Practicing Success
A set of solutions is prepared using 180 g of water as a solvent and 10 g of different non-electrolyte and non-volatile solutes A,B and C. What is the correct order of relative lowering of vapour pressure? (Given: molar mass of A = 100 g/mol, B = 200 g/mol, C = 10000 g/mol respectively) |
A>B>C B>C>A C>B>A A>C>B |
A>B>C |
The correct answer is option 1. A>B>C. The relative lowering of vapor pressure (\( \pi \)) for a dilute solution is given by: \(\pi = \frac{{\Delta P}}{{P_0}} = \frac{{n_1}}{{n_1 + n_2}} \) Where: \( \Delta P \) is the lowering of vapor pressure, \( P_0 \) is the vapor pressure of the pure solvent, \( n_1 \) and \( n_2 \) are the number of moles of solvent and solute respectively. The number of moles of solute can be calculated using the given mass and molar mass of each solute: \(n_2 = \frac{{\text{Mass of solute}}}{{\text{Molar mass of solute}}} \) Given: Mass of water (solvent) = 180 g Mass of solute: For solute A = 10 g For solute B = 10 g For solute C = 10 g Molar mass of solute: For solute A = 100 g/mol For solute B = 200 g/mol For solute C = 10000 g/mol For solute A: \( n_2^A = \frac{{10 \, \text{g}}}{{100 \, \text{g/mol}}} = 0.1 \, \text{mol} \) For solute B: \( n_2^B = \frac{{10 \, \text{g}}}{{200 \, \text{g/mol}}} = 0.05 \, \text{mol} \) \(n_2^C = \frac{{10 \, \text{g}}}{{10000 \, \text{g/mol}}} = 0.001 \, \text{mol} \) Now, let's calculate the relative lowering of vapor pressure for each case: \( \pi^A = \frac{{n_2^A}}{{n_1 + n_2^A}} = \frac{{0.1}}{{0.1 + 180}} \) For solute B: \(\pi^B = \frac{{n_2^B}}{{n_1 + n_2^B}} = \frac{{0.05}}{{0.05 + 180}} \) \(\pi^C = \frac{{n_2^C}}{{n_1 + n_2^C}} = \frac{{0.001}}{{0.001 + 180}} \) By comparing the values, we find: \(\pi^A > \pi^B > \pi^C \) |