chemistry-class-12-unit-03-chapter-05-electro-chemistry-l-5-6-yhyukobqg-i

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemistry Lecture-5</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Gibb’s free energy</B></primary></p>
<hr>
<main>
<div style='float: left; width:70%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$\Delta G_{rxn}=w_{el}=-Q\Delta E$</p>
</li>
<li>
<p>$=-nF\Delta E$</p>
</li>
<li>
<p>$Zn+CuSO_4 \rarr ZnSO_4 + Cu \darr$</p>
</li>
<li>
<p>$\Delta G < 0$</p>
</li>
<li>
<p>Electrolysis will take place</p>
</li>
</ul>
</div>
<div style='float: right; width:30%;'>
<img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/ab74f200-1e13-4092-8f16-4912845ed900/public" style='width:100%;'>

</div>
</main>
<hr>
<footer style="font-size:18px;"> <span style="color:blue">Gibb's free energy</span> $\rightarrow$ Electrolytic cell $\rightarrow$ Electrolysis $\rightarrow$ Electrolysis of pure-high resistance $\rightarrow$ Faraday's law $\rightarrow$ Electrolysis of brine solution $\rightarrow$ Types of cell $\rightarrow$ Lead-acid storage cell (1859) $\rightarrow$ Problems $\rightarrow$ Dry cell $\rightarrow$ Modern version of primary storage (1949) </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemistry Lecture-5</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Electrolytic cell</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p><strong>Galvanic cell</strong>:- Electrons are generated at the anode (-)</p>
</li>
<li>
<p><strong>Electrolytic cell</strong>:- Cathode (-) Anode (+)</p>
</li>
</ul>
<p>Electrolysis of molten alkali halides (NaCl(Na-metal))</p>
<p>Carbon electrodes</p>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-03-chapter-05-electro-chemistry-l-5_6-yhyukobqg-i-02.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Gibb's free energy $\rightarrow$ <span style="color:blue">Electrolytic cell</span> $\rightarrow$ Electrolysis $\rightarrow$ Electrolysis of pure-high resistance $\rightarrow$ Faraday's law $\rightarrow$ Electrolysis of brine solution $\rightarrow$ Types of cell $\rightarrow$ Lead-acid storage cell (1859) $\rightarrow$ Problems $\rightarrow$ Dry cell $\rightarrow$ Modern version of primary storage (1949) </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemistry Lecture-5</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Electrolytic cell</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li><strong>Reaction of electrolytic Cell</strong></li>
</ul>
<p>Cathod reaction : $Na^+ + e^-\rarr Na(s) \hspace{3 mm} E\degree= -2.71$V</p>
<p>Anode reaction : $Cl^- \rarr \frac{1}{2} Cl_2(g)+e^- \hspace{3 mm} E\degree=-1.36$V</p>
<p><strong>Overall reaction</strong> : $Na^+ + Cl^- \rarr Na(s)+\frac{1}{2}Cl_2(g) \hspace{3 mm} E\degree=-4.1$V</p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Gibb's free energy $\rightarrow$ <span style="color:blue">Electrolytic cell</span> $\rightarrow$ Electrolysis $\rightarrow$ Electrolysis of pure-high resistance $\rightarrow$ Faraday's law $\rightarrow$ Electrolysis of brine solution $\rightarrow$ Types of cell $\rightarrow$ Lead-acid storage cell (1859) $\rightarrow$ Problems $\rightarrow$ Dry cell $\rightarrow$ Modern version of primary storage (1949) </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemistry Lecture-5</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Electrolysis</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li><strong>Ag Solution of $NiCl_2$ : Pt electrodes</strong></li>
</ul>
<p>Cathode reaction : $Ni^{2+}+2e^-\rarr Ni(s) \hspace{3 mm} E\degree=-0.24$V</p>
<p>Anode reaction : $2Cl^- \rarr Cl_2(g)+2e^- \hspace{3 mm} -1.36$V</p>
