Given the following standard reduction potentials. Fe^2+ (aq) + 2 e rightarrow F

Question

Given the following standard reduction potentials. Fe^2+ (aq) + 2 e rightarrow Fe(s0 E degree = - 0.42 V Cr^3+(aq) + 3 e rightarrow Cr(s) E degree = - 0.74 v (a) What is the cell potential by combining the above two half-reactions to make a galvanic cell)? (b) Which species will be oxidized in anode? Write the half-reaction for the anode (c) Write the overall reaction for this working voltaic cell. (d) If (Fe^2+] E-cell^degree = 1.0 M and [Cr^3+] = 0.10 M, the cell potential E should be i) E E_cell degree iv0 none of above

Explanation / Answer

5. Higher the standard reduction potential more is the ability to get reduce. As E° of fe2+/fe>E° of Cr3+/Cr

So Fe electrode would act as cathode while Cr electrode would act as anode.

a) E° cell=E° cathode - E° anode= -0.42-(-0.74)=0.32 volts

b) Cr

Cr=cr3++3e

c) overall reaction

2Cr+3fe2+=2Cr3++3Fe

d) E>E° using nernst equation

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