Depict the galvanic cell in which the reaction Zn(s) + 2Ag+ (aq) \(\rightarrow\) Zn2+ (aq) + 2Ag(s) takes place, further show: - which of the electrode is negatively charged,
- the carriers of the current in the cell, and
- individual reaction at each electrode.
- which of the electrode is negatively charged,
- the carriers of the current in the cell, and
- individual reaction at each electrode.
Solution and Explanation
The galvanic cell corresponding to the given redox reaction can be represented as:
\(Zn[Zn^{2+}_{(aq)}∥Ag^+_{(aq)}]Ag\)
(i) \(Zn\) electrode is negatively charged because at this electrode, \(Zn\) oxidizes to \(Zn ^{2+}\) and the leaving electrons accumulate on this electrode.
(ii) Ions are the carriers of current in the cell.
(iii) The reaction taking place at \(Zn\) electrode can be represented as:
\(Zn_{(s})\rightarrow Zn^{2+}_{(aq)}+2e^−\)
And the reaction taking place at Ag electrode can be represented as:
\(Ag^+_{(aq)}+e^-\rightarrow Ag_{(s)}\)
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Concepts Used:
Redox Reactions
Redox Reaction:
Redox reactions are chemical reactions where oxidation and reduction take place simultaneously. In this type of reaction, there is a gain of electrons for one chemical species while the other loses electrons or simply involves transfer of electrons. The species that loses electrons is oxidized while the one that gains electrons is reduced.
Types of Redox Reactions:
Redox reactions can be differentiated into 4 categories namely combination reactions, decomposition reactions, displacement reactions, and disproportionation reactions. Each is explained separately below:
Combination Reaction:
In this, the molecules combine to form new compounds. For example, when magnesium reacts to nitrogen.
Decomposition Reaction:
Opposite to the combination reaction, here there is a breakdown of compounds to simpler substances. For example, electrolysis of water.
Displacement Reaction:
In this, the more reactive metal will displace the less reactive one in a chemical reaction. The reactivity of an element is represented in a series called the reactivity series (arranged in decreasing order of reactivity) which makes it easier to determine the chemical reaction and its products.
Disproportionation Reaction:
This is a peculiar type of reaction where an element showing a particular oxidation state will be oxidized and reduced simultaneously. Another thing to note is that these reactions will always have an element that can exhibit three oxidation states.