How much energy is needed to boil 32,500 mg of H2O at 100°C?

Phase changes in pure water occur at a specific temperature. At 1 atm, water freezes at 0° C and boils at 100° C. The energy required to change water from a liquid to a solid is 333.7 kJ/kg while the energy required to boil water is 2257 kJ/kg. The amount of energy needed to change the phase of water to a gas from a liquid is 540 times the amount of energy needed to raise the same amount of water 1° C.  

The reason so much heat needs to be added for a phase change can be understood by looking at the molecules of water. When you look closely at the molecules in a liquid, the molecules are relatively close together and they have a little room to jiggle. As you increase the temperature, the atoms continue to jiggle more and more, which causes an increase in the temperature.

At some point, the temperature stop changing and it reaches a plateau. This is where the molecules have moved as far apart from each other as they possibly can. Any additional energy that is added to the system goes into overcoming the attractive forces the molecules have on each other. When the attractive forces are overcome, some of the water molecules are able to escape which results in the water boiling.

Explanation:

alkaline metals are lithium, sodium, rubidium, potassium, cesium and francium.

alkali metals have electronegativity from 0.7 to 1, lowest in periodic table of elements, which means that alkali metals (i group in periodic table) has positive oxidation number in compounds.

electronegativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself.

alkaline metals (far left in main group) have lowest ionizations energy and easy remove valence electrons,

for example, potassium is the alkali metal and has a single valence electron in the outer electron shell.

electron configuration of potassium is: ₁₉k 1s²2s²2p⁶3s²3p⁶4s¹.

they can not exist alone in nature, because they are very reactive.