Question

Calculate the osmotic pressure of a 0.237m aqueous solution of sucrose, c12h22o11, at 37 degrees celsius

Answer 1

Answer is: the osmotic pressure of aqueous solution of sucrose is 6.032 atm.
c(C₁₂H₂₂O₁₁) = 0.237 mol/L; concentration of solution.
T(C₁₂H₂₂O₁₁) = 37°C = 310.15 K; temperature in Kelvins.
R = 0.08206 L·atm/mol·K; universal gas constant.
π = c(C₁₂H₂₂O₁₁) · T(C₁₂H₂₂O₁₁) · R.
π = 0.237 mol/L · 310.15 K · 0.08206 L·atm/mol·K.
π = 6.032 atm · 101.325 kPa/atm = 611.2 kPa

Answer 2

The study of the chemical and bond is called chemistry. There are different types of elements and these are metals and nonmetals.

The correct answer 611.2kPa

What is osmotic pressure?

• Osmotic pressure is the minimum pressure that needs to be applied to a solution to prevent the inward flow of its pure solvent across a semipermeable membrane.
• It is also defined as the measure of the tendency of a solution to take in a pure solvent by osmosis

The is the osmotic pressure of an aqueous solution of sucrose is 6.032 atm.

• c(C₁₂H₂₂O₁₁) = 0.237 mol/L; concentration of solution.
• T(C₁₂H₂₂O₁₁) = 37°C = 310.15 K; temperature in Kelvins.
• R = 0.08206 L·atm/mol·K; universal gas constant.

π = $c(C_{12}H_{22}O_{11}) * T(C_{12}H_{22}O_{11}) * R.$

π =$0.237 mol/L *310.15 K * 0.08206$

π = $6.032 atm * 101.325 kPa/atm = 611.2 kPa$

Hence, the correct answer is 622.1kPa.

For more information about the osmotic pressure, refer to the link:-

https://brainly.com/question/9864045