A solution of30 g of an unknown compound in 116 g of solvent (molar mass =58gmol−1 has vapour pressure of 0.475 atm. If the vapour pressure of pure solvent is 0.5 atm, the molar mass of unknown compound is

A solution of30 g of an unknown compound in 116 g of solvent (molar mass $= 58 g {mol}^{- 1})$ has vapour pressure of 0.475 atm. If the vapour pressure of pure solvent is 0.5 atm, the molar mass of unknown compound is

A
$100 g {mol}^{- 1}$
B
$200 g {mol}^{- 1}$
C
$250 g {mol}^{- 1}$
D
$300 g {mol}^{- 1}$

Solution:

$M_{2} = \frac{m_{2}}{(m_{1} / M_{l}) (- Δ p_{1} / p_{l}^{*})} M_{2} = \frac{30 g}{(116 g / 58 g {mol}^{- 1}) (0.025 atm / 0.5 atm)} M_{2} = 300 g {mol}^{- 1}$

NRC Full Form – National Register of Citizens

Distance Speed Time Formula

Refractive Index Formula

Mass Formula

Electric Current Formula

Ohm’s Law Formula

Wavelength Formula

Electric Power Formula

Resistivity Formula

Solution:

Related content