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MMLU-Pro / 4569 / The mean ionic activity coefficient of an electrolyte in a dilute solution is…

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question

The mean ionic activity coefficient of an electrolyte in a dilute solution is given approximately by ln \gamma_\pm = - A\surd(m) where m is the molality and A is a constant. Using the Gibbs-Duhem equation find the activity coefficient \gamma_1 of the solvent in this dilute solution in terms of A, m, and constants characteristic of the solvent and solute. Ob-serve that ln X_1 = ln [(n_1) / (n_1 + mv)] = ln [(1) / {(1 + mv) / n_1}] \approx - [(mv) / (n_1)] where v is the number of ions in the formula (for example v = 2 for NaCl) and n_1 is the number of moles of solvent in 1000 g of solvent. All quantities except \gamma_1 , the un-known, can thus be expressed in terms of the variable m.

category

chemistry

options

  1. \gamma_1 = e[{(Av^2) / (3n_1)} m^3/2]
  2. \gamma_1 = e[{(Av^2) / (2n_1)} m^3/2]
  3. \gamma_1 = e[{(Av) / (3n_1)} m^3/2]
  4. \gamma_1 = e[{(Av) / (3n_1^2)} m^3/2]
  5. \gamma_1 = [{(Av) / (3n_1)} m^3/2]
  6. \gamma_1 = [{(Av^2) / (3n_1)} m^3/2]
  7. \gamma_1 = [{(A) / (n_1v)} m^3/2]
  8. \gamma_1 = e[{(A) / (2n_1v^2)} m^3/2]
  9. \gamma_1 = e[{(A) / (3n_1v)} m^3/2]
  10. \gamma_1 = [{(Av) / (2n_1)} m^3/2]

src

stemez-PhysicalChemistry

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