 This standard hydrogen electrode SHE may behave as cathode or phenol, may behave as cathode or SHE, standard hydrogen electrode. So if you draw the diagram of this, we will have a hydrogen electrode, right? This is the diagram of standard hydrogen electrode. This is the inlet of hydrogen gas, H2 gas, right? And since it is a gas, so we have to provide the surface where the reaction takes place, right? And that is why we are using platinum there in this demonstration, right? So how do we represent that? This is a platinum wire and here we have the platinum sheet coated with a black color so that the adsorption of H2 gas will be more, right? So what happens is this H2 gas comes through here and it adsorbs on the surface, right? What is this like here? What is this like? H2-SCl. H2-SCl, we can take H2-SCl also, right? It is H2-SCl. What is the concentration of this? 1 molar. Why 1 molar? Because it is the standard. That is why it is 1 molar. For standard, it is defined temperature is tonight 8 Kelvin and concentration is unit concentration, 1 molar, right? And the concentration of HCl is what? 1 molar, right? So it is measured with 1 molar concentration or molar base? No, it is not like that. Concentration will always take 1 molar. Because we are trying to get 1 molar of H plus 1. No, 1, the acid that we are taking, the concentration of this is 1 molar. Concentration of acid should be 1 molar if it is standard. Now this is a platinum wire. What is this? It is a platinum sheet and this is the platinum wire. This kind of, you know, the setup is not required when you have a solid electrode, that zinc. What we do in case of zinc? We just dip the electrode, zinc electrode. But since it is a gas, so we have to provide the surface as well as the setup. Okay? Now this is the standard hydrogen electrode. Now suppose if you have to find it out for copper, so what we do? We take a copper electrode with copper oxide and we connect that with the boiling material. Whatever reflection we have, Tm of the cell that we can find it out, right? So that we are not going to discuss one by one. Just we will see one example of copper. Now for this one, since this can behave as cathode and anode both, so if it is behave as cathode, what is the reaction then? Reduction takes place, right? For 2H plus we get reduced into, right? And the E naught value of this is what? E naught of H plus to H2 is equals to what? Zero because we have assumed the standard hydrogen electrode at zero electrode potential, right? Our assumption is this, at 298 Kelvin and this is the assumption we have, okay? If it behaves as anode then the reaction. So anode reaction is what? H2 gas converts into 2H plus equals plus 2 electron. And hence its E naught value is what? E naught of H2 H plus will be zero again at the same condition 288 Kelvin and this is the assumption, okay? Now if we have to, you have to draw this diagram again, okay? I am doing this one. If we have to find out for copper, we will take copper electrode. This is the copper rod placed in that was Cu S O 4 solution, one moment of concentration. And this is connected with voltmeter and this will work. Now deflection in voltmeter gives you E naught of the cell, okay? Deflection in voltmeter gives you the EMF of the cell. Now the formula of E naught cell is what? E naught cell, what is the formula? E of? Capital minus. If I am taking production potential, so capital minus? Capital. Anode. Anode. So the reaction of cathode is getting reduced to Cu 2 plus converting into C and the anode reaction is E of H2 2. It is also production potential, you know? H plus 2 H2. Production potential we have, so it is production H plus 2 H2. When you write H2 2 H plus it is oxidation, right? But whatever it is, it will be zero. And this value is what? This is the rating in, in what? Voltmeter. Voltmeter. Voltmeter. Sir, this means salt will not be required. Salt will be required. Yes, salt will be required. This salt will not be considered. Salt will be required, it is understood. Without salt it will not work. But not. Right? Salt will not work. Right? So in our cell, whatever the rating you get here, in our cell is the value of that standard electrode potential, which is found to be what? Zero point? That is how we find out the reduction potential of all the electrodes. Suppose we, 2.7 is the value of this standard. Isn't it 2.7? 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. 25. other electrode and if we arrange them in ascending or descending order, if we arrange them in ascending or descending order, we will get a series which is known as electrochemical series so the electrochemical series actually you have to memorize it is given in the book that E naught value of h2 to h plus is 0 and this is in between right and here also we have some measure here also we have some measure the nature of this series you have to keep in mind values will be given in the questions you do not have to memorize the values ok. Lithium has highest negative reduction potential and chlorine has most positive reduction potential again this also you do not have to remember right but here as the most negative reduction potential we have most negative reduction potential and this one we have most positive reduction potential so maximum reduction potential we have here so it is a maximum tendency to get reduced right so as we go down from this h plus part we go down in this electrochemical series the tendency to get reduced will increase it means it is a better oxidizing agent right so first property here is more strong is reducing right if it is also as reduction potential increases its tendency to get reduced will be reduced what we have done so far zinc is minus 0.76 copper is 0.34 copper has higher rp so copper will get reduced and zinc will get oxidized right so more reduction potential means what more tendency to get reduced and more tendency to oxidizes it means more rp stronger oxidizing agent understood as the reduction potential increases as rp increases the tendency to get reduced will be more and hence it is a good oxidizing agent it is a good oxidizing agent right so as we go from bottom to top it will be a good reducing agent it will easily get oxidized and reduce others and this will be a good oxidizing that is what you have to give you the property of this electrochemical series values you do not have to memorize values will be given in the question okay now the next thing we have to discuss is NUST equation you know what is NUST equation derivation you have done derivation of NUST equation you have done yes or no