Question

Nernst equation for the following cell reaction at 298 K is:

\[\ce{Mg_{(s)} | Mg^{2+}_{( aq)} || Ag^+_{( aq)} | Ag_{(s)}}\]

विकल्प

• E_cell = `"E"_"cell"^0 - 0.0592/2 log_10  (["Mg"^(2+)])/(["Ag"^+])`

• E_cell = `"E"_"cell"^0 - 0.0592/3 log_10  (["Mg"^(2+)])/(["Ag"^+]^2)`

• E_cell = `"E"_"cell"^0 - 0.0592/2 log_10  (["Mg"^(2+)])/(["Ag"^+]^2)`

• E_cell = `"E"_"cell"^0 - 0.0592 log_10  (["Mg"^(2+)])/(["Ag"^+]^2)`

Answer 1

E_cell = `"E"_"cell"^0 - 0.0592/2 log_10  (["Mg"^(2+)])/(["Ag"^+]^2)`