Question

Write the Nernst Equation of the following cell and find the electromotive force of the cell at 25°C temperature —

Mg(s)।Mg^+2(0.001M)॥Cu^+2(0.01M)।Cu(s)

Given —

E^0Mg^+2/Mg = –2.36 volt, E^0Cu^+2/Cu = 0.34 volt​

Answer 1

Answer:

Explanation:

nernst eqn:

Ecell=E^0cell - {(0.0591/2)log(Mg^2+/Cu^2+)}

for EMF calculation

calculate E0cell via below eqn

E^0cell= E^0cathode - E^0 anode

here cathode is Cu^2+/Cu

      anode is Mg^2+/Mg

therefore E^0cell = 0.34--2.36 =+2.7

by putting the concentrations 0.001M and 0.01M of Mg^2+ and Cu^2+ respectively we get E^0cell or EMF =2.729 V