When the zinc electrode having electrode reduction potential -0.76V is attached to NHE, will it acts as anode or cathode?

How can you increase the reduction potential of an electrode?

What is the effect of an increase in concentration of Zinc ions on the electrode potential of Zinc electrode for which E^@ equals -0.76V.

What is the effect of an increase in concentration of zinc ions on the electrode potential of zinc electrode for which E^@ equals to -0.76V.

Calculate the electrode potential at a copper electrode dipped in 0.1 M solution of copper sulphate at 25^@C . Given, the standard emf of Cu^(2+) system is +0.34V at 298K.

Why it is not possible to measure the voltage of an isolated reduction half reaction or the potential of a single electrode?

One half-cell in a voltaic cell is constructed from a silver wire dipped in silver nitrate solution of unknonw concentration. It other half cell consists of a zinc electrode dipping in 1.0M solution of Zn(NO_3)_2 . A voltage of 1.48V is measure for this cell. Use this information to calculate the concentration of silver nitrate solution used (E_(Zn^(2+)//Zn)^0=-0.76V,E_(Ag^+//Ag)^0=+0.80V)

Calculate the electrode potential of a copper electrode dipped in 0.1M solution of copper sulphate at 25^@C . (Given E^@ for Cu is +0.34V at 298K)

Calculate the equilibrium constant for the reaction. 2Fe^(3+)+3I^-harr2Fe^2+I_3^- The standary reduction potentials in acidic conditions are 0.77V and 0.54V respectively for Fe^(3+)//Fe^(2+) and I_3^-//I^- couples.

The standard electrode potential for Daniel cell is 1.1V. Calculate the standard Gibb's energy for the reaction. Zn_(s)+ Cu_(aq)^(2+) rarr Zn_(aq)^(2+)+Cu_(s) .