What is E°_cell for the following reaction? 2Au(s) + 3Ca²⁺(aq) → 2Au³⁺(aq) + 3Ca(s)
Au³⁺(aq) + 3e^- → Au(s) E° = 1.50 V
Ca²⁺ (aq) + 2e^- → Ca(s) E° = -2.87 V

Question

What is E°_cell for the following reaction? 2Au(s)+ 3Ca²⁺(aq)→ 2Au³⁺(aq)+ 3Ca(s) Au³⁺(aq)+ 3e^- → Au(s)E° = 1.50 V Ca²⁺ (aq)+ 2e^- → Ca(s)E° = -2.87 V

Quizplus · Accepted Answer

First, we need to write the balanced equation for the overall cell reaction: 2Au(s) + 3CaS2(aq) → 2AuS3(aq) + 3Ca(s) Then, we can use the standard reduction potentials to calculate the overall standard cell potential: E°cell = E°(AuS3(aq)/Au(s)) - E°(CaS2(aq)/Ca(s)) E°cell = (1.50 V) - (-2.87 V) E°cell = 4.37 V However, the question is asking for E°_cell, which includes the stoichiometric coefficients of the balanced equation: E°_cell = (2)(1.50 V) + (3)(-2.87 V) E°_cell = 3.00 V - 8.61 V E°_cell = -5.61 V Finally, we need to flip the sign of E°_cell because the question is asking for the standard emf of the cell in the reverse direction: E°_cell = -(-5.61 V) E°_cell = 5.61 V Therefore, the answer is A, -4.37 V.

What Is E°cell for the Following Reaction? 2Au(s)+ 3Ca2+(aq)→ 2Au3+(aq)

What Is E°_cell for the Following Reaction? 2Au(s)+ 3Ca²⁺(aq)→ 2Au³⁺(aq)