Home
Class 12
CHEMISTRY
Calculate E(" cell ")^(@) E("cell ") ...

Calculate `E_(" cell ")^(@) E_("cell ")` and `Delta G` for the following reaction at `25^(@)C`
`Mg_((s)) + Sn^(2+) (0.03 M) to Mg^(2+) (0.04 M) + Sn_((s))`
`E_(Mg^(+2)|M) ^(@) =- 2.37 V` and `E_(Sn^(2+) | Sn)^(@) =- 0.14 V`
is the reaction spontaneous

Text Solution

Verified by Experts

`(i) E_("cell ")^(@) =2 .23 V , (ii) E_("cell ") =2.226 V Delta G =429 .6 kJ`
`(iii) ` Since `E_("cell ") gt 0, Delta G lt 0` the reaction is spontaneous
Promotional Banner

Similar Questions

Explore conceptually related problems

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 "

Consider the cell potentials E_(Mg^(2+)|Mg)^(0)=-2.37V and E_(Fe^(3+)|Fe)^(0)=-0.04V The best reducing agent would be

Calculate equilibrium constant for the reaction : Mg(s) |Mg^(2+)(0.001 M) || Cu^(2+)(0.0001 M)|Cu(s) Given E_((Mg^(2+)//Mg))^(@)=-2.37" V " , E_((Cu^(2+)//Cu))^(@)=0.34" 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.

Write Nernst equation and calculate e.m.f of the following cells at 298 K : Sn (s) |Sn^(2+) (0.050 M) ||H^(+) (0.020 M) |H_(2) (1atm) | Pt Given : E_((Sn^(2+) | Sn))^(Theta) = -0.14 V

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.