`Fe_(0.94) O to Fe^(3+)`, the equivalent mass of `Fe_(0.94)O` will be:

Options

A. `("mol. Mass")/(2)`
B. `("mol.mass")/(3)`
C. `(3xx " mol. Mass)/(8)`
D. `("mol.mass")/(0.87)`

Answer

To find the equivalent mass of Fe₀.₉₄O when it is converted to Fe³⁺, we can follow these steps:

### Step 1: Determine the oxidation state of Fe in Fe₀.₉₄O
Let the oxidation state of Fe be \( x \). The compound Fe₀.₉₄O is neutral, so we can set up the equation based on the oxidation states:

\[ 0.94x + (-2) = 0 \]

This simplifies to:

\[ 0.94x = 2 \]

Now, solving for \( x \):

\[ x = \frac{2}{0.94} \approx 2.13 \]

### Step 2: Calculate the change in oxidation state
The change in oxidation state from Fe in Fe₀.₉₄O to Fe³⁺ is:

\[ \Delta x = 3 - 2.13 = 0.87 \]

### Step 3: Determine the n-factor (valency factor)
The n-factor is equal to the change in oxidation state, which we found to be:

\[ n = 0.87 \]

### Step 4: Calculate the molar mass of Fe₀.₉₄O
To calculate the molar mass of Fe₀.₉₄O, we need the atomic masses:
- Atomic mass of Fe ≈ 55.85 g/mol
- Atomic mass of O ≈ 16.00 g/mol

Calculating the molar mass:

\[ \text{Molar mass of Fe}_{0.94}\text{O} = (0.94 \times 55.85) + (1 \times 16.00) \]

Calculating each part:

\[ 0.94 \times 55.85 \approx 52.51 \]
\[ \text{Total Molar Mass} = 52.51 + 16.00 \approx 68.51 \text{ g/mol} \]

### Step 5: Calculate the equivalent mass
The equivalent mass is given by the formula:

\[ \text{Equivalent mass} = \frac{\text{Molar mass}}{n} \]

Substituting the values we have:

\[ \text{Equivalent mass} = \frac{68.51}{0.87} \approx 78.73 \text{ g/equiv} \]

### Conclusion
The equivalent mass of Fe₀.₉₄O when it is converted to Fe³⁺ is approximately 78.73 g/equiv.

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