Copper reduces `NO_3^(-)` into `NO_2` depending upon concentration of `HNO_3` in solution Assuming `[Cu^(2+)]=0.1M, "and&qu

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"]`
A. `10^(1.23)M`
B. `10^(0.56)M`
C. `10^(0.66)M`
D. `10^(0.12)M

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

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