Home
Class 12
CHEMISTRY
Calculate E("cell")^(0) of the following...

Calculate `E_("cell")^(0)` of the following galvanic cell
`Mg(s) // Mg^(2+)(1 M) // Ag^(+)(1 M) // Ag(s)` if `E_(Mg)^(0) = -2.37V` and `E_(Ag)^(0) = 0.8V`. Write cell reactions involved in the above cell. Also mention if cell reaction is spontaneous or not.

Text Solution

AI Generated Solution

Promotional Banner

Similar Questions

Explore conceptually related problems

Calculate the voltage of the cell Sn(s) // Sn^(2+)(0.02 M) // Ag^(+)(0.01 M) // Ag(s) at 25^(@)C. Given: E_(Sn)^(0) = -0.136V , E_(Ag)^(0) = 0.800V

Calculate the emf for the following cell at 298 K. Cd//Cd^(2+)(0.1 M) || Ag^(+)(0.1 M)//Ag "Given"E_(Cd^(2+)//Cd)^(@)=-0.40" V ",E_(Ag^(+)//Ag)^(@)=0.80" V "

Calculate emf and DeltaG for the following reaction at 298 K Mg(s)|Mg^(2+)(0.01 M)||Ag^(+)(0.0001 M)|Ag(s) Given E_((Mg^(2+)//Mg))^(@)=-2.37" V ", E_((Ag^(+)//Ag))^(@)=+0.80" V "

Calculate the emf of the following cell at 298K: Mg(s)|Mg^(2+)(0.1M)||Cu^(2+)(1.0xx10^(-3)M)|Cu(s) [Given= E_(Cell)^(@)=2.71V ]

Calculate the e.m.f of the cell Mg(s)//Mg^(2+)(0.1 M)||Cu^(2+)(1.0xx10^(-3) M)//Cu(s) Given E_(Cu^(2+)//Cu)^(@)=+0.34 V and E_(Mg^(2+)//Mg)^(@)=-2.37 V

Calculate the emf of the following cell: Cu(s)|Cu^(2+) (aq)||Ag^(+) (aq)| Ag(s) Given that, E_(Cu^(2+)//Cu)^(@)=0.34 V, E_(Ag//Ag^(+))^(@)=-0.80 V

Find E_(cell)^(@) for the cell : Zn | Zn^(2+)(1M) || Ag^(+)(1M) | Ag [Given that : E_(Zn//Zn^(2+))^(@)=0.76" V" , E_(Ag^(+)//Ag)^(@)=0.80" V" .

Calculate the e.m.f. of the following cell at 25^(@)C Mg(s)//Mg^(2+)(0.01 M)||Sn^(2+)(0.1 M)//Sn(s) Given " " E_(Mg^(2+)//Mg)^(@)=-2.34 V, E^(@)Sn^(2+)//Sn=-0.136 V Also calculate the maximum work that can be accomplished by the operation of the cell.