calculate the minimum P.D. to reduce `Al_(2)O_(3)` 500°C. [Given ∆G=+960 kj,1F=96,500C `mol^(-1)`]

Calculate the minimum emf required to carry out the electrolysis of Al_(2)O_(3) Given that, DeltaG for the reaction (4)/(3)Al +O_(2) to (2)/(3)Al_(2)O_(3) is -827 kJ mol^(-1)

Calculate the strength of the current required to deposit 1.2 g of magnesium from molten MgCl_(2) in 1h. [ 1F = 96500 C "mol"^(-1) , Atomic mass of Mg = 24.0 ]

The standard electrode potential ( E^(@) ) for Daniel cell is + 1.1 V. Calculate, the Delta G^(@) for the reaction, Zn(s) + Cu^(2+) ( aq) rarr Zn^(2+) ( aq) + Cu(s) 1F = 96500 C "mol"^(-1))

Calculate the temperature at which a solution containing 54 g of glucose (C_(6)H_(12)O_(6)) in 250 g of water will freeze. ( K_(f) for water = 1.86 K mol^-1 kg).

Calculate kinetic energy of 1 gm of helium at 127^@C . Given that R= 8.31 j/(mol K) , M=4g/(mol)

The value of Delta_(f)G^(@) for the formation of Cr_(2)O_(3) is-540 kJ "mol"(-1) and that of Al_(2)O_(3) is - 827 kJ mol-¹. Is the reduction of Cr_(2)O_(3) possible with Al?

Calculate the standard cell potential of a galvanic cell in which the following reaction takes place 2Cr(s) + 3Cd^(2+) ( aq) rarr 2Cr^(3+) ( aq) + 3Cd(s) Calculate Delta_( r) G^(@) and equilibrium constant K of the above reaction at 25^(@)C . [Given, E_(Cr^(3+) //Cr)^(@) = - 0.74 V, E_(Cd^(2+)//Cd)^(@) = - 0.40V, 1F = 96500 C "mol"^(-1)]