For the cell reaction 2 F e 3 + a q + 2 I - a q → 2 F e 2 + a q + I 2 a q E c e l l 0 = 0.24 V at 298 K .…

For the cell reaction

2Fe3+aq+2I-aq→2Fe2+aq+I2aq

Ecell0=0.24 V at 298 K. The standard Gibbs energy ΔrG- of the cell reaction is:

[Given that Faraday constant F=96500 Cmol-1 ]

  1.  -46.32 kJ mol-1
  2.  -23.16 kJ mol-1
  3.  46.32 kJ mol-1
  4.   23.16 kJ mol-1

Solution

For the cell reaction
2Fe3+aq+2I-aq→2Fe2+aq+I2aq

n=2

F=96500

Ecello=0.24 V

ΔGo=-nFEcello=-2×96500×0.24=-46320 J=-46.32 kJ

Asked in: NEET 2019 (All India)

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