rom a table of Standard Reduction Potentials:  Fe2+(aq) + 2 e- → Fe(s)         E = -0.447 V Cr3+(aq)  + 3 e-  → Cr(s)       E = -0.744 V   a) Which species gets oxidized?   b) What is the overall balanced reaction?   c) Calculate the cell potential E at 25°C for the reaction.   d) What is the cell potential at non-standard conditions given that [Fe2+] = 0.030 M, [Cr3+] = 0.40 M

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From a table of Standard Reduction Potentials: 

Fe2+(aq) + 2 e- → Fe(s)         E = -0.447 V

Cr3+(aq)  + 3 e-  → Cr(s)       E = -0.744 V

 

a) Which species gets oxidized?

 

b) What is the overall balanced reaction?

 

c) Calculate the cell potential E at 25°C for the reaction.

 

d) What is the cell potential at non-standard conditions given that [Fe2+] = 0.030 M, [Cr3+] = 0.40 M.

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