What amount of bromine will be required to convert `2g` of phenol into `2,4,6-` tribromphenol

Options

A. `4.00`
B. `6.00`
C. `10.22`
D. `20.44`

Answer

To determine the amount of bromine required to convert 2 grams of phenol into 2,4,6-tribromophenol, we can follow these steps:

### Step 1: Write the balanced chemical equation
The reaction of phenol (C6H5OH) with bromine (Br2) can be represented as follows:

\[ \text{C}_6\text{H}_5\text{OH} + 3 \text{Br}_2 \rightarrow \text{C}_6\text{H}_2\text{Br}_3\text{OH} + 3 \text{HBr} \]

This indicates that one molecule of phenol reacts with three molecules of bromine to form 2,4,6-tribromophenol.

### Step 2: Calculate the molar mass of phenol
The molar mass of phenol (C6H5OH) can be calculated as follows:

- 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

Total molar mass of phenol = 72 + 6 + 16 = 94 g/mol

### Step 3: Calculate the molar mass of bromine
The molar mass of bromine (Br2) is:

- Bromine (Br): 80 g/mol × 2 = 160 g/mol

Since 3 moles of bromine are required for the reaction, the total mass of bromine needed is:

Total mass of bromine = 3 × 160 g/mol = 480 g/mol

### Step 4: Determine the amount of bromine needed for 2 grams of phenol
From the balanced equation, we know that 94 g of phenol reacts with 480 g of bromine. We can set up a proportion to find out how much bromine is needed for 2 g of phenol:

\[ \text{Amount of bromine required} = \left( \frac{480 \text{ g Br}}{94 \text{ g phenol}} \right) \times 2 \text{ g phenol} \]

Calculating this gives:

\[ \text{Amount of bromine required} = \left( \frac{480}{94} \right) \times 2 \approx 10.22 \text{ g} \]

### Final Answer
The amount of bromine required to convert 2 g of phenol into 2,4,6-tribromophenol is approximately **10.22 g**.

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