Answer:
2710.2g/mol
Explanation:
Step 1:
Data obtained from the question. This include the following:
van 't Hoff factor (i) = 1 (since the compound is non-electrolyte)
Mass of compound = 33.2g
Volume = 250mL
Osmotic pressure (Π) = 1.2 atm
Temperature (T) = 25ºC = 25ºC + 273 = 298K
Gas constant (R) = 0.0821 atm.L/Kmol
Molar mass of compound =.?
Step 2:
Determination of the molarity of the compound.
The molarity, M of the compound can be obtained as follow:
Π = iMRT
1.2 = 1 x M x 0.0821 x 298
Divide both side by 0.0821 x 298
M = 1.2 / (0.0821 x 298)
M = 0.049mol/L
Step 3:
Determination of the number of mole of compound in the solution. This can be obtain as follow:
Molarity = 0.049mol/L
Volume = 250mL = 250/1000 = 0.25L
Mole of compound =..?
Molarity = mole /Volume
0.049 = mole / 0.25
Cross multiply
Mole = 0.049 x 0.25
Mole of compound = 0.01225 mole.
Step 4:
Determination of the molar mass of the compound. This is illustrated below:
Mole of the compound = 0.01225 mole.
Mass of the compound = 33.2g
Molar mass of the compound =.?
Mole = Mass /Molar Mass
0.01225 = 33.2/Molar Mass
Cross multiply
0.01225 x molar mass = 33.2
Divide both side by 0.01225
Molar mass = 33.2/0.01225
Molar mass of the compound = 2710.2g/mol
Therefore, the molar mass of the compound is 2710.2g/mol
