Consider the following Galvanic cell:-

By what value the cell voltage when concentration of ions in anodic and cathodic compartments both increased by factor of 10 at 298K:

Consider the following galvanic cell given below- Cu|Cu^(2+)||Cl^(-)|Cl_(2) , Pt. Write the reactions that occur at anode and cathode.

The Nernst equation: Consider the following galvanic cell Pb(s) | Pb^(2+)(aq.) || Ag^(2+)(aq.) | Ag(s) (a) What is the quantitative change in the cell voltage on increas-ing the ion concentrations in the anode compartment by a factor of 10 ? (b) What is the quantitative change in the cell voltage on increas-ing the ion concentration in the cathode compartment by a factor of 10 Strategy: The conventional notation of the cell tells us that lead is the anode while silve is the cathode. Therfore, the cell reaction is Pb(s) + 2Ag^(+)(aq.) rarr Pb^(2+)(aq.) + 2Ag(s) The cell potantial (at 25^(@)C ) is given by the Nernst equation, where n = 2 and Q = C_(Pb^(2+))//C_(Ag^(+)) : E_("cell") = E_("cell")^(@)-(0.0592 V)/(n) "logQ" E_("cell")^(@)-(0.0592 V)/(n) "logQ" C_(Pb^(2+))/C_(Ag^(+))^(2)

For the cell, Pb(s) |Pb^(2o+)(1M)||Ag^(o+)(1M) |Ag (s) , if concentraton of an ion in the anode compartment is increased by a factor of 10, the emf of the cell will

Write the Nernst equation for the cell reaction in the Daniel cell. How will the E_(cell) be affected when concentration of Zn^(2+) ion is increased?

Write the Nernst equation for the cell reaction in the Daniel cell. How will the E_("cell") be affected when concentration of Zn^(+) ions is increased?

Write the Nernst equation for the cell reaction in the Daniel cell. How will the E_("cell") be affected when concentration of Zn^(+) ions is increased?

Write the Nernst equation for the cell reaction in the Daniel cell. How will the E_("cell") be affected when concentration of Zn^(2+) ions is increased?