Galvanic or Voltaic Cells - Introduction

Galvanic or a voltaic cell converts the chemical energy liberated during a redox reaction to ____________.

Standard electrode potential is measured taking the concentrations of all the species involved in a half-cell is ____________.

Standard hydrogen electrode operated under standard conditions of 1 atm H₂ pressure, 298 K, and pH = 0 has a cell potential of ____________.

Calculate emf of the following cell at 25°C:

Sn | Sn²⁺ (0.001 M) || H⁺ (0.01 M) | H₂ (g) (1 bar) | Pt (s)

`E_(Sn^(2+)"/"Sn)^0=-0.14V " " E_((H^+"/"H_2))^0=0.00V`

Calculate e.m.f. and ∆G for the following cell:

Mg (s) |Mg²⁺ (0.001M) || Cu²⁺ (0.0001M) | Cu (s)

`"Given :" E_((Mg^(2+)"/"Mg))^0=−2.37 V, E_((Cu^(2+)"/"Cu))^0=+0.34 V.`

Calculate the emf of the following cell at 25°C :

Depict the galvanic cell in which the reaction Zn(s) + 2Ag⁺(aq) → Zn²⁺(aq) + 2Ag(s) takes place. Further show:

(i) Which of the electrode is negatively charged?

(ii) The carriers of the current in the cell.

(iii) Individual reaction at each electrode.

Given the standard electrode potentials,

K⁺/K = −2.93V, Ag⁺/Ag = 0.80V,

Hg²⁺/Hg = 0.79V

Mg²⁺/Mg = −2.37 V, Cr³⁺/Cr = − 0.74V

Arrange these metals in their increasing order of reducing power.