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Consider the half-cell equations and their half-cell potentials in the table below - VCE - SSCE Chemistry - Question 28 - 2023 - Paper 1
Question 28
Consider the half-cell equations and their half-cell potentials in the table below. | Half-cell equations | Standard electrode potential (E°) in volts at 2... show full transcript
Worked Solution & Example Answer:Consider the half-cell equations and their half-cell potentials in the table below - VCE - SSCE Chemistry - Question 28 - 2023 - Paper 1
Step 1
Determine the Cell Voltage
Answer
To calculate the cell voltage, we use the standard electrode potentials provided in the table. The cell voltage (E°_cell) can be calculated using:
In this cell:
- The cathode is Mn²⁺/Mn with a potential of +1.56 V.
- The anode is SO₃²⁻/SO₄²⁻, which has a potential of -0.57 V.
Thus, substituting these values:
This value doesn't match the options directly, which suggests we should consider the options carefully.
Step 2
Evaluate the Cell Options
Answer
From the above calculations, we need to match the result with provided options:
- A. 2.50 V if the electrode in the second half-cell is Mn(s).
- B. 1.75 V if the electrode in the second half-cell is Pt(s).
- C. 1.75 V if the electrode in the second half-cell is Mn(s).
- D. 2.50 V if the electrode in the second half-cell is Pt(s).
Given that the calculation suggests potential variations depending on the electrodes used, we conclude:
- Correct Answer: B. 1.75 V if the electrode in the second half-cell is Pt(s).
This indicates that using a platinum electrode can deliver the required potential according to the cell configuration.