Calculate the maximum electrical work obtainable at 25^oC from the following voltaic cell.
Cd(s) |Cd²⁺(0.840M) ||Cl₂(g,0.0354atm) |Cl^-(0.0473M) |Pt;Eº_cell = 1.76V

Question

Calculate the maximum electrical work obtainable at 25^oC from the following voltaic cell. Cd(s)|Cd²⁺(0.840M)||Cl₂(g,0.0354atm)|Cl^-(0.0473M)|Pt;Eº_cell = 1.76V

Quizplus · Accepted Answer

The maximum electrical work obtainable can be calculated using the formula ΔG = -nFE, where n is the number of electrons transferred, F is the Faraday constant (96,485 C/mol), and E is the cell potential. First, we need to balance the redox equation: Cd(s) + 2Cl₂(g) → Cd²⁺(aq) + 2Cl^-(aq) The number of electrons transferred is 2, since each Cl2 molecule is reduced to 2 Cl- ions. The cell potential is Ecell = Eºcell - (RT/nF)lnQ, where R is the gas constant, T is the temperature in Kelvin, and Q is the reaction quotient. At standard conditions, Q = 1, so Ecell = Eºcell. Substituting the given values, we get: Ecell = 1.76V - (8.314 J/mol*K * 298 K / (2 * 96,485 C/mol))ln(0.0473 / 0.840^2 * 0.0354^2) Ecell = 1.22V Now we can calculate the maximum electrical work obtainable: ΔG = -nFE = -2 * 96,485 C/mol * 1.22V = -2.36 * 10^5 J/mol Since we have 0.7 moles of Cd²⁺, the maximum electrical work obtainable is: -2.36 * 10^5 J/mol * 0.7 mol = -1.65 * 10^5 J or 3.47 × 10^15 J in scientific notation. Therefore, the best choice is D.

Calculate the Maximum Electrical Work Obtainable at 25oC from the Following

Calculate the Maximum Electrical Work Obtainable at 25^oC from the Following