<p>$Ni^{2+}+2Cl^- \rarr 2Ni(g)+Cl_2(g) \hspace{3 mm} E\degree_{net}=-1.6$V</p>
<ul>
<li><strong>Electrolysis of water:</strong></li>
</ul>
<p>Anode reaction : $H_2O\rarr \frac{1}{2}O_2(g)+2H^+ +2e^- \hspace{3 mm} E\degree=-1.23$V</p>
<p>Cathode reaction : $2H_2O +2e^- \rarr H_2(g)+2OH^- \hspace{3 mm} E\degree=-0.83$V</p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Gibb's free energy $\rightarrow$ Electrolytic cell $\rightarrow$ <span style="color:blue">Electrolysis</span> $\rightarrow$ Electrolysis of pure-high resistance $\rightarrow$ Faraday's law $\rightarrow$ Electrolysis of brine solution $\rightarrow$ Types of cell $\rightarrow$ Lead-acid storage cell (1859) $\rightarrow$ Problems $\rightarrow$ Dry cell $\rightarrow$ Modern version of primary storage (1949) </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemistry Lecture-5</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Electrolysis</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li><strong>Ag solution of NaCl</strong></li>
</ul>
<p><strong>Cathode reaction:</strong></p>
<p>$2H_2O +2e^- \rarr H_2(g)+2OH^- \hspace{3 mm} E\degree=0.4$ V $[O^-H]\sim 10^{-7}M$</p>
<p><strong>Anode reaction:</strong></p>
<p>$Cl^- +H_2O \rarr \frac{1}{2}Cl_2 + e^- \hspace{3 mm} E\degree=-0.95$V</p>
<p>$Cl^- +H_2O \rarr 2H_2(g)+\frac{1}{2}Cl_2 + 2OH^- \rarr E=-0.95$V</p>
<p>$Na^+ +e^- \rarr Na(s) \quad E \degree = -2.7$V</p>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-03-chapter-05-electro-chemistry-l-5_6-yhyukobqg-i-03.jpg">
<img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-03-chapter-05-electro-chemistry-l-5_6-yhyukobqg-i-3.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Gibb's free energy $\rightarrow$ Electrolytic cell $\rightarrow$ <span style="color:blue">Electrolysis</span> $\rightarrow$ Electrolysis of pure-high resistance $\rightarrow$ Faraday's law $\rightarrow$ Electrolysis of brine solution $\rightarrow$ Types of cell $\rightarrow$ Lead-acid storage cell (1859) $\rightarrow$ Problems $\rightarrow$ Dry cell $\rightarrow$ Modern version of primary storage (1949) </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemistry Lecture-5</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Electrolysis of pure-high resistance</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li><strong>Difficult to undergo electrolysis $\rarr$ little bit of acid</strong></li>
</ul>
<p><strong>Cathode reaction:</strong></p>
<p>$2H_2O+2e^-\rarr H_2(g)+2OH^- \hspace{3 mm} E\degree=-0.83$V</p>
<p><strong>Anode reaction:</strong></p>
<p>$H_2O \rarr \frac{1}{2}O_2(g)+2H^+ +2e^- \hspace{3 mm} E\degree=-1.29$V</p>
<p>$3H_2O(l)\rarr H_2+\frac{1}{2}O_2+……E\degree=-2.06$V</p>
<p><strong>Faraday’s Law of electolysis (Michael Faraday) in 1832.</strong></p>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-03-chapter-05-electro-chemistry-l-5_6-yhyukobqg-i-04.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Gibb's free energy $\rightarrow$ Electrolytic cell $\rightarrow$ Electrolysis $\rightarrow$ <span style="color:blue">Electrolysis of pure-high resistance</span> $\rightarrow$ Faraday's law $\rightarrow$ Electrolysis of brine solution $\rightarrow$ Types of cell $\rightarrow$ Lead-acid storage cell (1859) $\rightarrow$ Problems $\rightarrow$ Dry cell $\rightarrow$ Modern version of primary storage (1949) </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemistry Lecture-5</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Faraday’s law</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ol>
<li>Weight of substance formed at the electrode during electrolysis in directly proportional to the quantity of electricity that passes through the electrolyte.</li>
