Starting as a solid at -25°C, a sample of water is heated at a constant rate until the sample is at 125°C. This heating occurs at standard pressure. The graph below represents the relationship between temperature and heat added to the sample.
Heating Curve for H2O
125
F
D
100.
E
75
Temperature (°C)
50.
25
BC
0-
-25-
<
12
20.
28
36
44
52
60.
Heat Added (kJ)
a. Explain, in terms of heat of fusion and heat of vaporization, why the heat added during interval DE is greater than the heat added
during BC for this sample of water.
b. Describe what happens to both the potential energy and the average kinetic energy of the molecules in the water sample duirng
interval AB
c. Using the graph, determine the total amount of heat added to the sample during interval

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the enthalpy of formation of water is given as -285.8kj/mol, which states that the enthalpy of formation is negative.

negative enthalpy of formation indicates that the heat is released during the reaction process. the heat is released from reaction to the surroundings the enthalpy is expressed with a negative sign with the energy given out in the reaction process.

the formation of water takes place by giving out heat which is -285.8 kj/mol.

d

explanation:

the seeing the electronic configuration we can say that the element is fluorine.

fluorine is the most electronegative element in the periodic table.

but by only seeing the configuration we cannot say about its reactivity because we don't know if its configuration after excitation or by addition of electrons.

but if not then, it is the lightest halogen and exists as a highly toxic pale yellow diatomic gas at standard conditions. as the most electronegative element, it is extremely reactive: almost all other elements, including some noble gases, form compounds with fluorine.