An electrochemical cell has both a silver anode and a silver cathode. The soluti

Question

An electrochemical cell has both a silver anode and a silver cathode. The solutions of silver nitrate in contact with the electrodes have different concentrations. Which statement(s) correctly describe this cell? I. The cell potential is 0. II. The cell potential is negative. III. The cell potential is positive. IV. No electrons will flow through the external circuit. (a) I only (b) II only (c) III only (d) I and IV (e) II and IV When a voltaic cell reaches equilibrium, _____ (a) E degree _cell = 0. (b) E_cell = 0. (c) E_cell = K. (d) E degree _cell = K. (e) E_cell = Q. Calculate the equilibrium constant for the oxidation of bromine by ozone at 298 K. O_3 (g) + 2 H^+ (aq) + 2 e^- rightarrow H_2 O (l) E degree = +2.08 V BrO_3^- (g) + 6H^+ (aq) + 5e^- rightarrow 1/2 Br_2 (s) + 3 H_2 O (l) E degree = +1.52 V (a) 2.88 times 10^9 (b) 3.47 times 10^-10 (c) 6.47 times 10^60 (d) 3.93 times 10^94 (e) 8.83

Explanation / Answer

(52) Since the electrodes are immersed in different concentrations of silver nitrate solutions. There should be the generation of potential. Hence,

(c) III. the cell potential is positive.

(53) when voltaic cell reaches equilibrium there is no change in the cell potential. SO, cell potential reaches to zero.

(b) Ecell = 0 at equilibrium

(54) E0cell = 2.08 - 1.52 = 0.56 V

relation between deltaG0 and E0cell and deltaG0 and K is as,

deltaG0 = - nFE0cell and deltaG0 = - RTlnK

So, R T lnK = n F E0cell

lnK = 10 * 96500 * 0.56 / (8.314 * 298)

lnK = 218.1

K = 5.24 * 1094

So, (d)

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