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The E\u00b0 values for two electrodes are shown - AQA - A-Level Chemistry - Question 13 - 2019 - Paper 3
Question 13
The E\u00b0 values for two electrodes are shown. Fe<sup>3+</sup>(aq) + 2e<sup>-</sup> \u2192 Fe(s) E\u00b0 = -0.44 V Cu<sup>2+</sup>(aq) + 2e<sup>-</sup> \u2192 Cu... show full transcript
Worked Solution & Example Answer:The E\u00b0 values for two electrodes are shown - AQA - A-Level Chemistry - Question 13 - 2019 - Paper 3
Step 1
Calculate the EMF of the cell
Answer
To find the EMF of the cell, we use the formula:
In this case:
- The cathode is the copper half-cell (Cu²⁺/Cu) with a standard reduction potential of +0.34 V.
- The anode is the iron half-cell (Fe³⁺/Fe) with a standard reduction potential of -0.44 V.
Substituting the values into the equation:
This simplifies to:
Therefore, the EMF of the cell is +0.78 V.