The given reaction `2HgO(s)rarr 2Hg+O_2` is an example of

Options

A. reduction process
B. oxidation process
C. addition process
D. all of these

Answer

To determine what type of reaction the given equation represents, we can analyze the reaction step by step.

**Step 1: Write down the reaction.**
The reaction given is:
\[ 2 \text{HgO}(s) \rightarrow 2 \text{Hg}(l) + \text{O}_2(g) \]

**Step 2: Identify the reactants and products.**
In this reaction, the reactant is mercury(II) oxide (HgO), and the products are mercury (Hg) and oxygen gas (O₂).

**Step 3: Determine the oxidation states.**
- In HgO, the oxidation state of mercury (Hg) is +2, and the oxidation state of oxygen (O) is -2.
- In the products, elemental mercury (Hg) has an oxidation state of 0, and oxygen (O₂) also has an oxidation state of 0.

**Step 4: Analyze the changes in oxidation states.**
- Mercury (Hg) goes from +2 in HgO to 0 in the elemental form, indicating a reduction (gain of electrons).
- Oxygen (O) goes from -2 in HgO to 0 in O₂, indicating an oxidation (loss of electrons).

**Step 5: Classify the reaction.**
Since there is a reduction process (Hg is reduced) and an oxidation process (O is oxidized), this reaction is classified as a redox reaction (reduction-oxidation reaction). Additionally, since HgO is breaking down into its constituent elements, it is also a decomposition reaction.

**Final Answer:**
The given reaction \( 2 \text{HgO}(s) \rightarrow 2 \text{Hg}(l) + \text{O}_2(g) \) is an example of a **decomposition reaction** and a **redox reaction**.

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