Given standard reduction potentials E_deg(Cu^2+/Cu) = +0.34 V and E_deg(Zn^2+/Zn) = -0.76 V, what is the standard cell potential E_deg_cell for the Daniell cell?

Answer and explanation

Correct answer: B. +1.10 V

  1. Step 1: Identify cathode and anode: Cu^2+ has a higher reduction potential, so it acts as the cathode.
  2. Step 2: Zinc has a lower reduction potential, so Zn oxidizes at the anode.
  3. Step 3: Use cell potential formula: E_deg_cell = E_deg_cathode - E_deg_anode.
  4. Step 4: Calculate: E_deg_cell = (+0.34 V) - (-0.76 V) = +0.34 + 0.76 = +1.10 V.
Answer
+1.10 V.
Why not the others: '+0.42 V' subtracts potentials without the double negative (+0.34 - 0.76); '-1.10 V' reverses cathode and anode; '+0.76 V' takes the zinc oxidation potential alone.

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