A compound was found of contain 14.34% oxygen. The minimum molecular weight of the compound is

Options

A. 111.5 g
B. 223.15 g
C. 97.62 g
D. 195.26 g

Answer

To find the minimum molecular weight of the compound containing 14.34% oxygen, we can follow these steps:

### Step 1: Understand the Percentage Composition
We know that the compound contains 14.34% oxygen by weight. This means that in 100 grams of the compound, there are 14.34 grams of oxygen.

### Step 2: Use the Atomic Mass of Oxygen
The atomic mass of oxygen (O) is approximately 16 grams per mole. This means that 14.34 grams of oxygen corresponds to a certain number of moles of oxygen.

### Step 3: Calculate the Moles of Oxygen
To find the number of moles of oxygen in 14.34 grams, we can use the formula:
\[ \text{Moles of O} = \frac{\text{mass of O}}{\text{molar mass of O}} = \frac{14.34 \text{ g}}{16 \text{ g/mol}} \]
Calculating this gives:
\[ \text{Moles of O} = \frac{14.34}{16} \approx 0.89625 \text{ moles} \]

### Step 4: Relate Moles of Oxygen to the Molecular Weight of the Compound
Since we are looking for the minimum molecular weight (X) of the compound, we can set up the equation based on the percentage:
\[ \text{Percentage of O} = \frac{\text{mass of O}}{\text{mass of compound}} \times 100 \]
Substituting the known values:
\[ 14.34 = \frac{14.34}{X} \times 100 \]

### Step 5: Solve for X
Rearranging the equation gives:
\[ X = \frac{14.34 \times 100}{14.34} \]
This simplifies to:
\[ X = \frac{16 \times 100}{14.34} \]
Calculating this gives:
\[ X \approx \frac{1600}{14.34} \approx 111.5 \text{ grams} \]

### Conclusion
Thus, the minimum molecular weight of the compound is approximately **111.5 grams**.