Sketch a voltaic cell for each redox reaction. Label the anode and cathode and indicate the half-reaction that occurs at each electrode and the species present in each solution. Also indicate the direction of electron flow. a. Ni2+(aq) + Mg(s) ¡ Ni(s) + Mg2+(aq)

Video transcript

Hello everyone today. We are being asked to consider the following redox reaction. So we have this redox reaction here and then we're asked to identify the correct it'll take cell that represents the equation above. So we want to first recall some basic principles at the anodes oxidation is occurring and at the cathode we have our reduction And so our second principle or a second point to make is we want to write what the reaction at the anodes looks like. So at the anodes since we have oxidation, we're losing electrons that could be represented by our lead solid with an arrow being dissociating into our lead two plus ions as well as two electrons that were lost. And then for our catheter reduction, the gaining of electrons that can be denoted by our silver Gaining two electrons or plus two electrons to form our silver solid. Next we must make note that in a voltaic cell we are going to be utilizing a volt meter. So that immediately gets rid of answer choices B and C. Since they use batteries. And so in determining what the answer would be between A and D. We must know and look at where these reactions are going and where the electronic flow is. And so if we look closely, we can see that the answer choice. The correct answer is answer choice A Because it correctly shows the electrons flowing from the anodes where oxidation is happening. We're losing those electrons and then it shows where the cathode or reduction is happening, where those electrons are being gained. And so anti choice is correct. I hope this helped, and until next time.