Calculate the equilibrium constant for this reaction at 25 degree C. Zn(s) + 2Ag

Question

Calculate the equilibrium constant for this reaction at 25 degree C. Zn(s) + 2Ag^+ (aq) rightarrow Zn^2+ (aq) + 2Ag(s) (A)2 times 10^1 (B) 2 times 10^26 (C) 5 times 10^52 (D) 5 times 10^79 Chlorine will oxidize I^- as shown in this equation: Cl_2 + 2I^- rightarrow I_2 + 2CI^- Use reactivity trends to predict which can be used to prepare Br_2 from Br^-. I. F_2 + Br^- II. Cl_2 + Br^- III. I_2 + Br^- (A) I, II, and III (B) II and III only (C) III only (D) I and II only What is the oxidation number of chlorine in copper(II) chlorate, Cu(ClO_3)_2? (A) +10 (B) +5 (C) +4 (D) -1 Which statement about a galvanic cell is true? (A) Electrons flow from the anode to the cathode. (B) Oxidation occurs at the cathode. (C) The cell reaction is nonspontaneous. (D) Electrons are transferred through the salt bridge. Which substance is not a possible product in the combustion of a hydrocarbon? (A) CO (B) CO_2 (C) O_3 (D) H_2O

Explanation / Answer

Q57.

Find Keq for:

redox reaction

dG = -nF*E°

E° = Ereduction - Eoxidation

Ered = silver, Eox = zing

E° = 0.80 --0.76 = 1.56 V

n = 2 electrons transferred

dG = -2*96500*1.56 = -301080 J

now

dG = -RT*ln(K)

K = exp(-dG/(RT))

K = exp(301080/(8.314*298))

K = 5.976*10^52

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