Two samples of water of equal volume are put into two dishes and kept at room temperature for several days. The water in the first dish is completely vaporized after 2.8 days while the water in the second dish takes 8.3 days to completely evaporate.What can you conclude about the two dishes?
When a non-volatile solute is placed in a volatile solvent, three things happen.
1. The boiling point is raised (which doesn't apply to this problem).
2. The freezing point is lowered (which doesn't apply to this problem).
3. The vapor pressure is lowered. (Wouldn't that apply to this problem? If the vapor pressure is lowered it will take longer for it to evaporate. right?)
To continue with what my freshman chemistry teacher said, (verbatim) "and the extent to which these things happen depends solely upon the number of dissolved particles.
To analyze the situation and draw conclusions about the two dishes, we can compare the rates of evaporation. The dish in which the water completely vaporized after 2.8 days indicates a faster rate of evaporation compared to the dish where it took 8.3 days for the water to evaporate completely.
From this, we can draw the following conclusions:
1. The dish in which water evaporated in 2.8 days has a higher rate of evaporation compared to the dish in which it took 8.3 days.
2. Factors such as temperature, humidity, air movement, and surface area can affect the rate of evaporation.
Remember, the information you have provided only relates to the evaporation rate of water in the two dishes. To make more precise conclusions, you could also consider other factors, such as the initial volume of water in each dish, the presence of impurities, or differences in the environment surrounding the dishes.