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Valency and Oxidation State

Here is an el...

Question

Here is an electrode reaction:
$C u \to C u^{2 +} + 2 e^{-}$
At which electrode (anode or cathode) would such a reaction takes place? Is this an example of oxidation or reduction?

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Solution

Oxidation is the process when an element loses electrons whereas reduction is the process of gain of electrons.
The reaction is $C u \to C u^{2 +} + 2 e^{-}$ .
There is a loss of electrons so, the reaction will take place at the anode and is an example of an oxidation reaction.
The reaction will take place at anode and it is an example of oxidation.

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Similar questions

(a) Here is an electrode reaction :

$C u \to C u^{2 +} + 2 e^{-}$ . At which electrode (anode or cathode) would such a reaction take place? Is this an example of oxidation or reduction ?

(b) A solution contains magnesium ions $(M g^{2 +})$ , iron (II) ions $F e^{2 +}$ and copper ions $C u^{2 +}$ . On passing an electric current through this solution, which ions will be the first to be discharged at the cathode? Write the equation for the cathode reaction.

(c) Why is carbon tetrachloride, which is a liquid, a non-electrolyte ?

(d) During the electrolysis of molten lead bromide, which of the following takes place ?

A. Bromine is released at the cathode,

B. Lead is deposited at the anode,

C. Bromine ions gain electrons,

D. Lead is deposited at the cathode.

Q. (a) Here is an electrode reaction:
Cu → Cu²⁺ + 2e.
At which electrode (anode or cathode) would such a reaction take place? Is this an example of oxidation?
(b) A solution contains magnesium ions (Mg²⁺), iron (II) ions (Fe²⁺) and copper ions (Cu²⁺). On passing an electric current through this solution which ions will be the first to be discharged at the cathode? Write the equation for the cathode reaction.
(c) Why is carbon tetrachloride, which is a liquid, a non-electrolyte?

Q. Assertion: Starting from aq. copper [II] sulphate solution, equations for the reactions at the cathode and anode during electrolysis of aq.

C u S O_{4}

using active copper electrodes is;
at anode:

C u^{+ 2} + 2 e^{-} \to C u

C u \to C u^{+ 2} + 2 e^{-}

Reason: Oxidation always take place at anode and reduction at cathode.

Electrochemical Battery

An electrochemical battery is a device powered by oxidation and reduction reactions that are physically separated. So that the electrons must travel through a wire from the reducing agent to the oxidizing agent.

The reducing agent loses electrons and is oxidized in a reaction that takes place at an electrode is called the anode. The oxidizing agent gains electrons and is reduced in a reaction that takes at an electrode is called the cathode.

To maintain a net zero charge in each compartment, there is a limited flow of ions through a salt bridge.

For example, in a car battery the reducing agent is oxidized by the following reaction, which involves a lead (

P b

) anode and sulfuric acid (

H_{2} S O_{4}

). Lead sulfate (

P b S O_{4}

H

), and electrons (

e^{-}

) are produced.

At the cathode, the below reaction occurs :

P b O_{2} + H_{2} S O_{4} + 2 H^{+} + 2 e^{-} \to

At the anode, the below reaction occurs :

P b + H_{2} S O_{4} \to P b S O_{4} + 2 H^{+} + 2 e^{-}

Electrons are produced by a chemical reaction that takes place at the:

Q. Assertion :Anode is the electrode at which oxidation occurs and cathode is the electrode at which reduction occurs. Reason: Anode and cathode in electrochemical cells and electrolytic cells have opposite polarity.

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