4.7 g of phenol is heated with Zn to give product X. If this reaction goes to 60% completion then the number of moles of compound X formed will be _______ $$\times 10^{-2}$$. (Nearest Integer)
(Given molar mass in g mol$$^{-1}$$: H:1, C:12, O:16)

1. Identify the Reaction

When phenol is heated with zinc (Zn) dust, it undergoes a reduction reaction to form benzene (product X) and zinc oxide.

Reaction equation: Phenol + Zn -> Benzene + ZnO

From the balanced equation, 1 mole of phenol produces 1 mole of benzene.

2. Calculate the Molar Mass of Phenol

• Formula of Phenol: C6H6O (or C6H5OH)
• Carbon (C): 6 atoms * 12 = 72
• Hydrogen (H): 6 atoms * 1 = 6
• Oxygen (O): 1 atom * 16 = 16
• Total Molar Mass of Phenol = 72 + 6 + 16 = 94 grams/mole

3. Calculate the Initial Moles of Phenol

• Given mass of phenol = 4.7 grams
• Initial moles of phenol = Given mass / Molar mass
• Initial moles of phenol = 4.7 / 94 = 0.05 moles

4. Calculate the Moles of Benzene (Product X) Formed

Since the reaction only goes to 60% completion:

• Moles of product X = Initial moles of phenol * 60%
• Moles of product X = 0.05 * (60 / 100)
• Moles of product X = 0.03 moles

5. Convert to the Required Scientific Format

The question asks for the answer in the form: ______ * 10^-2

• 0.03 can be written as 3 * 10^-2

Final Answer

3