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The cathode in this cell and the maximum voltage produced by this cell, under standard conditions, are respectively A - VCE - SSCE Chemistry - Question 18 - 2012 - Paper 1

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The cathode in this cell and the maximum voltage produced by this cell, under standard conditions, are respectively A. Ag and 0.16 V B. Ag and 1.56 V C. Zn and 0.16 ... show full transcript

Worked Solution & Example Answer:The cathode in this cell and the maximum voltage produced by this cell, under standard conditions, are respectively A - VCE - SSCE Chemistry - Question 18 - 2012 - Paper 1

Step 1

The cathode in this cell

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Answer

To determine the cathode in the electrochemical cell, we need to identify the species that is being reduced. In general, the cathode is where reduction occurs, which typically involves the gaining of electrons. In standard conditions, silver (Ag) has a higher reduction potential compared to zinc (Zn). Therefore, the cathode is Ag.

Step 2

maximum voltage produced by this cell under standard conditions

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Answer

The standard cell potential can be calculated based on the reduction potentials of both cathode and anode. The standard reduction potential for Ag is +0.80 V and for Zn it is -0.76 V. The cell voltage (E°) is given by:

Eextcell=Eextcathode−EextanodeE^{ ext{cell}} = E^{ ext{cathode}} - E^{ ext{anode}}

Substituting the values, we find:

Eextcell=0.80extV−(−0.76extV)=0.80extV+0.76extV=1.56extVE^{ ext{cell}} = 0.80 ext{ V} - (-0.76 ext{ V}) = 0.80 ext{ V} + 0.76 ext{ V} = 1.56 ext{ V}

Thus, the maximum voltage produced is 1.56 V.

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