The reduction potential values are given below
`AI^(3_)//AI =- 1.67 "volt" Mg^(2+)//Mg =- 2.34 "volt" Cu^(2+)//Cu = +0.34` volt
`I_(2)//2I^(-) = +0.53` volt. Which one is the best reducing agenet?

The reduction potential values are given below Al^(3_)//Al =- 1.67 "volt" Mg^(2+)//Mg =- 2.34 "volt" Cu^(2+)//Cu = +0.34 volt I_(2)//2I^(-) = +0.53 volt. Which one is the best reducing agent?

The reduction potential velues are given below Al^(3+)//Al=-1.67"volt", Mg^(2+)//Mg=-2.34"molt", Cu^(2+)//Cu=+0.34"volt" I_(2)//I^(-)=+0.53"volt" . Which one is the best reducing agent?

A solution containing one mole per litre of each Cu(NO_(3))_(2), AgNO_(3), Hg_(2)(NO_(3))_(2) is being electrolysed by using inert electrodes. The values of standard electrode potentials in volts (reduction potentials) are Ag^(+)//Ag = +0.80 V, HG_(2)^(2+)//Hg = +0.79 V Cu^(+)//Cu = +0.34 V, Mg^(2+)//Mg = -2.37 V With increasing valtage, the sequence of deposition of metals on the cathode will be

An aqueous solution containing one mole per litre of each Cu(NO_3)_2 , AgNO_3 . Hg(NO_3)_(2), Mg(NO_3)_2 is being electrolysed using inert electrodes. The values of standard electrode potential (reduction potential) in volts are Ag//Ag^(+) = + 0.80 V " "Hg//Hg^(2+) = + 0.79V " " Cu//Cu^(2+) = +0.34 V " " Mg//Mg^(2+) = -2.37 V With increasing voltage, the sequence of deposition of metals on cathode will be

A solution containing one mole per litre of each Cu(NO_(3))_(2), AgNO_(3), Hg_(2)(NO_(3))_(2) and Mg(NO_(3))_(2) is being electrolysed by using electrode potential in volts ( reduction potentials) are Ag^(+)"|"Ag = + 0.80, Hg_(2)^(2+)"|" Hg = 0.79 . Cu^(2+) "|" Cu=0.34" and "Mg^(2+)"|"Mg= - 2.37 V. With increasing voltage, the sequence of deposition of metal on the cathode will be

Answer, whether under standard conditions, the following reactions are possible or not: (i) Will copper reduce Ag^(+) " to " Ag ? Given E_(Ag^(+)//Ag)^(@) = 0.799 " volt" , E_(Cu^(2+)//Cu)^(@) = - 0.337 volt (ii) Will Fe^(3+) be reduced to Fe^(2+) by Sn^(2+) ions? given {:(Fe^(3+) | Fe^(2+) = 0.771 " volt"),(Sn^(2+) |Sn^(4+) = - 0.250 " volt"):} (iii) would you use a silver spon to stir a solution of Cu(NO_(3))_(2) ?

Answer, whether under standard conditions, the following reactions are possible or not: (i) Will copper reduce Ag^(+) " to " Ag ? Given E_(Ag^(+)//Ag)^(@) = 0.799 " volt" , E_(Cu^(2+)//Cu)^(@) = - 0.337 volt (ii) Will Fe^(3+) be reduced to Fe^(2+) by Sn^(2+) ions? given {:(Fe^(3+) | Fe^(2+) = 0.771 " volt"),(Sn^(2+) |Sn^(4+) = - 0.250 " volt"):} (iii) would you use a silver spon to stir a solution of Cu(NO_(3))_(2) ?

E^(@) (SRP) of different half cell given {:(E_(Cu^(2+)//Cu)^(@) =0.34"volt",,,E_(Zn^(2+)//Zn)^(@) =- 0.76"volt"),(E_(Ag^(+)//Ag)^(@) = 0.8"volt",,,E_(Mg^(2+)//Mg)^(@) =- 2.37 "volt"):} In which cell Delta^(@) is most negative:-

E^(@) (SRP) of different half cell given {:(E_(Cu^(2+)//Cu)^(@) =0.34"volt",,,E_(Zn^(2+)//Zn)^(@) =- 0.76"volt"),(E_(Ag^(+)//Ag)^(@) = 0.8"volt",,,E_(Mg^(2+)//Mg)^(@) =- 2.37 "volt"):} In which cell Delta^(@) is most negative:-