[" If "[E_()^(@),_Cu^(2)+_(ICu),=0.34vv" and "E_(Au^(3+)/Au)=1.4vv" then "E_(" Cell ")^(@)" for cell reaction "3Cu(s)+2Au^(3+)],[(aq)rarr3Cu^(2+)(aq)+2Au(s)," is "]]

If E_(Cu^(2+)|Cu^(+))^(@)=+0.15V and E_(Cu^(2+)|Cu)^(@) and E_(Cu^(2+)|Cu)^(@)=+0.34V at 25^(@)C, then E^(@) value of the reaction 2Cu^(+)(aq)rarr Cu^(2+)(aq)+Cu(s) is -

If E_(Au^(+)//Au)^(@) is 1.69 V and E_(Au^(3+)//Au)^(@) is 1.40 V, then E_(Au^(+)//Au^(3+))^(@) will be :

If E_(Au^(+)//Au)^(@) is 1.69 V and E_(Au^(3+)//Au)^(@) is 1.40 V, then E_(Au^(+)//Au^(3+))^(@) will be :

If E_(Au^(+)//Au)^(@) is 1.69 V and E_(Au^(3+)//Au)^(@) is 1.40 V, then E_(Au^(+)//Au^(3+))^(@) will be :

If E_(Au^(+)// Au)^(@) is 1.69 V and E_(Au^(3+)//Au)^@ is 1.40 V . Then E_(Au^(+)//Au^(3+))^(@) will be :

For the cell reaction Zn(s) + Cu^(2+)(aq) rarr Cu(s) + Zn^(2+)(aq) E_("cell")^(@) = 1.10 V, DeltaG^(@) is :

E^(@) for the electrochemical cell Zn(s) | Zn^(2+)1M (aq)|| Cu^(2+) 1M(aq)| Cu (s) is 1.10 V at 25^(@) C. The equilibrium constant for the cell reaction, Zn(s)+Cu^(2+) (aq.) rarr Zn^(2+) (aq.) + Cu(s) will be:

For the half-cell reaction, Au^(3+) + 3e^(-) rarr Au the value of n used in Nernest equation is: