l 1. As indicated in figure 8 a given pure substance at room temperature (20°C) was heated. While heating the pure substance, the temperature started to rise up. After 7 minutes, the temperature reached 70°C and stayed as it is even when heated for 30 minutes more. What does the 70°C indicate?
2. A given mixture at room temperature (20°C) was heated. On a 15 minute duration of being subjected to heat, its temperature steadily increased and stopped changing at 50°C for about 20 minutes. However, the mixture's temperature increased again and eventually stopped at 100°C even after being heated for 30 minutes more as shown in figure 9. Why does the given mixture exhibit two constant temperature readings for a certain amount of time?
2. A given mixture at room temperature (20°C) was heated. On a 15 minute duration of being subjected to heat, its temperature steadily increased and stopped changing at 50°C for about 20 minutes. However, the mixture's temperature increased again and eventually stopped at 100°C even after being heated for 30 minutes more as shown in figure 9. Why does the given mixture exhibit two constant temperature readings for a certain amount of time?
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Answer:
Evaporation is a phase transition from the liquid phase to the gas phase that occurs at temperatures below the boiling point at a given pressure.
For molecules of a liquid to evaporate, they must be located near the surface, be moving in the proper direction, and have sufficient kinetic energy to overcome liquid-phase intermolecular forces.
Boiling is a phase transition from the liquid phase to the gas phase that occurs at or above the boiling temperature.
Boiling is the rapid vaporization of a liquid and occurs when a liquid is heated to its boiling point. A liquid’s boiling point is the temperature at which the vapor pressure of the liquid is equal to the pressure exerted on the liquid by the surrounding environment (air).
Explanation:
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