Compute the value of x :
x = 9.4g of phenol `(C_(6)H_(5)OH) +6.02xx10^(23)` molecules of phenol - 0.2 mole of phenol
Here x is:

Options

A. 0.9 mol
B. 9.2 g
C. 0.1 mol
D. `6.02xx10^(23)` molecules

Explanation

To compute the value of \( x \) in the equation:

\[ x = 9.4 \, \text{g of phenol} + 6.02 \times 10^{23} \, \text{molecules of phenol} - 0.2 \, \text{mole of phenol} \]

we will convert all quantities to moles and then perform the calculations.

### Step 1: Convert grams of phenol to moles
First, we need to find the molecular mass of phenol, \( C_6H_5OH \).

- Carbon (C): 12 g/mol × 6 = 72 g/mol
- Hydrogen (H): 1 g/mol × 6 = 6 g/mol
- Oxygen (O): 16 g/mol × 1 = 16 g/mol

Adding these together gives:

\[ \text{Molecular mass of phenol} = 72 + 6 + 16 = 94 \, \text{g/mol} \]

Now, we can convert the mass of phenol to moles using the formula:

\[ \text{Moles} = \frac{\text{Given mass}}{\text{Molecular mass}} \]

For 9.4 g of phenol:

\[ \text{Moles of phenol} = \frac{9.4 \, \text{g}}{94 \, \text{g/mol}} = 0.1 \, \text{moles} \]

### Step 2: Convert molecules of phenol to moles
Next, we convert the number of molecules to moles. We use Avogadro's number, which is \( 6.02 \times 10^{23} \) molecules/mol.

\[ \text{Moles of phenol} = \frac{6.02 \times 10^{23} \, \text{molecules}}{6.02 \times 10^{23} \, \text{molecules/mol}} = 1 \, \text{mole} \]

### Step 3: Combine the moles
Now, we can substitute the values we calculated into the equation for \( x \):

\[ x = 0.1 \, \text{moles} + 1 \, \text{mole} - 0.2 \, \text{mole} \]

### Step 4: Perform the calculation
Calculating this gives:

\[ x = 0.1 + 1 - 0.2 = 0.9 \, \text{moles} \]

### Final Answer
Thus, the value of \( x \) is:

\[ \boxed{0.9 \, \text{moles}} \]