How many grams of sucrose (C₁₂H₂₂O₁₁, 342.3 g/mol)would be needed to make 2.5 L of a solution with an osmotic pressure of 14 atm at 25°C? (R = 0.0821 L.atm/K.mol) A)0.57 g B)6.8 g C)2.0 × 10² g D)4.9 × 10² g E)5.8 × 10³ g

Question

Quizplus · Accepted Answer

First, we need to use the Van't Hoff equation to calculate the number of moles of sucrose required to achieve an osmotic pressure of 14 atm at 25°C:
Π = iMRT
14 atm = (1)(Molarity)(0.0821 L atm/mol K)(298 K)
Molarity = 0.592 M
Next, we can calculate the number of moles of sucrose required to make 2.5 L of a 0.592 M solution:
moles sucrose = Molarity x volume
moles sucrose = 0.592 mol/L x 2.5 L
moles sucrose = 1.48 mol
Finally, we can use the molar mass of sucrose to convert moles to grams:
grams sucrose = moles x molar mass
grams sucrose = 1.48 mol x 342.3 g/mol
grams sucrose = 505.284 g
Therefore, the answer is D, 4.9 × 10¹² g (in scientific notation).

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How Many Grams of Sucrose (C₁₂H₂₂O₁₁, 342