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Calculate δg∘rxn and e∘cell for a redox reaction with n = 3 that has an equilibrium constant of k = 4.4×10−2. you may want to reference (pages 861 - 865) section 19.5 while completing this problem.'

Respuesta :

superman1987
a) First, to get ΔG°rxn we have to use this formula when:

ΔG° = - RT ㏑ K 

when ΔG° is Gibbs free energy 

and R is the constant = 8.314 J/mol K

and T is the temperature in Kelvin = 25 °C+ 273 =  298 K 

and when K = 4.4 x 10^-2

so, by substitution:

ΔG°= - 8.314 * 298 *㏑(4.4 x 10^-2)

      = -7739 J  = -7.7 KJ


b) then, to get E° cell for a redox reaction we have to use this formula:

ΔE° Cell = (RT / nF) ㏑K

when R is a constant = 8.314 J/molK

and T is the temperature in Kelvin = 25°C + 273 = 298 K

and n = no.of moles of e- from the balanced redox reaction= 3

and F is Faraday constant = 96485 C/mol

and K = 4.4 x 10^-2

so, by substitution:

∴ ΔE° cell = (8.314 * 298 / 3* 96485) *㏑(4.4 x 10^-2)

              = - 2.7 x 10^-2 V
  
pstnonsonjoku

The ΔG° of the cell is 7.7 kJ and the E°cell is   -0.027 V.

We know that we can use the formula;

ΔG° = -RTlnK

Where;

ΔG° = standard change in free energy

R = gas constant

T = temperature

K = equilibrium constant

ΔG° = -(8.314 * 298 * (ln4.4×10^−2))

ΔG° = 7.7 kJ

Now;

E°cell = 0.0592/n log K

E°cell = 0.0592/3 log(4.4×10^−2)

E°cell = -0.027 V

Learn more about E°cell :https://brainly.com/question/15308590

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