</ol>
<ul>
<li>$m \propto Q \rarr $It</li>
<li>$\rarr m=ZQ$</li>
<li>$Z \rarr$ Electrochemial  equivalent.</li>
</ul>
<ol start="2">
<li>The weight of different substances formed by the passage of same quantity of electricity are proportional to the equivalent weight of each substance.</li>
</ol>
<ul>
<li>$\frac{W_1}{W_2}=\frac{m_1}{m_2}=\frac{E_1}{E_2}$</li>
<li>$\frac{Z_1 It}{Z_2 It}=\frac{E_1}{E_2}\rArr \frac{Z_1}{Z_2}=\frac{E_1}{E_2}$</li>
</ul>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-03-chapter-05-electro-chemistry-l-5_6-yhyukobqg-i-05.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Gibb's free energy $\rightarrow$ Electrolytic cell $\rightarrow$ Electrolysis $\rightarrow$ Electrolysis of pure-high resistance $\rightarrow$ <span style="color:blue">Faraday's law</span> $\rightarrow$ Electrolysis of brine solution $\rightarrow$ Types of cell $\rightarrow$ Lead-acid storage cell (1859) $\rightarrow$ Problems $\rightarrow$ Dry cell $\rightarrow$ Modern version of primary storage (1949) </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemistry Lecture-5</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Electrolysis of brine solution</B></primary></p>
<hr>
<main>
<div style='float: left; width:50%;font-size:22px;text-align:left'>
<img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/3b1abae9-930b-4347-9e87-b49b5cc55900/public" style='width:80%;'>
</div>
<div style='float: right; width:50%;'>
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</div>
</main>
<hr>
<footer style="font-size:18px;"> Gibb's free energy $\rightarrow$ Electrolytic cell $\rightarrow$ Electrolysis $\rightarrow$ Electrolysis of pure-high resistance $\rightarrow$ Faraday's law $\rightarrow$ <span style="color:blue">Electrolysis of brine solution</span> $\rightarrow$ Types of cell $\rightarrow$ Lead-acid storage cell (1859) $\rightarrow$ Problems $\rightarrow$ Dry cell $\rightarrow$ Modern version of primary storage (1949) </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemistry Lecture-5</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Types of cell</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li><strong>Primary storage cell</strong></li>
</ul>
<ul>
<li>
<p>Ordinary flashlight battery/all.</p>
</li>
<li>
<p>Cannot be recharged the amount of el. en</p>
</li>
</ul>
<ul>
<li><strong>Secondary storage cell</strong></li>
</ul>
<ul>
<li>
<p>Capable of being recharged</p>
</li>
<li>
<p>Electrical work done on the all provide the free energy to focus the reaction in the reverse direction</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-05-electro-chemistry-l-5_6-yhyukobqg-i-124-1992.0.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Gibb's free energy $\rightarrow$ Electrolytic cell $\rightarrow$ Electrolysis $\rightarrow$ Electrolysis of pure-high resistance $\rightarrow$ Faraday's law $\rightarrow$ Electrolysis of brine solution $\rightarrow$ <span style="color:blue">Types of cell</span> $\rightarrow$ Lead-acid storage cell (1859) $\rightarrow$ Problems $\rightarrow$ Dry cell $\rightarrow$ Modern version of primary storage (1949) </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemistry Lecture-5</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Lead-acid storage cell (1859)</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>$P_{H_2SO_4} \sim 2P_{H_2O}$</p>
</li>
<li>
<p>$[H_2SO_4]=6mol/dm^3$</p>
</li>
<li>
