What reaction happens at the cathode during electrolysis of sodium chloride solution?

Electrolysis of sodium chloride solution (brine) at the cathode, 2H + + 2e – → H 2 ( reduction close reductionThe loss of oxygen, gain of electrons, or gain of hydrogen by a substance during a chemical reaction.)

What product formed at cathode when aqueous sodium chloride is electrolysed?

During the electrolysis of aqueous sodium chloride, sodium ions having a greater tendency than water to get oxidized, gets oxidized and forms sodium at the cathode.

Which reactions occur at cathode during electrolysis?

Electrolysis involves oxidation at the anode and reduction at the cathode. Reason: Oxidation always take place at anode and reduction at cathode.

Is cathode positive or negative?

The anode is usually the positive side. A cathode is a negative side . It acts as an electron donor.

What happens at anode during electrolysis of NaCl?

Chlorine gas is obtained at the anode during the electrolysis of molten sodium chloride.

What is the product formed at the cathode in the electrolysis of aqueous Na2SO4?

A solution of Na2SO4 in water is electrolysed using inert electrodes. The products at cathode and anode are respectively, H2, O2 .

When an aqueous solution of NaCl is electrolysed sodium metal is deposited at the cathode?

Assertion :If an aqueous solution of NaCl is electrolysed, the product obtained at the cathode is H2 gas and not Na . Reason: Gases are liberated faster than the metals.

What is the electrolysis of aqueous sodium chloride?

An aqueous solution of NaCl on electrolysis gives H2(g)′, Cl2(g) and NaOH according to the reaction. 2Cl−(aq)+2H2O⇌2OH−(aq)+H2(g)+Cl2(g)

What are the products obtained at cathode and anode when sodium chloride solution is electrolysed?

Assertion :The electrolysis of NaCl solution gives H2 (g) at cathode and Cl2 (g) at anode . Reason: Cl2 has higher oxidation potential than H2O.

What will be the product obtained at cathode on electrolysis of an aqueous solution of NaCl using platinum pt electrode?

Electrolysis of aqueous NaCl solution using Pt electrodes gives H2 (g) at cathode and Cl2 (g) at anode.

What type of reaction occurs at the cathode?

Cathode: The cathode is where the reduction reaction takes place. This is where the metal electrode gains electrons.

Which of the following reactions occurs at the cathode?

Hint: Always reduction occurs at cathode. During the process of reduction, the oxidation state of the element decreases and the loss of electrons occurs.

What is the cathode in electrolysis?

Anode is the positive part of electrolyte where oxidation takes place and cathode is the negative part of the cell where reduction takes place . The symbol of anode and cathode are A and K respectively. In electrolysis anode is positively charged and cathode is negatively charged.

The following reaction occurs at cathode during the electrolysis of aqueous sodium chloride solution.$Na_{aq}^ + + {e^ - } \\to Na\\left( s \\right),{E^0} =

Hint:
Electrode potential is the electromotive force of the cell that has two electrodes. Standard reduction potentials are calculated under standard temperature and pressures.During electrolysis there is a redox reaction which takes place. The reduction takes place at cathode and oxidation at anode.

See Also

Voltaic Cells

Complete step by step answer:
The standard reduction potentials are defined as the potential of the half cell as the standard hydrogen potential.
It is denoted by the symbol ${E^0}$ .
Standard hydrogen electrode is a gas electrode which is used as a reference electrode for determining the standard electrode potential of elements and the other half cells.

$E_{N{a^ + }/Na}^0 = - 2.71V$
$E_{{H^ + }/{H_2}}^0 = 0.00V$
The standard reduction potential of $N{a^ + }$ is less than that of hydrogen.
From this we get to know that there will be reduction of hydrogen and oxidation of sodium.
So there will be a reduction of hydrogen at cathode as the reduction potential of hydrogen is greater than sodium.
Therefore the reduction reaction is given below as follows:
$H_{aq}^ + + {e^ - } \to \dfrac{1}{2}H\left( g \right)$
In a mercury cell there is a container made up of zinc.
In that container there is a cathode made up of carbon rod and there is a paste of mercuric oxide with $KOH$ as an electrolyte.
In mercury cell mercury oxide reacts with zinc in the presence of an alkali.
Thus in this cell there is no overall reduction taking place as it does not contain ions whose concentration will change.
As its potential does not change, the life span of mercury cells is greater than dry cells.
That is why the cell potential of mercury remains constant throughout its life.

Note: Standard electrode potentials are only applied to aqueous equilibrium only. From standard reduction potential we can only possibly predict the type of reaction and not the rate of reaction. In mercury cells $KOH$ is used as an electrolyte so there might be a chance of it spilling out of the cell due to which there is less ease of handling.

The following reaction occurs at cathode during the electrolysis of aqueous sodium chloride solution.$Na_{aq}^ + + {e^ - } \\to Na\\left( s \\right),{E^0} = - 2.71V$$H_{aq}^ + + {e^ (2024)

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