4.7 text{ g} of phenol is heated with Zn to g | vedclass

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(C) The chemical reaction for the reduction of phenol with zinc dust is: $C_6H_5OH + Zn \rightarrow C_6H_6 + ZnO$.First, calculate the molar mass of p

Vedclass · Accepted Answer

$3$

Vedclass · Answer

(C) The chemical reaction for the reduction of phenol with zinc dust is: $C_6H_5OH + Zn ightarrow C_6H_6 + ZnO$.First, calculate the molar mass of phenol $(C_6H_5OH)$: $(6 	imes 12) + (6 	imes 1) + 16 = 72 + 6 + 16 = 94 	ext{ g mol}^{-1}$.Calculate the initial moles of phenol: $	ext{Moles} = \frac{	ext{mass}}{	ext{molar mass}} = \frac{4.7 	ext{ g}}{94 	ext{ g mol}^{-1}} = 0.05 	ext{ moles}$.Since the reaction goes to $60\%$ completion, the moles of product $X$ (benzene) formed is: $0.05 	imes 0.60 = 0.03 	ext{ moles}$.Expressing this in the required format: $0.03 = 3 	imes 10^{-2}$.Therefore, the value is $3$.

$4.7 \text{ g}$ 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 $\text{g mol}^{-1}$: $H:1, C:12, O:16$)

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