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Illusion [34]
3 years ago
6

How many grams of testosterone, C19H28O2 (288.4 g/mol), must be dissolved in 299.0 grams of benzene to reduce the freezing point

by 0.500°C ? Refer to the table for the necessary boiling or freezing point constant.
Solvent

Formula

Kb (°C/m)

Kf (°C/m)

Water

H2O

0.512

1.86

Ethanol

CH3CH2OH

1.22

1.99

Chloroform

CHCl3

3.67

Benzene

C6H6

2.53

5.12

Diethyl ether

CH3CH2OCH2CH3

2.02


? g testosterone.
Chemistry
1 answer:
iVinArrow [24]3 years ago
8 0

Answer: 8.42 grams of testosterone

Explanation:

Depression in freezing point is given by:

\Delta T_f=i\times K_f\times m

\Delta T_f=0.500^0C = Depression in freezing point

i= vant hoff factor = 1 (for non electrolyte)

K_f = freezing point constant  of benzene= 5.12^0C/m

m= molality

\Delta T_f=i\times K_f\times \frac{\text{mass of solute}}{\text{molar mass of solute}\times \text{weight of solvent in kg}}

Weight of solvent (benzene)= 299.0 g = 0.299 kg

Molar mass of solute testosterone= 288.4 g/mol

Mass of solute testosterone added = ?

0.500=1\times 5.12\times \frac{xg}{288.4 g/mol\times 0.299kg}

x=8.42g

Thus 8.42 grams of testosterone must be dissolved in 299.0 grams of benzene to reduce the freezing point by 0.500°C.

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