X and Y are two different elements having their atomic masses in `1:2` ratio. The compound formed by the combination of X and Y contains `50%` of X by weight. The empirical formula of the compound is

Options

A. `X_(2)Y`
B. `XY_(2)`
C. `XY`
D. `X_(4)Y`

Explanation

To find the empirical formula of the compound formed by elements X and Y, we can follow these steps:

### Step 1: Determine the Atomic Masses
Given that the atomic masses of X and Y are in the ratio of 1:2, we can assign:
- Atomic mass of X = 1 unit
- Atomic mass of Y = 2 units

### Step 2: Calculate the Weight Contribution
The problem states that the compound contains 50% of X by weight. Since the total weight of the compound is 100%, this means that:
- Weight of X = 50 g
- Weight of Y = 50 g (since 100% - 50% = 50%)

### Step 3: Calculate Moles of X and Y
Next, we need to convert the weights into moles using the formula:
\[ \text{Moles} = \frac{\text{Weight}}{\text{Atomic Mass}} \]
For X:
\[ \text{Moles of X} = \frac{50 \, \text{g}}{1 \, \text{g/mol}} = 50 \, \text{mol} \]
For Y:
\[ \text{Moles of Y} = \frac{50 \, \text{g}}{2 \, \text{g/mol}} = 25 \, \text{mol} \]

### Step 4: Determine the Simplest Ratio
Now, we have:
- Moles of X = 50
- Moles of Y = 25

To find the simplest ratio, we divide both values by the smallest number of moles:
\[ \text{Ratio of X:Y} = \frac{50}{25} : \frac{25}{25} = 2:1 \]

### Step 5: Write the Empirical Formula
From the simplest ratio of 2:1, we can write the empirical formula of the compound as:
\[ \text{Empirical Formula} = X_2Y \]

### Final Answer
The empirical formula of the compound is \( X_2Y \).

---