Chemistry- Basic Energy Transfer Questions

[uestions]

Why does no temperature change occur while ice is melting? Specifially, when very little ice is left, how does so much water remain at 0 degrees Celcius?

Is the energy transfer (of heat) to ice constant? Specifically, does the time range in an exponential manner for different sizes of ice to melt? (Say a large chunk of ice is put over a flame. When it gets to be 1/6 of its original size form melting, does the liquid water surrounding the cube transfer more energy to the small cube because there is so much water to give energy that at the beginning of melting when there was less water?)

When given the explanation "the heat energy breaks down the bonds that hold the particles together," what does "break down" mean? (Does the heat cause particles to move with so much force that they escape attraction, or does heat actually destroy some chemical bond holding solid water particles together?)

Is the temperature of ice water an average of the liquid water and ice (i.e. ice = -0.5 degrees Celcius and water = 0.5 degrees Celcius) or are ice and water both have averages of 0 degrees Celcius and therefore average to 0 degrees?



I thought about this stuff and looked online, but all answers were the same. I think velocity has to do with causing phase change, and I'm missing something in understanding the lack of temperature change. All I can think of is the liquid water particles collide with ice and transfer energy to ice causing ice to melt. But, them the melting times for different sizes of ice wouldn't be constant because with more ice melted, there would be more water to transfer energy, and then the small ice chunk would melt quicker. On the same point, chemistry equations and heating curves state otherwise.
As for temperature, I think again the thermall energy form the liquid water particles would "transfer" to solid water particles, the solid then gaining phase energy.
Anyone willing to help?

 

[Borek]

Say a large chunk of ice is put over a flame. When it gets to be 1/6 of its original size form melting, does the liquid water surrounding the cube transfer more energy to the small cube because there is so much water to give energy that at the beginning of melting when there was less water?

Quite the opposite - smaller piece of ice gets less energy per unit of time than the large one, as as energy transfer takes place through the ice surface, and smaller piece has a smaller surface than the large one.

Does the heat cause particles to move with so much force that they escape attraction, or does heat actually destroy some chemical bond holding solid water particles together?

Is there a difference between both scenarios?

When we say the bath has a temperature of 0°C we refer to the equilibrium situation, when the amount of ice in the mixture is staying constant. As long as the ice is melting, water temperature can be not not zero. Otherwise, if they had both exactly the same temperature there would be by definition no energy transfer - so no melting would be possible.

 

[uestions]

Thank you!

 

[uestions]

The difference between scenarios is ice particles pull themselves apart compared to a bond "disintegrating" and then particles are free to separate.

 

[DeeNos]

I can provide some explanations for the questions posed about basic energy transfer in chemistry.

Firstly, why does no temperature change occur while ice is melting? This is because during the phase change from solid to liquid, the energy being added is being used to break the bonds between the particles rather than increasing the temperature. This is known as the latent heat of fusion. Once all the bonds are broken and the ice has fully melted, then the temperature can start to increase again.

When very little ice is left, how does so much water remain at 0 degrees Celsius? This is due to the fact that the energy being added is still being used to break the bonds between particles. Even though there is less ice left, the remaining ice still requires the same amount of energy to fully melt. This is why the temperature remains constant even with very little ice left.

Is the energy transfer (of heat) to ice constant? The energy transfer is not constant, but it does follow a specific pattern. As the ice melts, the amount of energy being transferred increases, as there is more water available to transfer energy. This is why the melting time for different sizes of ice is not constant, but rather increases as the ice gets smaller.

When given the explanation "the heat energy breaks down the bonds that hold the particles together," what does "break down" mean? In this context, "break down" means that the heat energy is providing enough energy to overcome the forces of attraction between the particles and break the bonds that hold them together. This allows the particles to move freely and change into a different phase.

Is the temperature of ice water an average of the liquid water and ice? The temperature of ice water is an average of the two, as the ice and water are in thermal equilibrium with each other. This means that they are exchanging energy until they reach the same temperature, which in this case is 0 degrees Celsius.

In summary, energy transfer in chemistry involves breaking bonds between particles during phase changes, and the temperature remains constant until all the bonds are broken. The energy transfer is not constant, but rather increases as the phase change progresses. And finally, the temperature of a mixture in thermal equilibrium is an average of the temperatures of the individual components. I hope this helps clarify some of the concepts in basic energy transfer in chemistry.