Given the standard electrode potentials: K^+/K=-2.93V . Ag^+/Ag=0.80V',Arrange these metals in their increasing order of reducing power.
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)
Tarnished silver contains Ag_2S . Can this tranish be removed by placing tranished silver articels in an aluminium pan containing an inert electrolyte solution such as NaCl? The standard electrode potentials for the half cell reactions are: Ag_2S(s)+2barerarr2Ag(s)+S^(2-)(aq) , E^@=-0.71V and Al^(3+)+3barerarrAl(s) , E^@=-1.66V .
The standard reduction potentials for two reactions are given below: AgCl(s)+barerarrAg(s)+Cl^(-)(aq) , E^@=0.22V and Ag^(+)(aq)+barerarrAg(s) , E^@=0.80V The K_(sp) of AgCl under standard conditions of temperature is given by
Is Ag(At. No. 47) a transition metal. Explain. Why ?
In a saturated solution of AgCl, NaCl is added gradually. The concentration of Ag^(+) is plotted against the concentration of Cl^(-) . The graph appears as :
The e.m.f of the cell: Cu(s)|Cu^(2+)(1M)||Ag^(+)(1M)|Ag is 0.46V. The standard reductio potential of Ag^+|Ag is 0.80V. The standard reduction potential of Cu^(2+)|Cu is
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.
Calculate the standard cell potentials of galvanic cell in which the following reactions take place: Calculate the Delta_rG^o and equilibrium constant of the reactions. Fe^(2+)(aq) + Ag^+ (aq) rarr Fe^(3+) (aq) + Ag(s)
