Calculate the cell potential for the following reaction as written at 25.00 °C,

Question

Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Mg2 ] = 0.886 M and [Fe2 ] = 0.0160 M. Standard reduction potentials can be found here.

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Question 4 of 12 Incorrect Incorrect Mapoob Map ddo sapling learning Calculate the cell potential for the following reaction as written at 25.00 , given that [Mg21 = 0.886 M and [Fe21 0.0160 M. Standard reduction potentials can be found here. Mg(s)+Fe2+(aq) Mg2+(aq)+ Fe(s) Number E= 1.8016 | V

Explanation / Answer

Mg2+(aq) + 2e- -> Mg(s)    Eo= -2.38V reversing the reaction Mg (s) ---> Mg+2 +2e- Eo=2.38V (1)

Fe2+(aq) + 2e- -> Fe(s)   Eo= -0.41V (2)

Addiing Eq.1 and 2 gives the required equation Mg+Fe+2---> Mg+2 +Fe, Eo= 2.38-0.41=1.97 V

E= Eo-0.0591/2 * logQ

Q= [Mg+2]/[Fe+2] =0.886/0.016=55.375, logQ= 1.74

E= 1.97-0.0591/2*1.74=1.92 V

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