Give the standard electrode potentials: `Mg^2+ / Mg = -2.37 V,` `Cr^3+/Cr = - 0.74V`. Arrange these metals in their increasing order of reducing power.

Given the standard electrode potentials: K^+/K=-2.93V . Ag^+/Ag=0.80V',Arrange these metals in their increasing order of reducing power.

Arrange the metals Mg, Na, Ag, Cu, Fe, Zn in the increasing order of reactivity.

Given that the standard electrode potentials of metals are: K^+|K=-2.93V, Ag^+|Ag=0.80V, Cu^(2+)|Cu=0.34V, Mg^(2+)|Mg= -2.37V , Cr^(3+)/Cr=-0.74V Fe^(2+)|Fe=-0.44V . Arrange the metals in the increasing order of their reducing power.

The standard reduction potential of three metallic cations X, Y and Z are +0.52 , -3.03 and -1.18 v respectively. The order of reducing power is:

E^@ of three metals A, B, C are -1.4 V, + 0.6V, - 3.4V respectively. The reducing power of these metals are in order :

The following chemical Feaction is occurring in an electrochemical cell. Mg(s) + 2 Ag^(+) (0.0001 M)rarr Mg^(2+) (0.10 M) + 2 Ag (s) The E^@ electrode values are Mg^(2+)//Mg = -2.36 V Ag^(+)//Ag = 0.81 V For this cell, calculate/write : (i)Symbolic representation of the above cell. (ii) Will the above cell reaction be spontaneous?

Using the standard electrode potentials given in Table 3.1 predict if the reaction between the following is feasible: Br_2 (aq) and Fe^(2+) (aq) .

K, Ca and Li metals may be arranged in the decreasing order of their standard electrode potentials as

What is the oxidation state of Cr in K_(2)Cr0_(3)