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

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.

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:

Using the standard electrode potentials given in Table 3.1 predict if the reaction between the following is feasible: Ag(s) and Fe ^(3+) (aq)

Using the standard electrode potentials given in Table 3.1 predict if the reaction between the following is feasible: Ag^+ (aq) and Cu(s)

Calculate the potential of the following cell reaction at 298K: Sn^(4+)(1.50M)+Zn(s)rarrSn^(2+)(0.5M)+zn^(2+)(2.0M) The standard potential of the cell is 0.89V, will the potential of the cell will increase or decrease if the concentration of Sn^(2+) is increased in the cell?

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

When the silver electrode having reduction potential 0.80V is attached to NHE, will it act as anode or cathode?