Consult the table on standard electrode potentials and suggest three substance that can oxidise ferrous ions under suitable conditions.

Which defines the standard reduction electrode potential of Zn^(2+) ions?

Oxidation is de-electronation whereas reduction is electronation. Oxidants are the substances which oxidise others and reduced themselves. On the other hand reductants are the substances which reduce others and oxidised themselves. The oxidation number of an element in a compound decides its nature to act as oxidant or reductant. Oxidation-reduction occur simultaneously and the overall chemical change is called redox reaction. Redox reactions are of three types: (i) Intermolecular redox reactions, (ii) Autoredox or disproportionation reaction, and (iii) Intramolecular redox reactions. Select the species which can act as oxidant and reductant both : (1) H_2SO_3 (II) H_2 O_2 (III) O_3 (IV) HNO_3 (V) CI_2

The following statements about electro chemical series are i) the metals occupying top positions in the series do not liberate hydrogen with dilute acids ii) the substances which are stronger reducing agents and stronger oxidising agents are placed below & top respectively iii) a metal higher in the series will displace the metal from its solution which is lower in the series iv) various electrodes are arranged in a series in the descending order of their potentials The correct statements are The correct statements are

Using the standard electrode potentials given below identify the correct statement from the following . Fe ^(2)+2e^(-)rarrFe,E^(@)=-0.44V Cu ^(2+)+2e^(-)rarr Cu,E^(@)=-0.34V Ag ^(+)e^(-)rarr Ag,E^(@)=-0.80V (i) Copper can displace iron from FeSO_(4) solution . (ii) Iron c an displace copper from CuSO_(4) solution . (iv) Iron can displace silver from AgNO_(3) solution.

Nernst equation gives the variation of potential of an electrode based on activity of ions temperature and pressure. The equation is E=E^(@) -(2.303RT)/(nF) logQ (or) E=E^@ - (0.0591)/(n) log Q E^@ = Standard potential and 'Q' is the reaction quotient. What is the reduction potential of a hydrogen electrode in an aqueous solution containing 0.1 M NH_4OH,(Kb=10^(-5)) , ?

hydrogen-oxygen fuel cell may have an acidic or alkaline electrolyte. The half-cell reactions are To maximize the power per unit mass of an electrochemical cell, the electronic and electrolytic resistances of the cell must be minimized. Since fused salts have lower electrolytic resistances that aqueous solutions, high-temperature electrochemical cells are of special interest for practical applications. High temperature also allow the use of liquid metal electrode, which make possible higher current densities than solid electrodes For a Hydrogen-Oxygen fuel cell if DeltaH_(f)^(@)=(H_2O, l) = – 285 kJ //" mole" , then what will be its thermodynamic efficiency under standard conditions

Nernst equation gives the variation of potential of an electrode based on activity of ions temperature and pressure. The equation is E=E^(@) -(2.303RT)/(nF) logQ (or) E=E^@ - (0.0591)/(n) log Q E^@ = Standard potential and 'Q' is the reaction quotient. Which cell has least potential ?