Which of the following reactions shows reduction of water ?

Options

A. `2H_(2)O + 2Na to 2NaOH + H_(2)`
B. `6CO_(2) + 12H_(2)O to C_(6)H_(12)O_(6) + 6H_(2)O + 6O_(2)`
C. `2F_(2) + 2H_(2)O to 4H^(+) + 4F^(-) + O_(2)`
D. `P_(4)O_(10) + 6H_(2)O to 4H_(3)PO_(4)`

Explanation

To determine which reaction shows the reduction of water, we need to analyze the oxidation states of the elements involved in each reaction. Reduction is defined as the gain of electrons, which corresponds to a decrease in oxidation state.

### Step-by-Step Solution:

1. **Understand Reduction**:
- Reduction involves the addition of electrons to a substance, resulting in a decrease in its oxidation state.

2. **Analyze the Given Reactions**:
- We have four reactions to consider. Our goal is to identify the reaction where the oxidation state of an element in water decreases.

3. **Examine the First Reaction**:
- The first reaction is:
\[ 2H_2O + 2NaOH \rightarrow 2NaOH + H_2 \]
- Here, we need to determine the oxidation state of hydrogen in both the reactants and products.
- In \(H_2O\), the oxidation state of hydrogen (H) is +1 and that of oxygen (O) is -2.
- In \(H_2\) (the product), the oxidation state of hydrogen is 0 (since it is in its elemental form).
- Therefore, the oxidation state of hydrogen changes from +1 in water to 0 in hydrogen gas, indicating that reduction has occurred.

4. **Examine the Other Reactions**:
- For the remaining reactions, we will check if there is any change in the oxidation state of hydrogen:
- **Second Reaction**: Analyze the oxidation states. If they remain the same, there is no reduction.
- **Third Reaction**: Repeat the analysis for oxidation states.
- **Fourth Reaction**: Again, check the oxidation states.

5. **Conclusion**:
- After analyzing all the reactions, we find that only the first reaction shows a change in the oxidation state of hydrogen from +1 to 0, confirming that reduction has taken place.

### Final Answer:
- The correct answer is **Option 1**.