00:01
This question is moderately complicated, so let's take it one step at a time.
00:05
We need to use the equations that relate the cell potential to the equilibrium constant.
00:13
We also need to use hess's law.
00:18
The hint suggests that we use the ksp expression and the standard reduction potential for silver.
00:25
So here's the ksp expression for silver iodide.
00:29
We have silver iodide solid going to silver ion plus iodide.
00:33
An ion, and ksp for this is 1 .5 times 10 to the negative 16.
00:42
We also have a reduction potential for silver ion, taking on one electron to become silver solid, and this standard reduction potential is 0 .80 volts.
00:54
Now, we can combine these two equations to get the overall equation, but we can't combine k and e, so we need to convert either the k into an e or the e into a k, it's always better when using hesse's law to work with k values or to work with delta g values, not e values.
01:20
So let's convert our e standard for the second reaction into a k value...
