For the reaction :
`4Al+ 3O_(2) + 6H_(2)O+ 4OH^(-) rightarrow4A1(OH)_(4)^(-) E^(@)_(cell) = 2.73V`.
Standard Gibb's free energy change for the reaction is :

DeltaG^(c-) or the reaction is , 4Al+3O_(2)+6H_(2)O+4overset(c-)(O)H rarr 4 Al(OH)_(4)^(c-) E^(c-)._(cell)=2.73V Delta_(f)G^(c-)._((overset(c)(O)H))=-157k J mol^(-1) Delta_(f)G^(c-)._((overset(c-)(O)H))=-237k J mol^(-1)

In a fuel cell methanol is oxidised with oxygen as : CH_(3)OH(l) + 3/2O_(2)(g) to CO_(2)(g) + 2H_(2)O(l) Calculate the standard Gibbs energy change for the reaction that can be converted into electrical works. If standard enthalpy of combustion for methanol is 726 kJ mol^(-1) , calculate the efficiency of conversion of Gibbs energy into useful work. The standard Gibbs energies of formation, Delta_(f)G^(@)(kJ mol^(-1)) are : CO_(2)(g) = -394.4, H_(2)O(l) = -237.2, CH_(3)OH(l) = -166.2 .

In the reaction, B(OH)_(3) + 2H_(2)O to [B(OH)_(4)]^(-) + H_(3)O^(+) ,B(OH)_(3) functions as

In the following balanced reaction, 4O_(2)^(x)+2H_(2)O rarr 4OH^(-)+3O_(2)

In the reaction [A (H_(2)O)_(6)]^(3+)+H_(2)O hArr [Al(H_(2)O)_(5)OH]^(2+)+H_(3)O^(+)

Silane (SiH_(4)) burns in air as: SiH_(4)(g) +2O_(2)(g) rarr SiO_(2)(s) +2H_(2)O(l) the standard Gibbs energies of formation of SiH_(4)(g), SiO_(2)(s) , and H_(2)O(l) are +52.3, -805.0 , and -228.6kJ mol^(-1) , respectively. Calculate Gibbs energy change for the reaction and predict whether the reaction is spontaneous or not.

The standard change in Gibbs energy for the reaction: H_2O hArr H^+ +OH^- at 25^@C is :

In the following reaction: Cr(OH)_(3)+OH^(-)+IO_(3)^(-) toCrO_(4)^(2-)+H_(2)O+I^(-)