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6.*Consider a voltaic cell constructed from a Fe electrode in 1.0 MFeCl2 and a Ni electrode in 1.0 M Ni(NO3)2, linked by an externalcircuit and a KCl salt bridge. Based on the reduction potentialsshown, which of the following statements is correct?
Fe2+ + 2 e- ----> Fe, Eo = -0.44 V;
Ni2+ + 2 e- ----> Ni(s), Eo = -0.25 V
Ans: B) Electrons flow from the iron electrode to the nickelelectrode.


7.*Given the following standard reduction potentials in acidsolution, which species is the strongest oxidizing agent?
Al3+ + 3 e- ----> Al Eo = -1.66 V;
Sn4+ + 2 e- ----> Sn2+ Eo = 0.14 V;
I2 + 2 e- ----> 2 I- Eo = 0.53 V
Ans: D) I2


8. *What is Keq for the reaction Mg(s) + Pb2+ ----> Mg2+ + Pb ata temperature of 25oC?
Pb2+ + 2 e- ----> Pb, Eo = -0.13 V;
Mg2+ + 2 e- ----> Mg, Eo = -2.37 V.
Ans: A) 6 x 1075



17*. Which of the following isotopes is most likely to be stableand why?
Ans: C) 38Ar



18*. An alkaline earth element is radioactive. It and its daughterelements decay by emitting three alpha particles in succession. Inwhat group of the preceding period on the periodic table will theproduct of this decay sequence be found?
Ans: C) Group IV


21*. A typical neutron-initiated fission of 235U yields 97Mo, twoneutrons, and an isotope of what element?
Ans: B) Sn


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28 Sep 2019

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Related questions


1)Calculate forthe electrochemical cell below,

Pb(s) |PbSO4(s) | Pb2+(aq) Ag+(aq) | Ag(s)

given the following standard reduction potentials.

Ag+(aq) + e- ->Ag(s) E° = +0.799 V

PbSO4(s)+ 2e- -> Pb(s) + SO4 2-(aq) E = -0.356 V

a) -1.954 V

b) -1.155 V

c) +0.443V

d) +1.155 V

2) Consider the following half- reactions:

Cu2+ (aq) + 2e- --> Cu(s)E = +0.34 V

Sn2+(aq) + 2e- --> Sn(s) E = -0.14 V

Fe2+(aq) +2e- --> Fe(s)E = -0.44 V

Al3+(aq) +3e- --> Al(s) E = -1.66 V

Mg2+(aq) + 2e---> Mg(s) E = -2.37 V

Which of the abovemetals or metal ions will reduce Fe2+ ?

a) Cu(s) andSn(s)

b) Cu2+(aq) andSn2+(aq)

c) Al3+(aq) andMg2+ (aq)

d) Al(s) andMg(s)

e) Sn(s) and Al3+(aq)

3) The following reaction occurs spontaneously

2H+ (aq) +Ca(s) --> Ca2+(aq) + H2(g)

Write a balanced recuction half-reaction-

a) 2H+(aq) + 2e --> H2(g)

b) 2H+ (aq) --> H2(g) + 2e-

c) H2(g) --> 2H+(aq) + 2e-

d) Ca(s) + 2e- --> Ca2+(aq)

e) Ca(s) --> Ca2+(aq) + 2e-

± Cell Potential and Equilibrium
18 of 28
Constants | Periodic Table
The equilibrium constant, K, for a redox reaction is related to the standard potential, E?, by the equation
lnK=nFE?RT
where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e?) , R (the gas constant) is equal to 8.314 J/(mol?K) , and T is the Kelvin temperature.
Standard reduction potentials
Reduction half-reaction E? (V)
Ag+(aq)+e??Ag(s) 0.80
Cu2+(aq)+2e??Cu(s) 0.34
Sn4+(aq)+4e??Sn(s) 0.15
2H+(aq)+2e??H2(g) 0
Ni2+(aq)+2e??Ni(s) ?0.26
Fe2+(aq)+2e??Fe(s) ?0.45
Zn2+(aq)+2e??Zn(s) ?0.76
Al3+(aq)+3e??Al(s) ?1.66
Mg2+(aq)+2e??Mg(s) ?2.37

Part A Part complete
Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 ?C) for the following reaction:
Fe(s)+Ni2+(aq)?Fe2+(aq)+Ni(s)
Express your answer numerically.
View Available Hint(s)
K = 2.68×10^6 Correct
When E?>0 and K>1 the reaction favors the products.

Part B
Calculate the standard cell potential (E?) for the reaction
X(s)+Y+(aq)?X+(aq)+Y(s)
if K = 7.87×10?3.

Express your answer to three significant figures and include the appropriate units.

E? = ?

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