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Chapter 18 Bank
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  Chapter 21: ElectrochemistryPage 1 CHAPTER 21ELECTROCHEMISTRY 21-1.Consider an electrochemical cell formed from a Cu(s) electrode submerged in an aqueous Cu(NO 3 ) 2  solutionand a Cd(s) electrode submerged in a Cd(NO 3 ) 2 (aq) solution. The two electrodes are connected by a wire andthe two solutions are connected by a salt bridge containing NaNO 3 (aq). The following reaction takes place:Cu 2+ (aq) + Cd(s) →  Cu(s) + Cd 2+ (aq)Which statement describes how the electrons or nitrate ions will flow?(a) electrons will flow from Cu(s) to Cd(s)(b) nitrate ions will flow from Cu compartment to Cd compartment(c) nitrate ions will not flow between compartments(d) nitrate ions will flow from Cd compartment to Cd compartment21-2. Consider an electrochemical cell formed from a Cu(s) electrode submerged in an aqueous Cu(NO 3 ) 2  solutionand a Cd(s) electrode submerged in a Cd(NO 3 ) 2  solution. The two electrodes are connected by a wire and thetwo solutions are connected by a salt bridge containing NaNO 3 (aq). The following reaction takes place:Cu 2+ (aq) + Cd(s) →  Cu(s) + Cd 2+ (aq)Which statement describes how the electrons or nitrate ions will flow?(a) electrons will flow from Cu(s) to Cd(s)(b) electrons will flow from Cd(s) to Cu(s)(c) electrons will not flow between electrodes(d) nitrate ions will flow from Cd compartment to Cd compartment21-3. Consider an electrochemical cell where the following reaction takes place:2 Au 3+ (aq) + 3 Zn(s) →  2 Au(s) + 3 Zn 2+ (aq)Which of the following is the correct cell notation for this cell?(a) Au | Au 3+  || Zn 2+  | Zn(b) Au 3+  | Au || Zn | Zn 2+ (c) Zn | Zn 2+  || Au 3+  | Au(d) Zn | Au 3+  || Au | Zn 2+ NOTE: for spring 2001 ignore questions with an underlined number. Revised: February 2001  Chapter 21: ElectrochemistryPage 221-4. Consider an electrochemical cell where the following reaction takes place:3 Sn 2+ (aq) + 2 Al(s) →  3 Sn(s) + 2 Al 3+ (aq)Which of the following is the correct cell notation for this cell?(a) Al | Al 3+  || Sn 2+  | Sn(b) Al 3+  | Al || Sn | Sn 2+ (c) Sn | Sn 2+  || Al 3+  | Al(d) Sn | Al 3+  || Al | Sn 2+ 21-5.E o  for the following redox reaction is +1.05 V.2 Ag + (aq) + Ni(s) →  2 Ag(s) + Ni 2+ (aq)What is ∆ G o  for this reaction?(a) +203 kJ(b) -203 kJ(c) +101 kJ(d) -101 kJ21-6.E o  for the following redox reaction is -0.029 V.Fe 3+ (aq) + 3 Ag(s) →  Fe 2+ (aq) + 3 Ag + (aq)What is ∆ G o  for this reaction?(a) +2.8 kJ(b) -2.8 kJ(c) +8.4 kJ(d) -8.4 kJ21-7.An early method of producing aluminum metal was the reaction of aluminum salts with sodium metal:Al 3+  + 3 Na(s) →  Al(s) + 3 Na +  E o = +1.05 VWhat is ∆ G o  for this reaction?(a) -304 kJ(b) +101 kJ(c) -101 kJ(d) +304 kJ21-8.The following redox reaction can be used to form iodine.Br 2 (aq) + 2 I - (aq) →  2 Br - (aq) + I 2 (aq) ∆ G o = -105 kJWhat is E o  for this reaction?(a) +1.09 V(b) -1.09 V(c) +0.0011 V(d) +0.545 V Revised: February 2001  Chapter 21: ElectrochemistryPage 321-9.The following reaction can be used to form bromine.Cl 2 (aq) + 2 Br - (aq) →  2 Cl - (aq) + Br 2 (aq) ∆ G o = -102 kJ(a) +1.06 V(b) -1.06 V(c) +0.53 V(d) -0.53 V21-10.It would be useful if a battery could be made utilizing the following reaction:2 Li(s) + F 2 (g) →  2 LiF(s) ∆ G o = -1141 kJWhat is E o  for this reaction?(a) +11.8 V(b) -11.8 V(c) +2.7 V(d) +5.9 V21-11.Given the two following half reactions,Ni 2+ (aq) + 2e -   →  Ni(s) E o = -0.25 VHg 2+ (aq) + 2e -   →  Hg( l ) E o = +0.86 Vcalculate E o  for the following reaction:Hg 2+ (aq) + Ni(s) →  Ni 2+ (aq) + Hg( l )(a) -1.11 V(b) +0.61 V(c) +1.11 V(d) -0.61 V21-12.Given the two following half reactions,Cu 2+ (aq) + 2e -   →  Cu(s) E o = +0.34 VHg 2+ (aq) + 2e -   →  Hg( l ) E o = +0.86 Vcalculate E o  for the following reaction:Hg 2+ (aq) + Cu(s) →  Cu 2+ (aq) + Hg( l )(a) -1.20 V(b) +0.52 V(c) +1.20 V(d) -0.52 V Revised: February 2001  Chapter 21: ElectrochemistryPage 421-13.Given the two following half reactions,Mg 2+ (aq) + 2e -   →  Mg(s) E o = -2.37 VI 2 (aq) + 2e -   →  2 I - (aq) E o = +0.54 Vcalculate E o  for the following reaction:Mg 2+ (aq) + 2 I - (aq) →  I 2 (aq) + Mg(s)(a) -2.91 V(b) -1.83 V(c) +1.83 V(d) -2.91 V21-14.Given the two following half reactions,Sn 2+ (aq) + 2e -   →  Sn(s) E o = -0.14 VSn 4+ (aq) + 2e -   →  Sn 2+ (aq) E o = +0.15 Vcalculate E o  for the following reaction:Sn 4+ (aq) + Sn(s) →  2 Sn 2+ (aq)(a) -0.01 V(b) -0.29 V(c) +0.29 V(d) +0.01 V21-15.An electrochemical cell of notation Pd | Pd 2+  || Cu 2+  | Cu has E o = -0.65 V. If we know that the standardreduction potential of Cu 2+  /Cu is E o = 0.34 V, what is the standard reduction potential for Pd 2+  /Pd?(a) -0.99 V(b) -0.31 V(c) +0.31 V(d) +0.99 V21-16.An electrochemical cell of notation Pt | Pt 2+  || Ni 2+  | Ni has E o = -1.45 V. If we know that the standardreduction potential of Ni 2+  /Ni is E o = -0.25 V, what is the standard reduction potential for Pt 2+  /Pt?(a) +1.70 V(b) -1.20 V(c) +1.20 V(d) -1.70 V21-17.Given the following two half reactions,Cd 2+ (aq) + 2e -   →  Cd(s) E o = -0.40 VZr 4+ (aq) + 4e -   →  Zr(s) E o = -1.53 Vdetermine E o  and the spontaneity of the following reaction2 Cd 2+ (aq) + Zr(s) →  2 Cd(s) + Zr 4+ (aq)(a) +1.13 V and not spontaneous(b) +1.13 V and spontaneous(c) -1.13 V and not spontaneous(d) -1.13 V and spontaneous Revised: February 2001

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