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![Consider the combustion of SO2(g) represented by the following equation. 2SO2(g) +O2(g) → 2 SO3(g) State whether you would expect this reaction to be spontaneous or non-spontaneous at high temperatures. Clearly justify your choice. Refer to the information given in the table below to answer questions (a) - (c) following. E° (at 298 K)/V -0.338 -0.444 -0.549 Half Reaction in+(aq) + 3 e-→ In(s) In3+(aq) + 2 e-→ In+(aq) Ga3+(aq) + 3 e-→ Ga(s) (a) Calculate the standard cell voltage (E cel), at 298 K, for the cell represented by Ga(s) | Ga3 (aq) || In3 (aq), In (aq) | Pt(s) (b) Calculate ΔG°, at 298 K, for the chemical reaction occurring in the cell described in (a). Calculate the cell voltage, Ecell, at 298 K for the cell described in (a) with [Ga門= 0.150 M, [I㎡+] = 0.00 100 M and [In] = 0.200 M (c) The simplified equation for the industrial production of aluminum by the electrolysis of molten Al203 dissolved in Na3AlF6 is AP+() + 3 e- → Al(s) Calculate the mass of Al(s) produced if 15.0 A of electricity is passed through the solution for 85.0 minutes.](https://media.cheggcdn.com/media%2F957%2F957ba2c9-d124-4d9c-9e62-cc2f9302fdc0%2Fimage)
Consider the combustion of SO_2(g) represented by the following equation. 2SO_2(g) + O_2(g) rightarrow 2 SO_3(g) State whether you would expect this reaction to be spontaneous or non-spontaneous at high temperatures. Clearly justify your choice. Refer to the information given in the table below to answer questions (a) – (c) following. Calculate the standard cell voltage (E degree _cell), at 298 K, for the cell represented by Ga(s) | Ga^3+ (aq) || In^3+ (aq), In^+ (aq) | Pt(s) Calculate Delta G degree, at 298 K, for the chemical reaction occurring in the cell described in (a). Calculate the cell voltage, E_cell, at 298 K for the cell described in (a) with [Ga^3+] = 0.150 M, [In^3+] = 0.00100 M and [In^+] = 0.200 M The simplified equation for the industrial production of aluminum by the electrolysis of molten Al_2O_3 dissolved in Na_3AlF_6 is Al^3+(l) + 3e^- rightarrow Al(s) Calculate the mass of Al(s) produced if 15.0 A of electricity is passed through the solution for 85.0 minutes.
Expert Answer
2SO2(g) + O2(g) —-> 2so3(g)
DH0rxn = 2*-395.7-(2*-296.81+1*0) = -197.78 kj
DS0rxn = 2*256.7-(2*248.1+1*205) = -187.8 j/k
DG0 = dh0-Tds0
= -197.78-(273.15*-187.8)
= 51.1 kj
as DG0 = +ve , it is nonspontaneous at standrad temperature and higher also.
a) E0cell = E0cathode – E0anode
= -0.444 -(-0.549)
= 0.105 v
b) 2Ga(s) + 3In^3+(aq) —-> 3In^+(aq) + 2Ga^3+(aq)
DG0 = – nFE0cell
= -6*96500*0.105
= -60795 joule
c) Ecell = E0cell – 0.0591/nlog[Ga^3+]^2[In^+]^3/[In^3+]^3
= 0.105 – (0.0591/6)log(0.15^2*0.2^3/0.001^3)
= 0.0532 V
faradays first law
w = zit
= (E/F)it
= (9/96500)*15*85*60
mass of Al produced = 7.13 g
