The osmotic pressure at 65 °C of an aqueous solution containing 2.50 g of sucrose is 0.988 atm
<h3>How to determine the mole of sucrose </h3>
- Mass of sucrose = 2.5 g
- Molar mass of sucrose = 342 g/mol
- Mole of sucrose =?
Mole = mass /molar mass
Mole of sucrose = 2.5 / 342
Mole of sucrose = 0.0073 mole
<h3>How to determine the molarity of sucrose </h3>
- Mole of sucrose = 0.0073 mole
- Volume = 205 mL = 205 / 1000 = 0.205 L
Molarity =?
Molarity = mole / Volume
Molarity of sucrose = 0.0073 / 0.205
Molarity of sucrose = 0.0356 M
<h3>How to determine the osmotic pressure </h3>
- Molarity (M) = 0.0356 M
- Temperature (T) = 65 °C = 65 + 273 = 338 K
- Gas constant (R) = 0.0821 atm.L/Kmol
- Van't Hoff factor (i) = 1 (sucrose is non-electrolyte)
- Osmotic pressure (π) =?
π = iMRT
π = 1 × 0.0356 × 0.0821 × 338
π = 0.988 atm
Learn more about Osmotic pressure:
brainly.com/question/5925156
