The standard oxidation potential of `Zn` referred to SHE is 0.76 V and that of Cu is `-0.34V` at `25^(@)C` when excess of `Zn` is added to `CuSO_(4)`, Zn displaces `Cu^(2+)` till equilibrium is reached. What is the approx ratio of `Zn^(2+)` to `Cu^(2+)` ios at equilibrium?

The standard oxidation potential of Zn referred to SHE is 0.76V and that of Cu is -0.34V at 25^(@)C . When excess of Zn is added to CuSO_(4),Zn diplaces Cu^(2+) till equilibrium is reached. What is the ratio of Zn^(2+) to Cu^(2+) ions at equilibrium?

The standard oxidation potential of Zn referred to SHE is 0.76V and that of Cu is -0.34V at 25^(@)C . When excess of Zn is added to CuSO_(4),Zn diplaces Cu^(2+) till equilibrium is reached. What is the ratio of Zn^(2+) to Cu^(2+) ions at equilibrium?

The standard reduction potential of Zn is -0.76V and that of Cu is +0.34V . What do they indicate?

The normal oxidation potential of zinc referred to the standard hydrogen electrode is 0.76 volt and that of copper is -0.34 volt at 25^(@)C . When excess of zinc is added to a solution of copper sulphate the zinc displace copper till equilibrium is reached. What is the ratio of concentration of Zn^(2+) to Cu^(2+) ions at equilibrium ?

The e.m.f of galvanic cell , with oxidation potentials of Zn = +0.76 V and that of Cu = -0.34 V , is ________.