Item 12 Signed in as Item 12 Consider the reaction Learning Goal: To learn how t

Question

Item 12 Signed in as Item 12 Consider the reaction Learning Goal: To learn how to use the Nernst equation. Mg(s) + Fe2 + (aq)Mg2+ (aq) + Fe(s) g2+]= 0.310 M. at 45 °C, where [Fe2*) = 3.10 M and M The standard reduction potentials listed in any reference table are only valid at standard-state conditions of 25 C and 1 M. To calculate the cell potential at non-standard-state conditions, one uses the Nernst equation, Part A What is the value for the reaction quotient, Q. for the cell? Express your answer numerically. E=E", 2.303 RT E-Bo-2.303 RT log Q Q0.100 where E is the potential in volts, E° is the standard potential in volts R = 8.314 J / ( K . mol ) is the gas constant, T is the temperature in kelvins, rn is the number of moles of electrons transferred F-96, 500 C/(mol e-) is the Faraday constant, and Q is the reaction quotient Submit Hints My Answers Give Up Review Part Correct Part B What is the value for the temperature, T, in kelvins? Ask me anything

Explanation / Answer

Mg2+ (aq) + 2 e-   ---> Mg (s) E° = -2.36 V
Fe2+ (aq) + 2 e-    ---> Fe (s) E° = -0.44 V

Mg (s) --->Mg2+ (aq) + 2 e- E° = 2.36 V
Fe2+ (aq) + 2 e- --->Fe (s) E° = -0.44 V
Mg (s) + Fe2+ (aq) ---> Mg2+ (aq) + Fe (s)

E° cell 2.36 - 0.44 = 1.92 V

The standard cell potential is 1.92V

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