What amount of bromine will be required to co | vedclass

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(A) The reaction of phenol with bromine water is: $C_6H_5OH + 3Br_2 ightarrow C_6H_2Br_3OH + 3HBr$Molar mass of phenol $(C_6H_5OH) = (6 	imes 12) +

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$10.22$

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(A) The reaction of phenol with bromine water is: $C_6H_5OH + 3Br_2 ightarrow C_6H_2Br_3OH + 3HBr$Molar mass of phenol $(C_6H_5OH) = (6 	imes 12) + (6 	imes 1) + 16 = 72 + 6 + 16 = 94 \ g \ mol^{-1}$.Moles of phenol = $\frac{2 \ g}{94 \ g \ mol^{-1}} = 0.02128 \ mol$.According to the stoichiometry,$1 \ mol$ of phenol reacts with $3 \ mol$ of $Br_2$.Moles of $Br_2$ required = $3 	imes 0.02128 = 0.06384 \ mol$.Molar mass of $Br_2 = 2 	imes 80 = 160 \ g \ mol^{-1}$.Mass of $Br_2$ required = $0.06384 \ mol 	imes 160 \ g \ mol^{-1} = 10.2144 \ g \approx 10.22 \ g$.

What amount of bromine will be required to convert $2 \ g$ of phenol into $2, 4, 6-$tribromophenol (in $g$)? $($Given molar mass in $g \ mol^{-1}$ of $C, H, O, Br$ are $12, 1, 16, 80$ respectively$)$

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