(d) Why are active metals such as Al obtained by electrolysis using molten salts rather than aqueous solutions?

Video transcript

Hello everyone. So in this video we're being asked, why can't we use a quick solutions to obtain active metals via electrolysis? So let's recall some very important information about our reduction potentials. So a larger positive value of reduction potential indicates a greater tendency to get reduced. Let's go ahead and put this in writing. So basically to simplify or summarize this, if we have a larger reduction potential volume is going to get reduced or it increases the chances of it being reduced. So running out the camel called equation of water or like electrolysis of water, we have two moles of H 20. Of course, that's in a liquid state. We're gonna go ahead and add two electrons status to go ahead and produce H two gas And two moles of our hydroxide, which is. And the reduction potential for this, which is R E. Red is equal to r negative 0. volts. And active metals need to have a larger reduction potential than of this value right over here or else it won't be reduced in the presence of water. And knowing this fact, then then our answer for this question is that we cannot use agree a solutions of the active medal to obtain the metal of electrolysis unless the metal act is let's see, let's go ahead, write this out. So the metal unless the active medal, the red is greater than the red of water. So right here is going to be my final answer for this problem