00:01
To determine the cell potential we'll be using the nernst equation.
00:06
The chemical reaction is br aqueous reacting with chromium solid to produce cr3 plus and br minus.
00:15
To balance it we'll put a three in front of the br2, a six in front of the bromide, and then twos in front of the chromiums.
00:25
E cell will then be equal to e cell standard, which will be the reduction potential that want for the thing that wants to be reduced the most to have a galvanic cell, and then subtract off the reduction potential for what ends up being oxidized at the anode.
00:47
So it's cathode minus anode.
00:50
The rest of the nernst equation is minus at 25 degrees celsius, we can use the constant 0 .05916.
00:59
We then divide by n.
01:01
Each chromium loses three electrons, but there are two of them, so that's a total of six electrons, and then we multiply by the log of q.
01:10
Q is going to be the concentration of cr3 raised to its coefficient of two, multiplied by the concentration of the other product br minus raised to its coefficient of six...