`E^(@) (SRP)` of different half cell given
`{:(E_(Cu^(2+)//Cu)^(@) =0.34"volt",,,E_(Zn^(2+)//Zn)^(@) =- 0.76"volt"),(E_(Ag^(+)//Ag)^(@) = 0.8"volt",,,E_(Mg^(2+)//Mg)^(@) =- 2.37 "volt"):}`
In which cell `Delta^(@)` is most negative:-

E_("red")^(0) (Standard reduction potential ) of different half-cells are given E_(Cu^(+2)//Cu)^(0) = 0.34 V E_(Zn^(+2)//Zn)^(0) = -0.76 V , E_(Ag^(+) // Ag)^(0) = 0.80 V , E_(Mg^(2+) // Mg)^(0) = -2.37 V . In which cell DeltaG^(@) is most negative ?

Redox reactions play a pivotal role in chemistry and biology. The values of standard redox potential (E^(@)) of two half-cell reactions decide which way the reaction is expected to proceed. A simple example is a Daniel cell in which zinc goes into solution and copper gets deposited. E^(@)(SRP) of different half cells are given below: E_(Cu^(2+)|Cu)^(@)=0.34V, E_(Zn^(2+)|Zn)^(@)=-0.76V E_(Ag^(+)|Ag=0.8V, E_(Mg^(2+)|Mg))=-2.37V In which cell, DeltaG^(@) per "mole" of electron is most negative?

E^(c-)._(red) of different half cell are given as : E^(c-)._(Cu^(2+)|Cu)=0.34V,E^(c-)._(Zn^(2+)|Zn)=-0.76V . E^(c-)._(Ag^(o+)|Ag)=0.80 V, E^(c-)._(Mg^(2+)|Mg)=-2.37V. In which cell DeltaG^(c-) is most negative ?

E^(c-)._(red) of different half cell are given as : E^(c-)._(Cu^(2+)|Cu)=0.34V,E^(c-)._(Zn^(2+)|Zn)=-0.76V . E^(c-)._(Ag^(o+)|Ag)=0.80 V, E^(c-)._(Mg^(2+)|Mg)=-2.37V. In which cell DeltaG^(c-) is most negative ?

When E_(Ag^(+) | Ag)^@ = 0.80 volt and E_(Zn^(2+)|Zn)^@ = 0.76 volt, which of the following is correct?

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" .

Given E_(Ag^(+) // Ag)^(0) = 0.80 V , E_(Mg^(2+) // Mg)^(0) =-2.37 V , E_(Cu^(2+) // Cu)^(0) = 0.34 E_(Hg^(2+) // Hg)^(0) = 0.79 V Which of the following statement is / are correct ?

Given : E_(Ni^(2+)|Ni)^(@)=-0.25V, E_(Zn^(2+)|Zn)^(@)=-0.76V, E_(Cu^(2+)|Cu)^(@)=+0.34V, E_(Ag^(+)|Ag)^(@)=+0.8V . Under standard conditions, which reaction(s) will occur spontaneously -