Calculate the Gibbs energy change for the reaction given below:
`Zn_((s))+Cu_((s))^(2+)toCu_((s))+Zn_((aq.))^(2+)`
Given that standard Gibbs energy (`G^@`) for `Zn_((aq.))^(2+),Cu_((aq.))^(2+)` are `-147.2 kJ mol^(-1)` and `65.0 kJ mol^(-1)` respectively.

Zn_((s))+Cu_((aq))^(+2) rarr Cu_((s))+Zn_((aq))^(+2) given that Delta_(f)G^(@) for Cu_((aq))^(+2) and Zn_((aq))^(+2) as 65 kJ mol^(-1) and -147.2 kJ mol^(-1) respectively. Then the standard Gibb's energy change for the above reaction is

Calculate the standard free energy change for the reaction, Zn+ Cu^(2+) rarr Cu + Zn^(2+) Given that standard free energy (G°) for Zn2+(aq), Cu2+(aq), are -147.2 kJ mol-1 and 65.0 kJ mol-1 respectively.

Calculate DetlaG^(@) for the following reaction, Zn_((s)) + Cu_((aq))^(2+) to Zn_((aq))^(2+) + Cu_((s)) . DeltaG_(f)^(@) of Zn_((aq))^(2+) and Cu_((aq))^(+2) is -147.2 kJ mol^(-1) and 65kJmol^(-1) .

Calculate the standard free enegry change for the reaction: Zn + Cu^(2+)(aq) rarr Cu+Zn^(2+) (aq), E^(Theta) = 1.20V

Calculate the standard free enegry change for the reaction: Zn + Cu^(2+)(aq) rarr Cu+Zn^(2+) (aq), E^(Theta) = 1.20V

For the Daniel Cell involving the cell reaction Zn_((s))+Cu_((aq))^(+2)hArrZn_((aq))^(+2)+Cu_((s)) the standard free energies of formation of Zn_((s)),Cu_((s)),Cu_((aq))^(+2) and Zn_((aq))^(+2) are 0, 0, 64.4 KJ/Mole and -154.0 KJ/Mole, respectively. Calculate the standard EMF of the cell

Zn_((s)) + Cu_((aq))^(2+) to Zn_((aq))^(2+) + Cu_((s)) . In this reaction, which gets oxidised?

Represent the galvanic cell in which the reaction Zn_((s))+ Cu_((aq))^(2+)rightarrowZn_((aq))^(2+)+Cu_(s) take place .

Calculate the standard free energy change for the following reaction Zn(s) + Cu^(2+)(aq) to Zn^(2+) (aq) + Cu(s) Given : Delta_fG^@ [Cu^(2+)(aq)] = 65.0kJ mol^(-1) Delta_f G^@ [ Zn^(2+) (aq)] = -147.2 kJ mol^(-1)