Part B. Determine the cell notation for the redox reaction given below. Pb(s) +

Question

Part B. Determine the cell notation for the redox reaction given below.
Pb(s) + 2 H+(aq) Pb2+(aq) + H2(g)

Part C. How many kilowatt-hours of electricity are used to produce 4.00 kg of magnesium in the electrolysis of molten MgCl2 with an applied emf of 5.00 V?

Part D. What is the reducing agent in the redox reaction represented by the following cell notation?
Mn(s) | Mn 2+(aq) || Ag+(aq) | Ag(s)

Part E. Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of Cr(OH)4- and ClO- in the balanced reaction?
Cr(OH)4-(aq) + ClO-(aq) CrO42-(aq) + Cl-(aq)

Explanation / Answer

1.

dG = -nF*E°cell ;

n = 2 electrons, F = 96500 C/mol

E°cell =Ered - Eox = 0.34 - -0.13 = 0.47

dG = -2*96500*0.47

dG = -90710 J/mol

b.

Pb oidizes --> goe in the anode

H reduces, --> goes in cathode

Pb(s) | Pb2+(aq) || H+(aq) H2(g) | Pt

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