What is the osmotic pressure of a solution containing 0.1 moles of solute in 1 liter of solution at 25 °C? (R = 0.0821 L·atm/(K·mol)) (2020)

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Q: What is the osmotic pressure of a solution containing 0.1 moles of solute in 1 liter of solution at 25 °C? (R = 0.0821 L·atm/(K·mol)) (2020)

Solution: Osmotic pressure (π) = nRT/V = (0.1 moles * 0.0821 * 298) / 1 = 2.5 atm.

Steps: 6

Step 1: Identify the formula for osmotic pressure, which is π = nRT/V.
Step 2: Determine the values needed for the formula: n (number of moles) = 0.1, R (gas constant) = 0.0821 L·atm/(K·mol), T (temperature in Kelvin) = 25 °C + 273 = 298 K, and V (volume in liters) = 1.
Step 3: Plug the values into the formula: π = (0.1 moles * 0.0821 L·atm/(K·mol) * 298 K) / 1 L.
Step 4: Calculate the numerator: 0.1 * 0.0821 * 298 = 2.47598.
Step 5: Since the volume is 1 L, the osmotic pressure is π = 2.47598 atm.
Step 6: Round the answer to two decimal places: π ≈ 2.5 atm.