In this cell
A - VCE - SSCE Chemistry - Question 17 - 2012 - Paper 1
Question 17
In this cell
A. Ag^{+} (aq) is reduced and the Zn(s) is oxidised.
B. Ag(s) is oxidised and the Zn^{2+} (aq) is reduced.
C. Ag(s) is reduced and the Zn^{2+} (aq) is o... show full transcript
Worked Solution & Example Answer:In this cell
A - VCE - SSCE Chemistry - Question 17 - 2012 - Paper 1
Step 1
A. Ag^{+} (aq) is reduced and the Zn(s) is oxidised.
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Answer
In this option, Ag^{+} being reduced implies it gains electrons. At the same time, Zn(s) will lose electrons and be oxidised to Zn^{2+} (aq). This option is correct.
Step 2
B. Ag(s) is oxidised and the Zn^{2+} (aq) is reduced.
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Answer
In this case, if Ag(s) was oxidised, it would lose electrons, which contradicts the reduction of Zn^{2+} to Zn(s). Thus, this option is incorrect.
Step 3
C. Ag(s) is reduced and the Zn^{2+} (aq) is oxidised.
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Answer
If Ag(s) was reduced, it would gain electrons; however, this cannot occur simultaneously with the oxidation of Zn^{2+} because there is no source of electrons. Therefore, this option is also incorrect.
Step 4
D. Ag^{+} (aq) is oxidised and the Zn(s) is reduced.
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Answer
This option states that Ag^{+} (aq), which is a cation, is oxidised. For oxidation, Ag^{+} must lose electrons, contradicting the idea that it is being reduced. Therefore, this option is incorrect.
