2AgCl → 2Ag(s) + Cl₂(g)
What is the suitable condition for the above reaction to take place?

Correct option is B

Sol: The correct answer is (b) Sunlight

Key Points:

​Photodecomposition Reaction: Silver chloride decomposes when exposed to sunlight.​

The reaction:

$$2AgCl --Sunlight--> 2Ag(s) + Cl_2(g)$$​​

This reaction occurs because sunlight provides the energy needed to break the chemical bonds in silver chloride, leading to the formation of silver and chlorine gas.

Information booster:

Pressure

• Adding pressure does not influence the decomposition of silver chloride because this reaction depends on light energy (photolysis), not pressure. Pressure affects reactions involving significant volume changes
  

Heat

• Heat could theoretically provide the energy needed to break $\text{AgCl}$'s bonds, but this reaction specifically requires light energy because $\text{AgCl}$ is photosensitive. It decomposes only when exposed to light, not heat.

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