`0.1 g` of metal combines with `46.6 mL` of oxygen at `STP`. The equivalent weight of metal is

Options

A. 12
B. 24
C. 6
D. 36

Explanation

To find the equivalent weight of the metal that combines with oxygen, we can follow these steps:

### Step 1: Calculate the number of equivalents of oxygen
We know that at STP (Standard Temperature and Pressure), 1 mole of any gas occupies 22.4 liters (or 22,400 mL). The molar mass of oxygen (O₂) is 32 g, and since 1 mole of O₂ contains 2 equivalents of oxygen, we can calculate the equivalents of oxygen in the given volume.

Given:
- Volume of O₂ = 46.6 mL

We can calculate the equivalents of oxygen using the formula:
\[ \text{Equivalents of O}_2 = \frac{\text{Volume of O}_2}{\text{Molar Volume}} \times \text{Number of Equivalents per Mole} \]
\[ = \frac{46.6 \, \text{mL}}{22400 \, \text{mL}} \times 4 \]
\[ = \frac{46.6 \times 4}{22400} \]
\[ = \frac{186.4}{22400} \approx 0.00832 \, \text{equivalents} \]

### Step 2: Relate the equivalents of metal to the equivalents of oxygen
According to the law of equivalents, the equivalents of metal will be equal to the equivalents of oxygen that it combines with. Therefore, the equivalents of metal = equivalents of oxygen = 0.00832 equivalents.

### Step 3: Calculate the equivalent weight of the metal
The equivalent weight of a substance is calculated using the formula:
\[ \text{Equivalent Weight} = \frac{\text{Mass of the substance}}{\text{Number of equivalents}} \]
For the metal:
- Mass of metal = 0.1 g
- Number of equivalents = 0.00832

So, we can calculate the equivalent weight of the metal:
\[ \text{Equivalent Weight of Metal} = \frac{0.1 \, \text{g}}{0.00832} \approx 12 \, \text{g/equiv} \]

### Final Answer
The equivalent weight of the metal is **12 g/equiv**.

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