Question 14 of 20 Map oo Sapling Learning macmilan learning Calculate the cell p

Question

Question 14 of 20 Map oo Sapling Learning macmilan learning Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Mg2+] = 0.878 M and [Fe2+ 0.01 10 M. Standard reduction potentials can be found here Mg(s) + Fe2+(aq) Mg2+(aq) + Fe(s) Number Previous Give Up & View Solution e Check Answer Next Exit Use the Nemst equation RTIn where E is the cell potential, E° is the standard cell potential, R is the gas contant (8.3145 J(mol K)), Tis the Kelvin temperature, n is the number of electrons transferred, F is the Faraday constant (96485 J/(V mol)), and Q is the reaction quotient (product concentrations over reactant concentrations) Note that n is symbolized as Ve or z in some textbooks.

Explanation / Answer

E0cell   = Eright - Eleft

E0cell   = - 0.44 - (-2.36)

E0cell    = 1.92

E = E0  - RT /nF ln (Q)

if we substitute R , T and F then equation becomes as follows

E = E0  - 0.059 /2 log [Mg+2] /[Fe+2]

E = 1.92 - 0.0295 log [0.878] /[0.011]

E = 1.92 - 0.056

E = 1.864 V

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