What are the active masses of methyl alcohol | vedclass

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Question

(D) Active mass is defined as molar concentration (molarity) in $mol/L$.Formula: $	ext{Active Mass} = \frac{	ext{Mass in grams}}{	ext{Molar mass} \

Vedclass · Accepted Answer

$15.62$ and $7.79$

Vedclass · Answer

(D) Active mass is defined as molar concentration (molarity) in $mol/L$.Formula: $	ext{Active Mass} = \frac{	ext{Mass in grams}}{	ext{Molar mass} 	imes 	ext{Volume in Liters}}$.Given density $d = \frac{m}{V}$,so $m = d 	imes V$.For $1 \, L$ $(1000 \, mL)$ of solution:$1$. For $CH_3OH$ $(d = 0.5 \, g/mL)$:Mass $= 0.5 \, g/mL 	imes 1000 \, mL = 500 \, g$.$Molar mass of CH_3OH = 12 + 3(1) + 16 + 1 = 32 \, g/mol$.Active mass $= \frac{500 \, g}{32 \, g/mol 	imes 1 \, L} = 15.625 \approx 15.62 \, mol/L$.$2$. For $CCl_4$ $(d = 1.3 \, g/mL)$:Mass $= 1.3 \, g/mL 	imes 1000 \, mL = 1300 \, g$.$Molar mass of CCl_4 = 12 + 4(35.5) = 12 + 142 = 154 \, g/mol$.Active mass $= \frac{1300 \, g}{154 \, g/mol 	imes 1 \, L} = 8.44 \, mol/L$.Note: The provided option $D$ ($15.62$ and $7.79$) assumes a density of $1.2 \, g/mL$ for $CCl_4$ $(1200/154 = 7.79)$. Based on the provided density of $1.3 \, g/mL$,the calculation yields $8.44$. Given the options,$D$ is the intended answer based on the calculation method.

What are the active masses of methyl alcohol $(CH_3OH)$ and carbon tetrachloride $(CCl_4)$ respectively,if their densities are $0.5 \, g/mL$ and $1.3 \, g/mL$?

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