In a particular redox reaction, MnO2 is oxidized to MnO4– and
Fe3 is reduced to Fe2 . Complete and balance the equation for this
reaction in acidic solution. Phases are optional.
Consider a galvanic cell based in the reaction Fe2+ +
Cr2O72- → Fe3+ +
Cr3+ in acidic solution. What is the coefficient of
Fe3+in the balanced equation?
Reference: Ref 18-2
Select one:
a.
3
b.
4
c.
none of these
d.
6
e.
2
Derive a balanced equation for the reaction occurring in the
cell:
Fe(s)|Fe2+(aq)||Fe3+(aq),Fe2+(aq)|Pt(s)
a.) If E?cell = 1.21 V, calculate ?G? for the
reaction.
b.) If E?cell=1.21V, calculate the equilibrium constant
for the reaction.
c.) Use the Nernst equation to determine the potential for the
cell:
Fe(s)|Fe2+(aq,1.0�10-3M)||Fe3+(aq,1.0�10-3M),Fe2+(aq,0.10M)|Pt(s)
Write an essay on the role of transition metals (Mg, Fe2+,Fe3+,
Cobalt, copper 1+ and 2+ and Zn2+) in biological systems. You
should discuss the properties of transition metals that make them
more or less suited to each specific role. You must include
examples of a metalloprotein specific to each role. You may use
diagrams to help illustrate your answer. You should consider the
redox properties of metals and Hard-Soft Acid-Base theory in your
answer and the way that ligands...
a. Write the balanced equation in ACID solution for the reaction below:
Fe2++MnO-4→Fe3++Mn2+
b. To standardize a potassium permanganate solution (purple in appearance), a 0.250 g sample of FAS (iron II ammonium sulfate hexahydrate; molar mass = 342 g/mol) is dissolved in 25.00 mL distilled water, then acidified with sulfuric acid. The solution is then titrated with 35.00 mL potassium permanganate solution from a buret until a pale persistent purple color is attained. Calculate the molarity of the potassium...
Calculate the equilibrium constant for the reaction
S2O82-(aq) + 2 Fe2+(aq)
--> 2 Fe3+(aq) + 2 SO42-(aq) at
25.0°C, given that the standard cells potentials for the two half
reactions at this temperature are
S2O82-(aq) + 2 e- 2
SO42-(aq) E = +2.08 V
Fe3+(aq) + e- Fe2+(aq) E
= +0.77 V
The equilibrium constant for the reaction, 2 Fe3+(aq)
+ Hg22+(aq) <=> 2 Fe2+(aq) + 2
Hg2+(aq) is 9.1 x 10-6(aq) at 298 K.
Calculate ΔG in J when
{Fe3+(aq)} = 0.725
{Hg22+(aq)} = 0.022
{Fe2+(aq)} = 0.033
{Hg2+(aq)} = 0.056
1) Calculate ΔG∞ for the electrochemical cell Pb(s) |
Pb2+(aq) || Fe3+(aq) | Fe2+(aq) |
Pt(s).
A. –1.2 x 102 kJ/mol
B. –1.7 x 102 kJ/mol
C. 1.7 x 102 kJ/mol
D. –8.7 x 101 kJ/mol
E. –3.2 x 105 kJ/mol
2)Determine the equilibrium constant (Keq) at 25∞C
for the reaction
Cl2(g) + 2Br– (aq)
2Cl– (aq) + Br2(l).
A. 1.5 x 10–10
B. 6.3 x 109
C. 1.3 x 1041
D. 8.1 x 104
E. 9.8