What happens to the temperature of a substance while it is undergoing a change of state?

Answer 1

It can lose or gain energy or it forms the attractions between particles.

Answer 2

Overall the temperature and randomness of the molecules changes according to the absorption or expulsion of energy in the form of heat while changing states of matter. For example, when changing from a liquid to a gas, energy is needed, which increases the temperature of the substance, and therefore the energy it absorbs increases the molecules randomness (i.e. change of state from more ordered liquid to a random gas).

A change in state, from either a solid, liquid, or gas, is fundamentally caused by the absorption of energy in the form of heat. To demonstrate the energy involvement, you can calculate the amount of heat in Joules absorbed by a substance over a temperature or state change. For example, if i had a sample of ice that weighed 32g I could calculate the amount of energy needed to change that sample from ice (bellow/at 0 degrees C) to a gas (above/at 100degrees C). To do so, I am going to give an example of changing that sample from (-10)degrees Celsius to (200)degrees Celsius. to do so i must first change it from a solid to a liquid, by using the formula: q=(m)(s)(deltaT). So to go from -10 to 0 degrees C, you are increasing the temperature bu 10 degrees. The mas of the sample is 32g (as previously stated) and we know the specific heat of ice is 2.09J/g*degree C. So multiply 32 by 2.09 and then 10. which equals 668.8 J then to calculate the energy needed to go from 0degrees in a solid to 0degrees in the liquid (the transition period, called delta H of fusion). So multiply the moles of water by 6.8 kJ/mol (the delta H of fusion). water is 18.014g/mol so divide 32g by this number to get the number of moles which equals about 1.77639moles, times 6.8KJ/mol, which = 12.0795KJ. this is in kilo Joules so divide by 1000 to get the Joules number. then going from a liquid to a gas, use (m)(s)(deltaT) s in a liquid water is 4.184j/g*degrees C and a temp. change of 100 degrees C, which = 13376J, then find the delta H of vaporization, which for water is about 40.8KJ/mol- multiply it by the same value of moles = 72.476712 KJ. then go from 100 to 200 degrees C with the specific heat of gas being 2.01J/g*degree C. and the mass of the sample (32g). = 6432J.

Now add all the values for the multistage problem and find the KJ=

105.03KJ are needed to change 32g of ice from -10 degrees Celsius to 200 degrees Celsius.

The specific heat capacity is the amount of energy required to raise the temperature of one gram of a substance by one degree Celsius.

Answer 3

The temperature of the material stays the same.

Answer 4

As a substance changes state the temperature remains constant. The graph above is inaccurate

Answer 5

The temperature rises or drops depending on the state that it is changing into.

Answer 6

temperature decreases