Question

2AgCl ----heat----2Ag+ Cl2, is it a redox reaction? then which is oxidised and which is reduced. ​

Answer 1

Answer:

Explanation:

0xidation and Reduction ,

Oxidation and reduction reactions involve the transfer of electrons from one atom to another – one atom losing electrons

and another atom gaining electrons. This type of reaction is often called a “redox” reaction (short for reduction/oxidation)

as a reminder that both processes are going on at the same time.

For the reaction: Fe(s) + 2Ag+

(aq) → Fe2+

(aq) + 2Ag(s)

 The reduction half-reaction occurs when electrons are gained or added, causing an atom to become more negative

(less positive):

2Ag+

+2 e- → 2Ag(s)

In order for a reduction reaction to occur, another atom must be oxidized – in other words, if one atom is going to gain electrons,

another atom has to give electrons away. The atom that is reduced is also known as the “oxidizing agent” because it is causing

oxidation of another element.

 The oxidation half-reaction occurs when electrons are lost or donated, causing an atom to become less negative (more

positive):

Fe(s) → Fe2+

(aq) +2 eAgain, if oxidation is to occur, another atom must be reduced – if one atom is going to give electrons away, another atom must

accept them. The atom that is oxidized is also called the “reducing agent” because it is causing reduction of another element.

Notice that the number of electrons gained in the reduction reaction is exactly the same as the number of electrons that

were given away in the oxidation reaction. In order for a redox equation to balance, the same number of electrons must be

transferred in each half-reaction.

 To help identify oxidation and reduction, remember:

OILRIG: Oxidation Is Losing Electrons, Reduction Is Gaining Electrons

or

LEO the Lion says GER: Losing Electrons is Oxidation, Gaining Electrons is Reduction.

Assigning Oxidation Numbers

Oxidation numbers provide a way to identify the number of electrons gained or lost by an element. The following rules

help identify the oxidation number of an element:

1. Elements in their natural (uncombined) state have an oxidation number of 0 (zero).

2. The oxidation number of any monatomic ion (only 1 element) is equal to its ionic charge.

3. The oxidation number of hydrogen is usually +1.

 Exception: In metal hydrides (such as NaH), the oxidation number of hydrogen is -1.

4. The oxidation number of oxygen is usually -2.

 Exception: In peroxides (such as H2O2), the oxidation number of oxygen is -1.

5. The sum of the oxidation numbers in a compound equals 0 (zero).

6. The sum of the oxidation numbers of a polyatomic ion is equal to the charge of the ion.