osmotic pressure?
2019-02-20 7:07 am
What mass of sucrose (C12H22O11) should be combined with 468 g of water to make a solution with an osmotic pressure of 8.35 atm at 270 K? (Assume the density of the solution to be equal to the density of the solvent.)
回答 (2)
2019-02-20 11:49 am
✔ 最佳答案
Supposing the sucrose does not hydrolyze:(8.35 atm) / (0.082057338 L atm/K mol) / (270 K) x (342.2965 g C12H22O11/mol) = 129.005 g/L
(129.005 g/L) x ((z g + 468 g) / (1000 g/L)) = z g
Solve for z algebraically:
z = 69.3 g C12H22O11
2019-02-20 10:56 am
Density of water = 1.00 g/mL
Volume of water = (468 g) / (1.00 g/mL) = 468 mL = 0.468 L
Volume of the solution = Volume of water = 0.468 L
Molar mass of C₁₂H₂₂O₁₁ (sucrose) = (12.0×12 + 1.0×22 + 16.0×11) g/mol = 342 g/mol
Osmotic pressure, Π = 8.35 atm
Gas constant, R = 0.08206 L atm / (mol K)
Temperature, T = 270 K
Molarity, M = ? mol/L
Π = MRT
M = Π/(RT)
M = 8.35 / (0.08206 × 270) mol/L
Mass of sucrose = [8.35 / (0.08206 × 270) mol/L] × (342 g/mol) × (0.468 L) = 60.3 g
Volume of water = (468 g) / (1.00 g/mL) = 468 mL = 0.468 L
Volume of the solution = Volume of water = 0.468 L
Molar mass of C₁₂H₂₂O₁₁ (sucrose) = (12.0×12 + 1.0×22 + 16.0×11) g/mol = 342 g/mol
Osmotic pressure, Π = 8.35 atm
Gas constant, R = 0.08206 L atm / (mol K)
Temperature, T = 270 K
Molarity, M = ? mol/L
Π = MRT
M = Π/(RT)
M = 8.35 / (0.08206 × 270) mol/L
Mass of sucrose = [8.35 / (0.08206 × 270) mol/L] × (342 g/mol) × (0.468 L) = 60.3 g
收錄日期: 2021-05-01 22:29:01
原文連結 [永久失效]:
https://hk.answers.yahoo.com/question/index?qid=20190219230703AAFEGkX