The standard reduction potentials for the following half-reactions are given as:

Question

The standard reduction potentials for the following half-reactions are given as: Cr^+3 + 3e^- rightarrow Cr Edegree = -0.73 V Br_2 + 2e^- rightarrow 2Br^- Edegree = +1.09 V What is the Edegree for this galvanic cell? a. 1.82 V b. 0.36 V c. 4.75 V d. 1.79 V e. 0.72 V 28. In the cell shown, which reaction occurs at the cathode? Cu(s)|Cu^2+(aq)||Ag^+(aq)|Ag(s) a. Cu^2+(aq) + 2 e^- rightarrow Cu(s) b. Ag(s) rightarrow Ag^+(aq) + e^- c. Ag^+(aq) + e^- rightarrow Ag(s) d. Cu(s) rightarrow Cu2^+(aq) + 2 e^- e. None of the above 29. Consider the following standard reduction potentials in acid solution: Cr^3+ + 3e^- rightarrow Cr Edegree = -0.74 V Co^2+ + 2e^- rightarrow Co Edegree = -0.28 V MnO_4^- + 8H^+ + 5e^- rightarrow Mn^2+ + 4H_2O Edegree = +1.51 V The strongest oxidizing agent listed above is a. Cr^3+ b. Cr c. Mn^2+ d. Co^2+ e. MnO_4^- 30. What is the value of DeltaGdegree at 298K for the following reaction? Pb(s) + 2 H^+(aq) rightarrow Pb^2+(aq) + H_2(g) Edegree = 0.13 V a. 12 KJ b. -25000 KJ c. 25 kJ d. -25 kJ e. 39 KJ 31. What mass in grams of copper will be deposited from a solution of Cu^2+ by a current of 2.50 A in 2.00 hr? a. 11.9 b. 5.93 c. 23.7 d. 1.65 e. 5.00

Explanation / Answer

27. E0cell = Ec - Ea

   = 1.09 - -0.73

    = 1.82

answer: 1.82 V

28. answer: b

29. higher the reduction potential,stronger the oxidising agent nature.

answer: e

30. DG0 = - nFE0cell
  

      = -2*96500*0.13

     = -25090 joule

   answer : d - 25kj

31. w = zit

   w = ((63.54/2)/96500)*2.5*2*60*60

   w = 5.93 grams

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