Which of the following redox couple is stronger oxidizing agent ?
a. `Cl_2 (E^0 = 1.36 V)` and `Br_2 (E^0 = 1.09 V)`
b. `MnO_4^Theta (E^0 = 1.51 V)` and `Cr_2O_7^(2Theta) (E^0 = 1.33 V)`

Which of the following redox couple is stronger reducing agent ? a. Li (E^0 = -3.05 V) and Mg (E^0= -2.36 V) b. Zn (E^0 = -0.76 V) and Fe (E^0 = -0.44 V)

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

Predict whether the following reactions occur under standard state conditions: Oxidation of Ag_((s)) by Cl_(2(g)) E_(Ag)^@ = 0.8V'E_(C12)^@ = 1.36V

Which species in each of the following pairs is better oxidizing agent under standard state conditions ? (standard potentials are given). Give reasons for your answer :- CI_(2(g)) (1.36 V) or Cr_(aq)^(3+) (-0.74 V)

The E_(Ag)^@ = 0.80 V and E_(ceII)^@ = 1.20 V, for the cell. 2Ag^+ + Cd rarr 2 Ag + Cd^(2+) .The E_Cd^@ is

Which species in each of the following pairs is better oxidizing agent under standard state conditions (standard potentials are given)? Give reason for your answer: CI_2(g) (1.36V) or Cr_((aq))^(3+) (-0.74V)

Which species in each of the following pairs is better oxidizing agent under standard state conditions ? (standard potentials are given). Give reasons for your answer:- Br_(2(I)) (1.09V), or Au^(3+) (1.4V)

Which species in each of the following pairs is better reducing agent under standard state conditions. E^@ values are, given. Give reasons for your answer :- Co_(aq)^(2+) (1.81 V) or In_(s) (-0.14 V)

Which species in each of the following pairs is better oxidizing agent under standard state conditions (standard potentials are given)? Give reason for your answer. Br_(2(I)) (1.09 V) or Au_(aq)^(3+) (1.49 V)

Which species in each of the following pairs is better reducing agent under standard state conditions? E^@ values are given.Give reasons for your answer: Ce_((aq))^(3+) (1.61V) or Ti_((aq))^(2+) (-0.37V)