A. Internal Energy
If the steel is at a temperature of 20oC, you can hold it in your hand. If it is at a temperature of 200oC, you cannot hold it in your hand very long. Clearly, the ball at 200oC produces effects which the ball at 20oC cannot. Yet, if we measure the mass of the ball, it is the same at 20oC as it is at 200oC (within the precision of current measuring techniques). If we could label the atoms when the ball was at 20oC and take a census of them when the ball was at 200oC, we would find exactly the same atoms present. Therefore, the difference between what the ball will do at 20oC and what it will do at 200oC is not dependent on changing the mass or identify of the matter present. Something else obviously is involved. For now we say that a body which is hot possesses more internal energy that the same body does when cold.
Now suppose that instead of an iron ball we have a balloon which contain a mixture of gasoline and oxygen with a total mass of 1 kg at 20oC. Now we can introduce a small spark, and the contents of the balloon become very hot (explosively so). After a moment the contents will be much hotter than at the start, and they will have a different chemical composition; instead of being oxygen and gasoline, they will be carbon dioxide and water vapor. Clearly the oxygen-gasoline mixture at 20oC can produce effects that the mixture of carbon dioxide and water (when cooled to 20oC) could not. Therefore, there must be a different in energy. This we classify also as a change of internal energy.
Thus, an approximate rule (with exceptions to be seen later) is the internal energy is a measure of hotness plus the ability to cause heat releasing chemical reactions.