarrow$ Representation of cell $\rightarrow$ <span style="color:blue">Use of SHE to calculate half-cell potential</span> $\rightarrow$ Example $\rightarrow$ Standard electrode potential at 298 k $\rightarrow$ Daniell cell </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemisrty Lecture 3</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>$ Pt(S) |H_2(g, 1bar) (H^+ (aq, 1M) || Z^{2+} (aq, 1M) | Zn(s) \quad \quad \quad 298K $</p>
</li>
<li>
<p>$LHE \quad \quad \quad \quad \quad \quad \quad \quad RHE$</p>
</li>
<li>
<p><strong>Anode (Oxidation take place)</strong></p>
</li>
<li>
<p>$E^o=-0.76V$</p>
</li>
<li>
<p><strong>Cathod (Reduction)</strong></p>
</li>
<li>
<p>$Zn^{2+} + 2e \rarr Zn^0$</p>
</li>
<li>
<p>$\phi_{Zn^{2+} /Zn}=-0.76v$</p>
</li>
</ul>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Electrochemistry $\rightarrow$ Example of galvanic cell $\rightarrow$ Daniell cell $\rightarrow$ Representation of cell $\rightarrow$ Use of SHE to calculate half-cell potential $\rightarrow$ <span style="color:blue">Example</span> $\rightarrow$ Standard electrode potential at 298 k $\rightarrow$ Daniell cell </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemisrty Lecture 3</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>$\Delta G^0 = -nFE^0\Rightarrow 0$</p>
</li>
<li>
<p>$Zn(s)|(ZnSO_4 (C=1) || CuSO_4 (c=1) | Cu$</p>
</li>
<li>
<p>$-0.761 \qquad \qquad \qquad \qquad 0.34v$</p>
</li>
<li>
<p>$E_{cell} = \phi_{Cu^{2+}/Cu} - \phi_{Zn^{2+}/Zn}$</p>
</li>
<li>
<p>$=0.34 -(-0.76)V = 1.1V$</p>
</li>
</ul>
</div>
<div style='float: right; width:00%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-03-chapter-03-electro-chemistry-l-3_6-9oy6z_5nf_s-05.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Electrochemistry $\rightarrow$ Example of galvanic cell $\rightarrow$ Daniell cell $\rightarrow$ Representation of cell $\rightarrow$ Use of SHE to calculate half-cell potential $\rightarrow$ <span style="color:blue">Example</span> $\rightarrow$ Standard electrode potential at 298 k $\rightarrow$ Daniell cell </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemisrty Lecture 3</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>$Br_2$ - electrode : $Pt(S)|Br_2(aq)|Br^-(aq)$</p>
</li>
<li>
<p>$\frac {1}{2}Br_2(aq) +e \rarr Br^-(aq)$</p>
</li>
<li>
<p>$Ag(S) | Ag^+ (C =…)|$</p>
</li>
<li>
<p>$Fe^{3+} +e \rarr Fe^{2+}$</p>
</li>
<li>
<p>AgCl  $+e^{-} \rightarrow Ag^o+Cl^-$</p>
</li>
</ul>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-03-chapter-03-electro-chemistry-l-3_6-9oy6z_5nf_s-216.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Electrochemistry $\rightarrow$ Example of galvanic cell $\rightarrow$ Daniell cell $\rightarrow$ Representation of cell $\rightarrow$ Use of SHE to calculate half-cell potential $\rightarrow$ <span style="color:blue">Example</span> $\rightarrow$ Standard electrode potential at 298 k $\rightarrow$ Daniell cell </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemisrty Lecture 3</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>$Ag|AgCl(S),Cl^-$</p>
</li>
<li>
<p>$C=1 \quad \Delta G -nFE$</p>
</li>
<li>
<p>NERNST Equation</p>
</li>
<li>
<p>$\phi_{M^{n+}/M} = \phi_\frac {M^{n+}}{M}$ - $\frac {RT}{nF}ln \frac{[M]}{[M^{n+}]} $</p>
</li>
<li>
<p>$M^{n+} + ne^{-} \rarr M$</p>
</li>
<li>
<p>$F = \sim 96500$ C/mole & $R = 8.314 jK^{-1}mole^{-1}$</p>
</li>
<li>
