Calculate the osmotic pressure (in kPa) of a 350 mL solution containing 0.132 g of an unknown molecule with a molar mass of 665.76 g mol-1 at 37 oC. Assume a Van't Hoff Factor of one.Question 18Answer0.179 kPa2.92 kPa1.46 kPa0.141 kPa0.511 kPa

To calculate the osmotic pressure, we can use the formula:

π = nRT/V

where: π is the osmotic pressure, n is the number of moles of the solute, R is the ideal gas constant, T is the temperature in Kelvin, V is the volume of the solution in liters.

First, we need to calculate the number of moles (n) of the solute. We can do this by dividing the mass of the solute by its molar mass:

n = mass / molar mass n = 0.132 g / 665.76 g/mol n = 0.000198 mol

Next, we convert the temperature from Celsius to Kelvin:

T = 37°C + 273.15 T = 310.15 K

We also convert the volume from mL to L:

V = 350 mL = 0.35 L

The ideal gas constant (R) is 8.3145 L·kPa/(K·mol).

Now we can substitute these values into the formula:

π = nRT/V π = (0.000198 mol) * (8.3145 L·kPa/(K·mol)) * (310.15 K) / (0.35 L) π = 0.179 kPa

So, the osmotic pressure of the solution is 0.179 kPa.