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(D) Step $1$: Calculate the number of moles of urea. Given mass $= 300 \ mg = 0.3 \ g$. Molar mass $= 60 \ g/mol$. Moles $(n) = \frac{0.3 \ g}{60 \ g/

Vedclass · Accepted Answer

$0.166$

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(D) Step $1$: Calculate the number of moles of urea. Given mass $= 300 \ mg = 0.3 \ g$. Molar mass $= 60 \ g/mol$. Moles $(n) = \frac{0.3 \ g}{60 \ g/mol} = 0.005 \ mol$. Step $2$: Calculate the mass of the solvent in $kg$. Mass of water $= 30 \ g = 0.03 \ kg$. Step $3$: Calculate molality $(m)$. Molality $= \frac{	ext{moles of solute}}{	ext{mass of solvent in } kg} = \frac{0.005 \ mol}{0.03 \ kg} = 0.166 \ m$.

What is the molality of a solution containing $300 \ mg$ of urea (molar mass $60 \ g/mol$) dissolved in $30 \ g$ of water (in $m$)?

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