Can someone explain this to me on how to work out the process? Thanks
By convention, all of the equilibria are shown as reductions. Hence, the values are referred to as standard reduction potentials.
The equilibria of course can go either way, but only if there is an appropriate species that can either receive or donate the electrons involved.
The spontaneity of a possible (hypothetical) reaction depends on the cell potential once a reducing agent is put together with an oxidising agent. The reducing agents appear on the right hand side and the oxidising agents on the left hand side.
The cell potential is calculated as E(cell) = E(reduced species) - E(oxidised species) If E(cell) is positive the hypothetical reaction can happen (is spontaneous), although it is possible that an equilibrium may result If E(cell) is positive and greater than 0.3V the reaction is likely to go all the way If E(cell) is negative then the proposed reaction is not possible (under standard conditions)
By convention, all of the equilibria are shown as reductions. Hence, the values are referred to as standard reduction potentials.
The equilibria of course can go either way, but only if there is an appropriate species that can either receive or donate the electrons involved.
The spontaneity of a possible (hypothetical) reaction depends on the cell potential once a reducing agent is put together with an oxidising agent. The reducing agents appear on the right hand side and the oxidising agents on the left hand side.
The cell potential is calculated as E(cell) = E(reduced species) - E(oxidised species) If E(cell) is positive the hypothetical reaction can happen (is spontaneous), although it is possible that an equilibrium may result If E(cell) is positive and greater than 0.3V the reaction is likely to go all the way If E(cell) is negative then the proposed reaction is not possible (under standard conditions)
Ok thanks so how would I write this first equation?