The oxide of an element contains `67.67%` of oxygen.
Equivalent weight of the element is

Options

A. `2.46`
B. `3.82`
C. `4.36`
D. `4.96`

Explanation

To find the equivalent weight of the element in the oxide that contains 67.67% oxygen, we can follow these steps:

### Step-by-Step Solution:

1. **Determine the percentage of the metal in the oxide:**
- If the oxide contains 67.67% oxygen, then the percentage of the metal (let's denote it as M) in the oxide is:
\[ \text{Percentage of M} = 100\% - 67.67\% = 32.33\% \]

2. **Assume a sample mass of the oxide:**
- For simplicity, assume we have 100 grams of the oxide. This means:
- Mass of oxygen = 67.67 grams
- Mass of metal (M) = 32.33 grams

3. **Calculate the equivalent weight of the metal:**
- The equivalent weight of an element can be calculated using the formula:
\[ \text{Equivalent weight} = \frac{\text{Molecular weight}}{\text{Valency}} \]
- However, we can also relate the equivalent weight of the metal to the amount of oxygen it can combine with. Given that oxygen has an equivalent weight of 8 grams (since the atomic weight of oxygen is approximately 16, and its valency is 2), we can set up a proportion based on the amounts of metal and oxygen.

4. **Set up the proportion:**
- If 67.67 grams of oxygen combine with 32.33 grams of metal, we can find out how much metal would combine with 8 grams of oxygen:
\[ \text{Amount of M that combines with 8 grams of O} = \frac{32.33 \text{ grams of M}}{67.67 \text{ grams of O}} \times 8 \text{ grams of O} \]

5. **Calculate the amount of metal:**
- Performing the calculation:
\[ \text{Amount of M} = \frac{32.33}{67.67} \times 8 \approx 3.82 \text{ grams} \]

6. **Conclusion:**
- The equivalent weight of the metal is approximately 3.82 grams.

### Final Answer:
The equivalent weight of the element is **3.82 grams**.

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