Respuesta :
Answer:
11.23 atm
Explanation:
Given
Mass = 13.7 g
Volume = 500mL = 0.5 L
Molar concentration = [tex]\frac{\text{Moles}}{\text{Volume}}\\[/tex]
Moles =[tex]\frac{\text{MassC3H7OH }}{\text{Molar mass C3H7OH }}[/tex] = [tex]\frac{13.7}{0.5}[/tex]= 0.2279534 moles
Molar concentration =[tex]\frac{0.2279534}{0.5}[/tex] = 0.4559 M
π = icRT
where
Osmotic pressure = π
Van't Hoff factor (i) = 1
Molar concentration of solute (c) = 0.4559 M
Ideal gas constant (R) = 0.0821 L.atm/K.mol
Kelvin Temperature (T) = 273 + 27 = 300 K
[tex]\pi[/tex] = 1 * 0.4559 * 0.0821 * 300
= 11.23 atm
The value of osmotic pressure is 11.23 atm.
Equation of osmotic pressure:-
[tex]pi= icRT[/tex]......(1)
where Osmotic pressure = pi
Van't Hoff factor=i=1
Ideal gas constant =R= 0.0821 L.atm/K.mol
Temerature=T,(273 + 27) = 300 K
Concentration=c
Given:-
Mass = 13.7 g
Volume = 500mL = 0.5 L
Moles = [tex]\frac{Mass}{Molar mass} =\frac{13.7g}{60.09g/mol} =0.2279534\ mol[/tex]
Molar concentration = [tex]\frac{0.2279\ mol}{0.5\ L}[/tex] = 0.4559 M
Molar concentration of solute (c) = 0.4559 M
Substitute all the values in equation (1) as follows:-
[tex]pi = 1 * 0.4559 * 0.0821 * 300= 11.23 atm[/tex]
Find more information about Van't Hoff factor here
brainly.com/question/22047232