<p>Normal cell voltage ~ 2.1v at 298K</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-05-electro-chemistry-l-5_6-yhyukobqg-i-07.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Gibb's free energy $\rightarrow$ Electrolytic cell $\rightarrow$ Electrolysis $\rightarrow$ Electrolysis of pure-high resistance $\rightarrow$ Faraday's law $\rightarrow$ Electrolysis of brine solution $\rightarrow$ Types of cell $\rightarrow$ <span style="color:blue">Lead-acid storage cell (1859)</span> $\rightarrow$ Problems $\rightarrow$ Dry cell $\rightarrow$ Modern version of primary storage (1949) </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemistry Lecture-5</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Problems</B></primary></p>
<hr>
<main>
<div style='float: left; width:60%;font-size:22px;text-align:left'>
<ul>
<li>
<p>Weight</p>
</li>
<li>
<p>Viscosity $H_2SO_4$ $\uarr$ during winter$\rarr $Reduces current</p>
</li>
<li>
<p>Slowly it may discharge.</p>
</li>
<li>
<p>Fast charging, $H_2$</p>
</li>
</ul>
</div>
<div style='float: right; width:40%;'>
<img src ="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/d8056668-c37e-45a6-547c-da2b15857300/public" style ='width:100%;'>

</div>
</main>
<hr>
<footer style="font-size:18px;"> Gibb's free energy $\rightarrow$ Electrolytic cell $\rightarrow$ Electrolysis $\rightarrow$ Electrolysis of pure-high resistance $\rightarrow$ Faraday's law $\rightarrow$ Electrolysis of brine solution $\rightarrow$ Types of cell $\rightarrow$ Lead-acid storage cell (1859) $\rightarrow$ <span style="color:blue">Problems</span> $\rightarrow$ Dry cell $\rightarrow$ Modern version of primary storage (1949) </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemistry Lecture-5</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Dry cell</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li><strong>Le clanche’ dry cell 1866</strong></li>
</ul>
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</div>
<div style='float: right; width:1%;'>

</div>
</main>
<hr>
<footer style="font-size:18px;"> Gibb's free energy $\rightarrow$ Electrolytic cell $\rightarrow$ Electrolysis $\rightarrow$ Electrolysis of pure-high resistance $\rightarrow$ Faraday's law $\rightarrow$ Electrolysis of brine solution $\rightarrow$ Types of cell $\rightarrow$ Lead-acid storage cell (1859) $\rightarrow$ Problems $\rightarrow$ <span style="color:blue">Dry cell</span> $\rightarrow$ Modern version of primary storage (1949) </footer>

<p><Success style="float:center;text-align:center;font-size:28px;"> <B>Electrochemistry Lecture-5</B></Success></p>
<p><primary style="float:center;text-align:center;font-size:24px;"> <B>Modern version of primary storage (1949)</B></primary></p>
<hr>
<main>
<div style='float: left; width:100%;font-size:22px;text-align:left'>
<ul>
<li>
<p>KOH has been used in place of $NH_4Cl$ corrosive to Zn metal</p>
</li>
<li>
<p>KOH & Zn-powder $\rArr$ Gets higher current rating</p>
</li>
</ul>
<p>Voltage 1.5-1.65</p>
<p><strong>Net reaction:</strong></p>
<p>$Zn+2MnO_2\rarr ZnO+Mn_2O_3$</p>
<p><strong>Primary/Secondary Storage</strong></p>
</div>
<div style='float: right; width:0%;'>
<p><img alt="image" src="/subject-images/iitpal/image/chemistry-class-12-unit-03-chapter-05-electro-chemistry-l-5_6-yhyukobqg-i-169-2835.6.jpg"></p>
</div>
</main>
<hr>
<footer style="font-size:18px;"> Gibb's free energy $\rightarrow$ Electrolytic cell $\rightarrow$ Electrolysis $\rightarrow$ Electrolysis of pure-high resistance $\rightarrow$ Faraday's law $\rightarrow$ Electrolysis of brine solution $\rightarrow$ Types of cell $\rightarrow$ Lead-acid storage cell (1859) $\rightarrow$ Problems $\rightarrow$ Dry cell $\rightarrow$ <span style="color:blue">Modern version of primary storage (1949)</span> </footer>