Calculate `DeltaG^(@)` and log `K_(c)` for the following reaction at 298 K :
`2Al(s)+3Cu^(2+)(aq)rarr2Al^(3+)(aq)+3Cu(s)`
Given `E_(cell)^(@)`=2.02 V

Calculate E_("cell")^(@) for the following reaction at 298K : 2Al(s)+3Cu^(2+)(0.01M)rarr 2Al^(3+)(0.01M)+3Cu(s) [GIven E_(cell)=1.98V ]

Calculate E_(cell)^(@) for the following reaction at 298 K. 2Al_((s)) + 3Cu^(2+)(0.01M) rightarrow (0.01M) + 3Cu_((s)) Given : E_(cell) = 1.98V |

Write Nernst equation for the following cell reaction: 2Al(s)+3Fe^(2+)(aq)rarr2Al^(3+)(aq)+3Fe(s)

Calculate the equilibrium costant log (K_(c)) for the reaction Zn(s)+Cu^(2+)(aq)rarrZn^(2+)(aq)+Cu(s) [Given E_(cell)^(2)=1.1 V ]

In the cell reaction: 2Al(s)+3NI^(2+)(aq)rarr2Al^(3+)(aq)+3Ni(s) The value of n is

Calculate the equilibrium constant of the following reaction aty 298K. Cu(s)+2Ag^+(aq) rarr Cu^(2+)(aq)2Ag(s)~ Given E_(cell)^Theta=0.46V

Calculate the equilibrium constant for the reaction at 298 K Zn(s)+Cu^(2+)(aq)harr Zn^(2+)(aq)+Cu(s) Given " " E_(Zn^(2+)//Zn)^(@)=-0.76 V and E_(Cu^(2+)//Cu)^(@)=+0.34 V

Calculate the equilibrium constant for the reaction at 298K. Zn(s) +Cu^(2+)(aq) hArr Zn^(2+)(aq) +Cu(s) Given, E_(Zn^(2+)//Zn)^(@) =- 0.76V and E_(Cu^(2+)//Cu)^(@) = +0.34 V

Calculate the equilibrium constant for the reaction at 298K. Zn(s) +Cu^(2+)(aq) hArr Zn^(2+)(aq) +Cu(s) Given, E_(Zn^(2+)//Zn)^(@) =- 0.76V and E_(Cu^(2+)//Cu)^(@) = +0.34 V