A substance that will reduce Ag to Ag bu...

A substance that will reduce Ag to Ag but will not reduce`Ni^(2+)` to Ni is : `(E_(Ag^(+)//Ag)^(0))=0.80 V, E_(Ni^(2+)//Ni)^(0)`

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An aqueous solution containing 1M each of Au^(3+), Cu^(2+), Ag^(+), Li^(+) is being electrolysed by using inert electrodes. The value of standard potentials are E_(Ag^(+)//Ag)^(@)= 0.80V, E_(Cu^(2+)//Cu)^(@) = 0.34V, and E_(Au^(3+)//Au)^(@) = 1.50 V , E_(Li^(+)//Li)^(@)= -3.03V , With increasing voltage, the sequence of deposition of metals on the cathode will be

At equimolar concentration of Fe^(2+) and Fe^(3+) what must [Ag^(+)] be so that the voltage of the galvanic cell made from Ag^(+)//Ag and Fe^(3+)//Fe^(2+) electrodes equals zero? The reaction is Fe^(2+) + Ag^(+) hArr Fe^(3+) + Ag . Determine the equilibrium constant at 25^(@)C for the reaction. Given E_(Ag^(+)//Ag)^(@)= 0.799V and E_(Fe//Fe^(2+))^(@)= 0.771V

Calculate the emf of the cell at 298K E_(NI^(2+)//NI)^0 is -0.25V and E_(Ag^+//Ag)^0 is +0.80V .

Emf of the cell Ni|Ni^(2+) (0.1M)||Au^(3+) (1.0M)|Au will be (Given E_(Ni^(2+)//Ni)^(@)= 0.25V, E_(Au^(2+)//Au)^(@)= 1.5V )

Will Mg reduce CuSO_4 ? E_(Mg,Mg^(2+))^@=+2.36V and E_(Cu,Cu^(2+))^@=0.34V

Assertion : (Ni)|(Ni^(2+))(1.0M)|| Au^(3+)(l.0M)|Au for this cell emf is 1.75 V, if E_(Au^(3+)//Au)^(@) =1.50 and E_(Ni^(2+)) // Ni^(@)=0.25 V Reason: Emf of the cell = E_(cathode)^(@)-E_(anode)^(@)

Calculate the reduction potentials for the following half cells: Ag|Ag^+ (10^-5 M),E_(Ag^+,Ag)^@=0.80V

Tollen's reagent is used for the detection of aldehyde when a solution of AgNO_(3) is added to glucose with NH_(4)OH then gluconic acid is formed Ag^(+) + e^(-) rarr Ag , E_("red")^(@)= 0.8V C_(6)H_(12)O_(6) + e^(-) rarr C_(6)H_(12) O_(7) (Gluconic acid) +2H^(+) + 2e^(-) , E_("red")^(@)= -0.05V Ag(NH_(3))_(2)^(+) + e^(-) rarr Ag(s) + 2NH_(3) , E^(@)= -0.337V [Use 2.303 xx (RT)/(F)= 0.0592 and (F)/(RT)= 38.92 at 298K] When ammonia is added to the solution, pH is raised to 11. Which half-cell reaction is affected by pH and by how much ?

Tollen's reagent is used for the detection of aldehyde when a solution of AgNO_(3) is added to glucose with NH_(4)OH then gluconic acid is formed Ag^(+) + e^(-) rarr Ag , E_("red")^(@)= 0.8V C_(6)H_(12)O_(6) + e^(-) rarr C_(6)H_(12) O_(7) (Gluconic acid) +2H^(+) + 2e^(-) , E_("red")^(@)= -0.05V Ag(NH_(3))_(2)^(+) + e^(-) rarr Ag(s) + 2NH_(3) , E^(@)= -0.337V [Use 2.303 xx (RT)/(F)= 0.0592 and (F)/(RT)= 38.92 at 298K] Ammonia is always added in this reaction. Which of the following must be incorrect ?

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