The standard Gibbs energy `(Delta r G^@)` for the following cell reaction is `-300 kJ mol^(-1)` :
`Zn(s) + 2Ag^(+) (aq) to Zn^(2+) (aq) + 2Ag(s)`
Calculate `E_("cell")^@` for the reaction. (Given 1F` = 96500 mol^(-1)`)

The standard Gibbs energy for the given cell reaction is KJmol^(-1) at 298 K is : Zn(s)+CU^(2+) (aq) rightarrow Zn^(2+) (aq) + Cu(s) E^(@)= 2V at 298 K (Friday's constant , F = 96000 C mol^-1 )

Write Nernst equation for the following cell reaction : Zn(s) | Zn^(2+)(aq)|| Cu^(2+)(aq) | Cu(s)

Consider the following cell reaction Cu(s)+2Ag^(+)(aq) rarr Cu^(2+) (aq) +2Ag(s) E_("cell")^(@)=0.46 V By boubling the concentration of Cu^(2+) , E_("cell") is

The reaction, (1)/(2) H_(2) (g) + Ag Cl (s) = H^(+) (a.q) + Cl^(-) (a.q) + Ag (s) occurs in the galvanic cell:

Consider Delta G^(@) for the following cell reaction : Zn (s) + Ag_(2)O(s)+H_(2)O(l) hArr Zn^(2+)(aq)+2Ag(s)+2OH^(-)(aq) E_(Ag^(+)//Ag)^(@) = +0.80 and E_(Zn^(2+)//Zn)^(@) = - 0.76 V

(a) The cell in which the following reactions occurs: 2Fe^(3+)(aq)=2I^(-)(aq)to2Fe^(2+)(aq)+I_(2)(s) has E_(cell)^(@)=0.236V at 298 K. Calculate the standard Gibbs energy of the cell reaction. (Given: 1F=96,500" C "mol^(-1) ) (b) How many electrons flow through a metallic wire if a current of 0.5 A is passed for 2 hours? (Given: 1F=96,500" C "mol^(-1) )