The Gibbs energy for the decomposition of `FeO` at `600^@ C` is as follows
`FeO rarr Fe + (1)/(2) O_2 Delta_r G = 856 kJ//"mole"` the potential difference needed for electrolytic reduction of `FeO` at `600^@ C` is at least.

The Gibbs energy for the decomposition of Al_2 O_3 at 2/3 Al_2O_3 rarr 4/3 Al = O_2 Delta_r G = + 966 k J "mol"^(-1) The potential differnce needed for electrolytic reduction of Al_2 O_3 at 500^@C is at least.

The Gibbs energy for the decomposition of Al_(2)O_(3) at 500^(@)C is as follows : (2)/(3)Al_(2)O_(3)rarr (4)/(3)Al+O_(2), Delta_(r)G=+"960 kJ.mol"^(-1) . The potential difference needed for the electrolytic reduction of aluminium oxide (Al_(2)O_(3)) at 500^(@)C is at least -

The Gibbs energy for the decomposition of Al_(2)O_(3) at 500^(@)C is as follows: (2)/(3)Al_(2)O_(3) rarr (4)/(3)Al + O_(2), Delta_(r)G = +966kJ mol^(-1) The potential difference needed for electrolytic reduction of Al_(2)O_(3) at 500^(@)C is at least:

The Gibbs energy for the decomposition of Al_(2)O_(3) at 500^(@)C is as follows : 2/3 Al_(2)O_(3) rarr 4/3 Al + O_(2), Delta_(r)G= +966 "kJ mol"^(-1) The potential difference needed for electrolytic reduction of Al_(2)O_(3) at 500^(@)C is at least :

The Gibbs energy for the decomposition of Al_(2)O_(3) at 500^(@)C is as follow : (2)/(3)Al_(2)O_(3) rarr (4)/(3)Al+O_(2), Delta_(r)G= +960 kJ mol^(-1) The potential difference needed for the electrolytic reduction of aluminium oxide (Al_(2)O_(3)) at 500^(@)C is

The Gibbs energy for the decomposition of Al_(2)O_(3) at 500^(@)C is as follows: (2)/(3)Al_(2)O_(3) rarr (4)/(3)Al + O_(2), Delta_(r)G = +966kJ mol^(-1) The potential difference needed for electrolytic reeduction of Al_(2)O_(3) at 500^(@)C is at least:

The Gibbs energy for the decomposition of Al_(2)O_(3) at 500^(@)C is as follows: (2)/(3)Al_(2)O_(3) rarr (4)/(3)Al + O_(2), Delta_(r)G = +966kJ mol^(-1) The potential difference needed for electrolytic reeduction of Al_(2)O_(3) at 500^(@)C is at least: