Describe galvanic cells that use the following reactions. In each case, write the anode and cathode half-reactions and sketch the experimental setup. Label the anode and cathode, identify the sign of each electrode, and indicate the direction of electron and ion flow. (b)

Video transcript

Hello everyone in this video. We're given this following reaction here. We're trying to determine the cathode and an on half reactions. We also want to draw the electrochemical cell, label it correctly and show the direction of the flow of electrons and ions. Starting off with my cap outside which is where reduction occurs. This reaction is going to be the lead two plus Reacting with two electrons To give us a lead in its solid state. The standard reduction potential value here is equal to negative 0.126V. Then for my channel is where oxidation occurs. So we have our chromium in its solid state. This yields chromium two plus And two electrons. So the center reduction potential here is equal to 0.913V. We're gonna go ahead and calculate for the overall e cell value. So we're just gonna go ahead and add both standard reduction potential values. That zero point or negative 0.1 to six volts with 0.913 volts. Once you put that into the calculator receive that the resell value is equal to 0.805 volts. So we're gonna see here that the potential for the value is greater than one or is greater than zero because we have a positive value. So this is a galvanic cell and sell the antidote is the negative terminal while the cathode is the positive terminal. So electrons will flow from the road into the cathode and a galvanic cell also requires a salt bridge such as K N. 03. So out of the answer choices A and B, we can see here that what best fits our description earlier is going to be answer choice A. So answer choice A is going to be my final answer for this problem.