Determining molar mass of protein from osmotic pressure


> 
> A 299 mL solution containing 21 g of a protein in toluene had an osmotic pressure of 0.053 atm at 27 degrees Celsius. What is the molar mass (in g/mol) of the protein?
> 
> 
> 


We can use the formula that


$$\Pi = iMRT$$


where $\Pi$ is the osmotic pressure, $i$ the van't Hoff factor, $M$ being the molarity, $R$ being the constant (0.08206), and $T$ being temperature in Kelvin. 


Using these values, we can substitute into the equation:
0.053 atm = 1 \* *M* \* 0.08206 L atm/(mol \* K) \* 300.15 K


When we equate this to *M*, we get 
0.00215 = *M*


Now we know that there is 21 grams of toluene within the 299 mL solution. We can convert the Molarity given by multiplying it by the liters of solution there is. Therefore, 
0.299 L \* 0.00215 mol/L = 0.000643 mol


Finally, to get molar mass, you simply divide the mass of toluene by the mols given:


21 g / 0.000643 mol = 32639.41 g/mol


This value, however, doesn't seem to be correct, as it is absurdly large. Can anyone help tell me what I'm doing wrong?


-*EDIT*- I was reading through the question and realized that the answer was correct, I was just thinking about it in a different sense. Thanks to everyone for their help!