<p>$\phi_{M^{n+}/M} = \phi_{M^{n+}/M}^o - \frac{RT}{nF}ln \frac{1}{[M^{n+}]}$</p>
</li>
</ul>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-03-chapter-03-electro-chemistry-l-3_6-9oy6z_5nf_s-258-2655.6.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Electrochemistry $\rightarrow$ Example of galvanic cell $\rightarrow$ Daniell cell $\rightarrow$ Representation of cell $\rightarrow$ Use of SHE to calculate half-cell potential $\rightarrow$ <span style="color:blue">Example</span> $\rightarrow$ Standard electrode potential at 298 k $\rightarrow$ Daniell cell </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemisrty Lecture 3</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Daniell cell</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p><strong>Cathode RHE Reduction</strong></p>
</li>
<li>
<p>$\phi_{Cu^{2+}/Cu} = \phi^0_{Cu^{2+}/{Cu}} - \frac {RT}{2F} ln \frac {1}{[Cu^{2+}aq]}$</p>
</li>
<li>
<p><strong>Anode LHE Oxidation</strong></p>
</li>
<li>
<p>$\phi_{Zn^{2+} /{Zn} } =\phi_{Zn^{2+} /{Zn}}- \frac {RT}{2F}ln \frac {1}{Zn^{2+}aq}$</p>
</li>
<li>
<p>$=\phi_{Cu^{2+} /{Cu}} - \phi_{Zn^{2+} /{Zn}}$</p>
</li>
</ul>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Electrochemistry $\rightarrow$ Example of galvanic cell $\rightarrow$ Daniell cell $\rightarrow$ Representation of cell $\rightarrow$ Use of SHE to calculate half-cell potential $\rightarrow$ Example $\rightarrow$ Standard electrode potential at 298 k $\rightarrow$ <span style="color:blue">Daniell cell</span> </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemisrty Lecture 3</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Daniell cell</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$E_{cell}$ = $\phi_R-\phi_L$ (IUPAC, Reduction pot)</p>
</li>
<li>
<p>$ = \phi_{Cu^{2+} /Cu} -\phi_{Zn^{2+} /{Zn}}$</p>
</li>
<li>
<p>$ = \phi_{Cu^{2+} /Cu} ^0 -\phi_{Zn^{2+} /{Zn}} ^0 -\frac {RT}{2f}ln \frac{1}{Zn^{2+} (aq)} + \frac{RT}{2F} ln \frac{1} {Zn^{2+} (aq)}$</p>
</li>
</ul>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-03-chapter-03-electro-chemistry-l-3_6-9oy6z_5nf_s-07.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Electrochemistry $\rightarrow$ Example of galvanic cell $\rightarrow$ Daniell cell $\rightarrow$ Representation of cell $\rightarrow$ Use of SHE to calculate half-cell potential $\rightarrow$ Example $\rightarrow$ Standard electrode potential at 298 k $\rightarrow$ <span style="color:blue">Daniell cell</span> </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemisrty Lecture 3</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Daniell cell</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$E_{cell}= E^0_{cell} - \frac {RT}{2F}ln \frac {[Zn^{2+}(aq)]}{[Cu^{2+}(aq)]}$</p>
</li>
<li>
<p>$Zn + CuSO_4\rarr ZnSO_4 + Cu$</p>
</li>
<li>
<p>R,F,T = 298K</p>
</li>
<li>
<p>$E_{cell}=E^o_{cell}-\frac{0.059}{2} log \frac{[Zn^{2+}(aq)]}{[Cu^{2+}(aq)]}$</p>
</li>
</ul>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-03-chapter-03-electro-chemistry-l-3_6-9oy6z_5nf_s-08.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Electrochemistry $\rightarrow$ Example of galvanic cell $\rightarrow$ Daniell cell $\rightarrow$ Representation of cell $\rightarrow$ Use of SHE to calculate half-cell potential $\rightarrow$ Example $\rightarrow$ Standard electrode potential at 298 k $\rightarrow$ <span style="color:blue">Daniell cell</span> </footer>