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.

How can you increase the reduction potential of an electrode?

What is the effect of increased and decreased solute concentration on water potential inside the cells?

What effect does the concentration of H^+ (aq) ions have on the nature of the solution?

A copper silver cell is set up. The copper ion concentration is 0.10M . The concentration of silver ion is not known. The cell potential when measured was 0.422V. Determine the concentration of silver ions in the cell. (Given) E_(Ag^(2+)//Ag)^@=+0.80V,E_(Cu^(2+)//Cu)^@=+0.34V

. A wire is replaced by another wire of same length and material but of twice diameter. (/) What will be the effect on the increase in its length under a given load? (//) What will be the effect on the maximum load which it can bear?

The K.E. of an electron which is accelerated in a potential difference of 100V is

When a metal rod C in dipped in an aquos soluion of a metal D (having conentration 1M for D^(2+) ion) at 25^@C the standard electrode potential are C^(2+)//C=-0.76 volts. D^(2+)D=+0.34 volts .

Represent the cell with cell reaction- Zn(s)+2Ag^+(aq) rarr Zn^(2+) (aq)+2Ag(s) Calculate the emf of the cell at 298K if the molar concentraction of Ag^+ and Zn^(2+) ions in the half cwells are 0.10 mol dm^(-3) and 0.01 mol dm^(-3) respectively. Given that E^@ Ag^+//Ag= 0.80V and E^@Zn^(2+)//Zn=-0.76V,

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)