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"]

Copper reduces NO_3^(-) into NO_2 depending upon concentration of HNO_

1.	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"]
Answer» `10^(1.23)M` `10^(0.56)M` `10^(0.66)M` `10^(0.12)M Answer :C