From each of the pairs of substances choose the one that is the stronger oxidizi

Question

From each of the pairs of substances choose the one that is the stronger oxidizing agent. a. Cl_2 (g) or Br_2 (l) b. Zn^2+ (aq) or Cd^2+ (aq) b. Zn^2+ (aq) or Cd^2+ (aq) C. H_2 O_2 (aq) or O_3 (g) d. Cl^- (aq) or CIO_3^- (aq) Aqueous iodide ion is oxidized to I_2 (s) by Hg_2^2+ (aq) I^- (aq) rightarrow I_2 (s); Hg_2^2+ (aq) rightarrow Hg(l) a. write a balanced equation. b. calculate the standard emf, c. calculate Delta G degree at 298 K d. calculate the value of the equilibrium constant at 298 K A voltaic cell utilizes the following reaction and operates at 298 K: 3 Ce^4+ (aq) + Cr(s) rightarrow 3 Ce^3+ (aq) + Cr^3+ (aq) a. What is the emf of this cell under standard conditions? b. What is the emf of this cell when [Ce^4+] = 3.0 M, [Ce^3+] = 0.10 M, and [Cr^3+] = 0.010 M? c. What is the emf of the cell when [Ce^4+] = 0.010 M, [Ce^3+] = 2.0 M and [Cr^3+] = 1.5 M?

Explanation / Answer

Q4.

stronger oxidizing agent , will reduce itself, and favour oxidation of the other species

a.

Cl2, Br2, note that Cl2 is much mor electronagtive, so Cl is stronger

b.

Zn2+ + 2 e Zn(s) 0.7618

Cd2+ + 2 e Cd(s) 0.40

most negative will oxidize --> Zn

then, Cadmium will reduce, this is stronger reducing agent

c.

H2O2, O3

H2O2(aq) + 2 H+ + 2 e 2 H2O +1.78

O3(g) + 2 H+ + 2 e O2(g) + H2O +2.075

Clearly, O3 has a higher potential, so it will reduce first, i.e. it is stronger oxidizing agent

d)

Cl2(g) + 2 e 2 Cl +1.36

ClO3 + 2 H+ + e ClO2(g) + H2O +1.18

clearly, Cl2 is likely to from Cl-, therefore, Cl- is NOT our optio

choose ClO3-

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