Given below are two reactions of water with sodium and carbon dioxide. What is the nature of water is these reactions?
(i) `2Na+H_(2)Orarr 2NaOH+H_(2)`
(ii) `6CO_(2)+12H_(2)Orarr C_(6)H_(12)O_(6)+6H_(2)O+6O_(2)`

Options

A. In (ii) water acts as an oxidising agent and in (i) it acts as a reducing agent.
B. In (i) water acts as an oxidising agent while in (ii) it acts as a reducing agent.
C. In both, (i) and (ii) hydrogen acts as a reducing agent.
D. In both, (i) and (ii) hydrogen acts as an oxidising agent.

Explanation

To determine the nature of water in the given reactions, we will analyze each reaction step by step.

### Step 1: Analyze the first reaction
The first reaction is:
\[ 2 \text{Na} + \text{H}_2\text{O} \rightarrow 2 \text{NaOH} + \text{H}_2 \]

1. **Identify the changes in oxidation states:**
- Sodium (Na) is oxidized from 0 to +1 (it loses an electron).
- Water (H2O) is reduced as it loses oxygen and produces hydrogen gas (H2).

2. **Determine the role of water:**
- Since water loses oxygen, it is acting as an oxidizing agent (it facilitates the oxidation of sodium).

### Step 2: Analyze the second reaction
The second reaction is:
\[ 6 \text{CO}_2 + 12 \text{H}_2\text{O} \rightarrow \text{C}_6\text{H}_{12}\text{O}_6 + 6 \text{H}_2\text{O} + 6 \text{O}_2 \]

1. **Identify the changes in oxidation states:**
- Carbon dioxide (CO2) is reduced to glucose (C6H12O6), meaning carbon gains hydrogen.
- Water (H2O) is oxidized to oxygen (O2), meaning it loses hydrogen.

2. **Determine the role of water:**
- Since water is losing hydrogen (and thus gaining oxygen), it acts as a reducing agent (it facilitates the reduction of carbon dioxide).

### Conclusion
- In the first reaction, water acts as an **oxidizing agent**.
- In the second reaction, water acts as a **reducing agent**.

### Final Answer
The nature of water in these reactions is:
- In reaction (i), water acts as an oxidizing agent.
- In reaction (ii), water acts as a reducing agent.