Question

If 2 g phenol is allowed to react with \( \text{Br}_2/\text{H}_2\text{O} \), how much \( \text{Br}_2 \) will be required to produce 2,4,6-tribromophenol (rounded to the nearest integer)?

Hint:

To find the required mass in reactions, calculate the moles of the limiting reagent and use stoichiometry to determine the mass of other reagents.

Answer 1

We can calculate the required mass of \( \text{Br}_2 \) by first determining the molar mass of phenol and the stoichiometry of the reaction. - Molar mass of phenol = 94 g/mol. - Molar mass of \( \text{Br}_2 \) = 159.808 g/mol. For every mole of phenol, 3 moles of \( \text{Br}_2 \) are needed to form 2,4,6-tribromophenol. Therefore, the number of moles of \( \text{Br}_2 \) required is: \[ \frac{2}{94} \times 3 \times 159.808 = \text{grams of } \text{Br}_2. \] Thus, the required mass of \( \text{Br}_2 \) is calculated to the nearest integer.