In a laboratory experiment, a student found that a 136-mL aqueous solution containing 2.257 g of a compound had an osmotic pressure of 20.7 mm Hg at 298 K. The compound was also found to be nonvolatile and a nonelectrolyte. What is the molar mass of this compound?

Question

Chemistry

Sullivan Collins

20 November, 11:15

In a laboratory experiment, a student found that a 136-mL aqueous solution containing 2.257 g of a compound had an osmotic pressure of 20.7 mm Hg at 298 K. The compound was also found to be nonvolatile and a nonelectrolyte. What is the molar mass of this compound?

+5

Answers (1)

Know the Answer?

Amber Forbes · Answer 1

14889 g/mol is the molar mass of the compound

Explanation:

Let's apply the colligate property of osmotic pressure to solve this problem

π = M. R. T

First of all, we convert the osmotic pressure from mmHg to atm

20.7 mmHg. 1 atm/760 mmHg = 0.0272 atm

Let's replace the data in the formula to find out the molarity of the compound.

0.0272 atm = M. 0.082L. atm/mol. K. 298K

0.0272 atm / (0.082L. atm/mol. K. 298K) = M

1.11*10⁻³ = M

Molarity is mol/L, and mol is mass (g) / molar mass. Let's make the equation to replace the vaules.

(2.257 g / X) / 0.136L = 1.11*10⁻³ mol/L

(2.257 g / X) = 1.11*10⁻³ mol/L. 0.136L

2.257 g / X = 1.51*10⁻⁴ mol

2.257 g / 1.51*10⁻⁴ mol = 14889 g/mol