Determine the equilibrium constant (K_eq) at 25 degree C for the reaction. Cl_2(

Question

Determine the equilibrium constant (K_eq) at 25 degree C for the reaction. Cl_2(g) + 2 Br^-_(aq) Equilibrium 2Cl^- + Br_2(l) Cl_2(g) + 2e^- rightarrow 2Cl^-_(aq) E degree = +1.36V Br_2(l) + 2e^- rightarrow 2Br^-_(aq) E degree = +1.09V 1.5 times 10^-10 6.3 times 10^9 1.3 times 10^9 8.1 times 10^4 9.8 Calculate Delta G degree for the electrochemical cell Fe_(s) | Fe^2+_(aq) || Sn^4+_(aq) |Sn^2+_(aq) |Pt(s) -5.5 times 10^1 KJ/mol -1.2 times 10^2 KJ/mol 6.0 times 10^1 KJ/mol 1.1 times 10^5 KJ/mol 1.2 times 10^2 KJ/mol Calculate the cell EMF for the following reaction at 25 degree C: Ni_(s) + 2Cu^2+(0.010M) rightarrow Ni^2+(0.0010M) + 2Cu^+(1.0M) 0.40V -0.43V 0.43V 0.34V 0.36V

Explanation / Answer

(8) E0cell = 1.36 - 1.09 = 0.27 V

deltaG0 = - n F E0cell and deltaG0 = - R T lnK

SO,

lnK = n F E0cell / R T
lnK = 2 * 96500 * 0.27 / (8.314 * 298)

K = e21.0

K = 1.3 * 109

(C)

(9)

E0cell = E0Sn4+/Sn2+ - E0Fe2+/Fe = 0.151 - ( - 0.447 ) = 0.598 V

deltaG0 = - n F E0cell = - 2 * 96500 * 0.598 = - 1.15 * 105 J/mol = - 1.2 * 102 kJ/mol

(B)

(10)

E0cell = E0Cu2+/Cu+ - E0Ni2+/Ni = + 0.153 - ( - 0.257 ) = 0.410 V

Applying Nernst equation for the cell reaction,

Ecell = E0cell - (0.0591/n)*Log[Ni2+][Cu+]2/[Cu2+]2

= 0.410 - (0.0591 / 2) * Log(0.0010)(1.00)2/(0.010)2

= + 0.380 V

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