A compound having molecular formula `C_6 H_(14)O_6` and empirical formula `C_3 H_7 O_3` , value of n is _________

Options

A. 1
B. 2
C. 3
D. 4

Explanation

To find the value of \( n \) in the relationship between the molecular formula and the empirical formula, we can follow these steps:

### Step 1: Identify the Molecular Formula and Empirical Formula
The given molecular formula is \( C_6H_{14}O_6 \) and the empirical formula is \( C_3H_7O_3 \).

### Step 2: Determine the Empirical Formula's Ratio
The empirical formula represents the simplest whole number ratio of the elements in the compound.

### Step 3: Calculate the Ratio of the Molecular Formula to the Empirical Formula
To find \( n \), we need to determine how many times the empirical formula fits into the molecular formula.

1. **Count the number of each type of atom in the molecular formula:**
- Carbon (C): 6
- Hydrogen (H): 14
- Oxygen (O): 6

2. **Count the number of each type of atom in the empirical formula:**
- Carbon (C): 3
- Hydrogen (H): 7
- Oxygen (O): 3

### Step 4: Calculate \( n \) for Each Element
Now, we can calculate \( n \) for each element by dividing the number of atoms in the molecular formula by the number of atoms in the empirical formula.

- For Carbon:
\[ n_C = \frac{6}{3} = 2 \]

- For Hydrogen:
\[ n_H = \frac{14}{7} = 2 \]

- For Oxygen:
\[ n_O = \frac{6}{3} = 2 \]

### Step 5: Conclusion
Since \( n \) is the same for all elements, we conclude that:
\[ n = 2 \]

Thus, the value of \( n \) is **2**.

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