Question

Electrochemistry - Equilibrium

1. The electrochemical cell described by the balanced chemical equation has a standard emf (electromotive force) of -0.08 V. Calculate the value (J) for the W_max that the cell can do under standard conditions. Round your answer to 3 significant figures.

St. Red. Pot. (V)	Faraday's Constant
Hg2+/Hg +0.85	F = 96485 C
Fe3+/Fe2+ +0.77

2Fe³⁺(aq) + Hg(l) → 2Fe²⁺(aq) + Hg²⁺(aq)

2. The voltaic cell described by the balanced chemical equation has a standard emf of 0.12 V. Calculate the Wmax (kJ) the cell has done if 501.97 g of Cl-(aq) (Molar Mass - 35.45 g/mol) reacts. Round your answer to 3 significant figures. St. Red. Pot. (V) Faraday's Constant AgCl/Ag +0.22 F = 96485 C Cu2+/Cu +0.34 2Ag(s) + 2Cl-(aq) + Cu2+(aq) → 2AgCl(s) + Cu(s) 3. The galvanic cell described by the cell notation has a standard emf (electromotive force) of 0.20 V. Calculate the value (J) for the Wmax that the cell can do under standard conditions. Round your answer to 3 significant figures. St. Red. Pot. (V) Faraday's Constant H+/H2 0 F = 96485 C SO42-/H2SO3 +0.20 Pt(s), H2(g) l H+(aq) ll H+(aq), SO42-(aq), H2SO3(aq) l Pt(s)

Answer 1