The osmotic pressure of a solution is calculated using the formula Π=MRT where Π is the osmotic pressure in atm, M is the molarity, R is the ideal gas constant, and T is the kelvin temperature. Part A What is the osmotic pressure of a solution made by dissolving 40.0 g of glucose, C6H12O6, in enough water to form 700.0 mL of solution at 37.0 ∘C ? Express your answer to three significant figures and include the appropriate units. nothing nothing

Osmotic pressure of the solution will be 818.203 Pa.

Explanation:

Osmotic pressure of a solution is defined by the formula,

π = MRT

where π = Osmotic pressure

M = Molarity of the solution

R = Ideal gas constant

T = Temperature in °K

40 grams of glucose was dissolved in water so the Molarity of the solution will be,

M =

Moles of solute =

                          =

                          = moles

Morarity =

              = 0.3175 mole per liter

Value of ideal gas constant 'R' = 8.314

T = 37°C = (273 + 37)° K

              = 310°K

Now by substituting these values in the formula,

π =

  = 818.203 Pa

Therefore, osmotic pressure of the solution will be 818.203 Pa.

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.