Question

# A 200-mg sample of a purified compound of unknown molar mass is dissolved in benzene and dilut ed with that solvent to a volume of 25.0 cm^3. The resulting solution is found to have an osmotic pressure of 0.010 5 atm at 300 K. What is the molar mass of the unknown compound?

Solution

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\begin{aligned} c & = \frac { 0.0105 \mathrm { am } } { 0.08206 \mathrm { stm } \mathrm { L } \mathrm { mol } ^ { - 1 } \mathrm { K } ^ {-1 } \times 300.00 \mathrm { K } } \\\\ c & = 4.26 \times 10 ^ { - 3 } \mathrm { mol } \mathrm { L } ^ { - 1 } \end{aligned}

$c = \frac { \pi } { R T }$

$\pi = 0.0105$ atm

$T = 300.00 \mathrm { K }$

$R = 0.08206 \mathrm { atm } \mathrm { L } \mathrm { mol } ^ { - 1 } \mathrm { K } ^ { - 1 }$

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