Given, the standard electrode potentials, `K^+//K = -2.93 V, Ag^+//Ag = 0.80 V, Hg^(2+)//Hg =0.79 V, Mg^(2+)//Mg = - 2.37 V, Cr^(3+)//Cr = - 0.74 V` Arrange these metals in their increasing order of reducing power.

The strongest oxidizing agent among the species In^(3+) (E^@ = -1.34V), Au^(3+) (E^@ = 1.4V) , Hg^(2+) (E^@=0.86V),Cr^(3+)(E^@=-0.74V) is

The cell reaction of a cell is Mg+Cu^(2+) to Mg^(2+)+Cu (Given E_(Mg^(2+)//Mg) = -2.37 V , E_(Cu^(2+)//Cu) = 0.337 V ) The e.m.f of the cell will be _________.

Reduction potentials of A, B, C and D are 0.8 V, 0.79 V ,0.34 V and -2.37 V respectively. Which element displaces all the other three elements ?

The standard reduction electrode potential values of the elements A, B and C are + 0.68, - 2.50 and -0.50 V respectively. The order of their reducing power is

The standard reduction potenital of Zn^(2+)//Zn and Ag^(+)//Ag at 25^(@)C are -0.76 V and +0.80 V. Which of the following reactions actually takes place ?

Write the Nernst equation and emf of the following cells at 298K. Mg_((s))| Mg_(aq)^(2+)(0.001M)| Cu_((s)) (Given E_(Mg^(2+)//Mg)^@ = -2.37 V, E_(Cu^(2+) //Cu)^@=0.34V)

The standard potential for the cell reaction 2Ti_((S)) + Hg^(2+) (1M) rarr 2Ti^+ (1 M) + Hg_((I)) Where E_(Ti)^@ =- 0.34V, E_(Hg)^@ = 0.86 V is

Given, the standard electrode potentials, `K^+//K = -2.93 V, Ag^+//Ag = 0.80 V, Hg^(2+)//Hg =0.79 V, Mg^(2+)//Mg = - 2.37 V, Cr^(3+)//Cr = - 0.74 V` Arrange these metals in their increasing order of reducing power.

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