I shall return!
\(OH\) is an oxidative carrier that gives up its \(O\) at the anode.
\(H_2O^{+}\) or \(LiH^{+}\) are reductive carriers that gives up its \(H\) at the cathode.
This way, if ever we have a \(OH^{-}\), this is a CHARGED oxidative carrier.
A charged oxidative carrier will redistribute between the cathode and the anode naturally.
Furthermore, a buildup of \(OH\) causes the build up of \(LiOH\) as the carriers react,
\(LiH^{+}+2OH\rightarrow LiOH\cdot H_2O\) Lithium hydroxide
Lithium hydroxide monohydrate is much more soluble in water than in organic solvents, but none the less as its concentration increases locally it will precipitate out of the electrolyte. Both types of redox carriers are removed from solution and the battery electron production goes dead.
Heat can redistribute a charge neutral oxidative carrier, but in most battery design, the anode charge collector is a pin in a cylindrical cathode along the major axis that has a comparatively high concentration of heat. The cathode spreads out in the form of a cylinder around the anode has a lower concentration of heat per unit area. Heat in such designs drives the carriers away from the anode reaction site. Strictly speaking, the anode reactant are spread in the electrolyte uniformly, a charge collector pin provides the reaction site at which the anode reactant are oxidized. This way the battery discharge slowly.
A temperature gradient will act on both types of carriers, the diffusion rate at higher temperature will always be higher irrespective of whether the carrier is charged or not
Heat also facilitates the precipitation of \(LiOH\), breaks down the electrolyte and triggers undesirable chemical reactions in the constituent of the battery. This is how heat kills a battery.
This is a more expensive battery,
The wire cage requires more material and is difficult to form. The hollow cathode also be difficult to form. But the heat flows from the cathode to the wire cage in aid of \(OH\) carrier return to the anode. Heat is still concentrated at the cathode because of the small reaction area. The charged redox carrier, \(H_2O^{+}\) is still aided by its charge to move towards the cathode.
But the real improvement will be the use of chlorophyll and photosynthesis chemistry.
