Question

challenge me questions 1-5: as you explore the simulation, answer the following questions. 1. does the temperature of the water rise while it is boiling? 2. what is the relationship between molecular motion and energy? 3. when you boil water, why does the level of liquid decrease? 4. label each arrow using the following words: melting, freezing, sublimation, deposition, condensation, and evaporation. 5. can pure water exist as a liquid at 110°c? why or why not?

Explanation:

1. During boiling, water remains at its boiling - point temperature (100°C at standard atmospheric pressure) and the heat energy is used for the phase change from liquid to gas, not for temperature rise.
2. The more energy molecules have, the more vigorously they move. Kinetic energy of molecules is related to their motion. Higher energy means higher - speed and more random motion.
3. When water boils, it changes from the liquid phase to the gas phase (evaporates). The gas molecules escape into the atmosphere, reducing the amount of liquid water, thus the liquid level decreases.
4. Gas to Liquid: condensation; Liquid to Gas: evaporation; Liquid to Solid: freezing; Solid to Liquid: melting; Solid to Gas: sublimation; Gas to Solid: deposition.
5. At standard atmospheric pressure (1 atm), pure water boils at 100°C and turns into gas. But at higher pressures, the boiling - point of water increases. So, at pressures above 1 atm, pure water can exist as a liquid at 110°C.

Answer:

1. No.
2. The more energy molecules have, the more they move.
3. Because water evaporates into gas and escapes.
4. Gas to Liquid: condensation; Liquid to Gas: evaporation; Liquid to Solid: freezing; Solid to Liquid: melting; Solid to Gas: sublimation; Gas to Solid: deposition.
5. At standard pressure, no. But at higher pressures, yes.