Question detail
For the half-reaction Ag⁺ + e⁻ → Ag with a standard electrode potential of +0.80 V, what is the cell potential when paired with the half-reaction Zn²⁺ + 2e⁻ → Zn with a standard electrode potential of -0.76 V (A-level cue f794b143 focus)
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
MCQ
Type
practice
Style
Topic
Electrode potentials and electrochemical cells (A-level only)
Question
- A. 1.56 V
- B. 0.04 V (A-level cue f794b143 distractor 1)
- C. 0.80 V (A-level cue f794b143 distractor 2)
- D. 0.76 V (A-level cue f794b143 distractor 3)
Answer
1.56 V
Explanation
The correct option is 1.56 V. 1.56 V is correct because it supports the objective: Calculate cell potentials from standard electrode potentials.. The reasoning stays within Standard electrode potentials (A-level only) and avoids drifting into a similar A-Level Chemistry idea. This version is uniquely anchored to Standard electrode potentials (A-level only). Retrieval anchor: A-level cue f794b143.
Common mistake
Incorrect Cell Potential Calculation
Students often forget to subtract the standard electrode potentials correctly when calculating the cell potential, leading to incorrect signs or values.
To calculate the cell potential (E_cell), use the formula E_cell = E_cathode - E_anode. Substitute the values of the standard electrode potentials for the cathode and anode, then perform the subtraction. For example, if E_cathode = +0.76 V and E_anode = -0.44 V, the calculation would be: E_cell = 0.76 V - (-0.44 V) = 0.76 V + 0.44 V = 1.20 V. Therefore, the cell potential is 1.20 V. Keep the correction anchored to Standard electrode potentials (A-level only) and the objective: Calculate cell potentials from standard electrode potentials.
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