STATEMENT -1 : FeO is non-stoichiometric with formula `Fe_(0.95)O`.
STATEMENT -2 : Some `Fe^(2+)` ions are replaced by `Fe^(3+)` as `3Fe^(2+)` = `2Fe^(3+)` to maintain electrons neutrality .

Options

A. (a) If both the statement are TRUE and STATEMENT -2 is the correct explanation of STATEMENT -1
B. (b) If both the statement are TRUE and STATEMENT -2 is NOT the correct explanation of STATEMENT -1
C. (c) If STATEMENT -1 is TRUE and STATEMENT -2 is FALSE
D. (d) If STATEMENT -1 is FALSE and STATEMENT -2 is TRUE

Answer

To solve the question, we need to analyze both statements regarding the compound FeO and its non-stoichiometric nature.

### Step-by-Step Solution:

1. **Understanding Non-Stoichiometric Compounds**:
- Non-stoichiometric compounds are those that do not have a fixed ratio of elements. They often arise due to defects in the crystal structure, such as metal deficiency or excess.

2. **Analyzing Statement 1**:
- The first statement claims that FeO is non-stoichiometric with the formula Fe₀.₉₅O.
- This indicates that there is a deficiency of iron in the compound, as the formula suggests that there are fewer iron ions than oxygen ions.
- This statement is **correct**.

3. **Analyzing Statement 2**:
- The second statement suggests that some Fe²⁺ ions are replaced by Fe³⁺ ions in the compound to maintain electrical neutrality, represented by the equation 3Fe²⁺ = 2Fe³⁺.
- In FeO, iron typically exists in the +2 oxidation state. However, to maintain charge balance in the presence of a deficiency of iron, some Fe²⁺ ions can be substituted by Fe³⁺ ions.
- The substitution of Fe²⁺ with Fe³⁺ helps to balance the charge because Fe³⁺ has a higher positive charge than Fe²⁺.
- This statement is also **correct**.

4. **Conclusion**:
- Both statements are correct, and statement 2 provides a valid explanation for statement 1. Therefore, the answer is that both statements are true, and statement 2 is the correct explanation of statement 1.

### Final Answer:
Both Statement 1 and Statement 2 are correct, and Statement 2 is the correct explanation of Statement 1.

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