What is the osmotic pressure of a solution made by dissolving 75.0 g of glucose, c6h12o6, in enough water to form 700.0 ml of solution at 45.0 ∘c ? express your answer to three significant figures and include the appropriate u?

We will use the osmotic pressure formula:
π = n R T / V
When π is the osmotic pressure (atm)
n is no.of moles when the molar mass of glucose = 180 g/mol
so, n = 75 g / 180 g/mol= 0.42

and R is gas constant = 0.0821 L.atm/mol.k 
T is the temperature in Kelvin = 45 +273 = 318 K
and V is the volume in Litre = 700 / 1000 = 0.7 L
So, by substitution:
∴ π = 0.42 * 0.0821 * 318 / 0.7 = 15.665 atm

The answer to that would be magnesium

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