What is the osmotic pressure of a solution made by dissolving 55.0 g of glucose, C6H12O6, in enough water to form 800.0 mL of solution at 10.0 ∘C ? Express your answer to three significant figures and include the appropriate units. View Available Hint(s)

The osmotic pressure is 8.85 atm

Explanation:

Step : Data given

Mass of glucose = 55.0 grams

Volume of water =800.0 mL

Temperature = 10.0 °C

Step 2: Calculate moles glucose

Moles glucose = mass glucose / molar mass glucose

Moles glucose = 55.0 grams / 180.156 g/mol

Moles glucose = 0.305 moles

Step 3: Calculate osmotic pressure

π = iMRT  

⇒ with π = the osmotic pressure = TO BE DETERMINED

⇒ with i = the van't Hoff factor for glucose = 1

⇒ with M = the concentration = moles / volume = 0.305 moles / 0.800 L =0.381 M

⇒ with R = the gas constant = 0.08206 L*atm*mol¨K

⇒ with T = the temperature = 10.0 °C = 283 K

 π = 1* 0.381 *0.08206 * 283

 π = 8.85 atm

The osmotic pressure is 8.85 atm

the electronic configuration of an atom with eight electrons is 1s²2s²2p⁴. the orbital diagrams are shown in the figure.

as per the hunds rule:

1. electrons tend to avoid being in the same orbital as per as practicable.

2. electrons in different orbitals of the same energy will have their spin parallel.

this can be illustrated from the multiplicity of the orbitals of the atom. as there are four electrons in the p orbital and p orbital has 3 sub-shells. the electrons can be fed in different ways as shown in the figure but the correct orbital diagram will be as per the hunds rule.

the volume increases