When a solution of `AgNO_3` (1 M) is electrolysed using platinum anode and copper cathode, what are the products obtained at two electrodes?
Given :`E_(cu^(2+)|cu)^(@)=+0.34 "volt", E_(O_2,H^+|H_2O)^(@)=+1.23"volt",E_(H^+|H_2)^(@)=+0.0"volt" E_(ag^+|Ag)^(@)=+0.8 "volt"`

When a solution of AgNO_3 (1 M) is electrolysed using platinum anode and copper cathode, what are the products obtained at two electrodes? Given : E_(cu^(2+)|cu)^(@)=+0.34 V , E_(H_2O|O_2,H^+)^(@)=-1.23 V E_(H^+|H_2)^(@)=+0.0V , E_(ag^+|Ag)^(@)=+0.8 V

When a solution of AgNO_3 (1 M) is electrolysed using Pt anode and Cu cathode, the products at two electrodes are? E_(cu^(2+)|cu)^(@)=+0.34 "V" , E_(O_2,H^+|H_2O)^(@)=+1.23"V",E_(ag^+|Ag)^(@)=+0.8 "V"

Can a solution of 1 M copper sulphate be stored in a vessel made of nickel metal? Given that E_(Ni^(+2)//Ni)^(@)=0.25 " volt and "E_(Cu^(+2)//Cu)^(@)=+0.34" volt" .

Can a solution of 1 M copper sulphate be stored in a vessel made of nickel metal ? Given that E_(Ni^(+2)//Ni)^(@)=-0.25 volt and E_(Cu^(+2)//Cu)^(@) =+0.34 volt

Copper reduces NO_3^(-) into NO_2 depending upon concentration of HNO_3 in solution Assuming [Cu^(2+)]=0.1M, "and" P_(NO)=P_(NO_2)=10^(-3) bar, at which concentration of HNO_3 , Thermodynamic tendency for reduction of NO_3^(-) into NO and NO_2 by copper is same ? Given: E_(cu^(2+)|cu)^(@)=+0.34 "volt", E_(NO_3^(-)|NO)^(@)=+0.96 "volt",E_(NO_3^(-)|NO_(2))^(@)=+0.76 "volt"]

Can we use a copper vessel to store 1 M AgNO3 solution? Given that E_(Cu^(2+)| Cu )^(0) = + 0.34 volt and E_(Ag^(+)| Ag )^(0) = 0.80 volt