take a bowl of ice and put in ditect sunshine and note its temperature after five minutes ?what type of change in its temperatre do you observe ?how much time it take to melt completely ? and put the same water on the stove and note its temperature after thirty seconds what type of change in its temperature do you observe now ?how much time it take to boil?explain your observation with the help of time and temperature chart ?performed this experiment on a sunny day
Answers
The system is constructed so that no vapor evaporates while ice warms to become liquid water, and so that, when vaporization occurs, the vapor remains in of the system. The long stretches of constant temperature values at 0ºC and 100ºC reflect the large latent heat of melting and vaporization, respectively.
Answer:
When boiling occurs, the more energetic molecules change to a gas, spread out, and form bubbles. ... Therefore the temperature of the liquid remains constant during boiling. For example, water will remain at 100ºC (at a pressure of 1 atm or 101.3 kPa) while boiling.
Answer:
If the ambient temperature around a piece of ice increases, the temperature of the ice will increase as well. However, this steady increase in temperature stops as soon as the ice reaches its melting point. At this point, the ice undergoes a change of state and turns into liquid water, and its temperature won't change until all of it has melted. You can test this with a simple experiment. Leave a cup of ice cubes in a hot car and monitor the temperature with a thermometer. You'll find that the icy water remains at a frosty 32 degrees Fahrenheit (0 degrees Celsius) until all of it has melted. When that happens, you'll notice a quick temperature rise as the water continues to absorb heat from the inside of the car.
TL;DR (Too Long; Didn't Read)
When you heat ice, its temperature rises, but as soon as the ice starts to melt, the temperature stays constant until all the ice has melted. This happens because all the heat energy goes into breaking the bonds of the ice's crystal lattice structure.
Phase Changes Consume Energy
When you heat ice, the individual molecules gain kinetic energy, but until the temperature reaches the melting point, they don't have energy to break the bonds that hold them in a crystal structure. They vibrate more quickly within their confines as you add heat, and the temperature of the ice goes up. At a critical point – the melting point – they acquire enough energy to break free. When that happens, all the heat energy added to the ice is absorbed by H2O molecules changing phase. There's nothing left to increase the kinetic energy of the molecules in the liquid state until all the bonds holding the molecules in a crystal structure have been broken. Consequently, the temperature remains constant until all the ice has melted.
The same thing happens when you heat water to the boiling point. The water will heat until the temperature reaches 212 F (100 C), but it won't get any hotter until it has all turned to steam. As long as liquid water remains in a boiling pan, the temperature of the water is 212 F, no matter how hot the flame underneath it is.