Question 12.7: Calculate the vapor pressure of a solution made by dissolvin...
Calculate the vapor pressure of a solution made by dissolving 218 g of glucose (molar mass = 180.2 g/mol) in 460 mL of water at 30°C. What is the vapor-pressure lowering? The vapor pressure of pure water at 30°C is given in Table 5.3. Assume the density of the solvent is 1.00 g/mL.
Temperature (°C) |
Water Vapor Pressure (mmHg) |
0 | 4.58 |
5 | 6.54 |
10 | 9.21 |
15 | 12.79 |
20 | 17.54 |
25 | 23.76 |
30 | 31.82 |
35 | 42.18 |
40 | 55.32 |
45 | 71.88 |
50 | 92.51 |
55 | 118.04 |
60 | 149.38 |
65 | 187.54 |
70 | 233.7 |
75 | 289.1 |
80 | 355.1 |
85 | 433.6 |
90 | 525.76 |
95 | 633.9 |
100 | 760 |
Strategy We need Raoult’s law [Equation (12.4)] P_{1}=X_{1} P^{°}_{1} to determine the vapor pressure of a solution. Note that glucose is a nonvolatile solute.
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