So let's backtrack a little bit and talk about the first law of thermodynamics

which says energy cannot be created or destroyed. We know from this that the

total energy at the university is

constant. Now we can transfer energy and converted from one type to the other

but ultimately the sum of all those energies must be equal to the same constant value.

The second law of thermodynamics is a little bit different

instead of talking about energy we're talking about spontaneity,

Specifically talking about entropy and what we know is that for any spontaneous process.

The intro bf the universe increases. Processes that happen spontaneously

are those that increase the entropy of the universe. So although parts of a

process may not be spontaneous.

When we look at the entire system and its surroundings

what we find is that overall there's an increase in the entropy

of the universe . And that's what makes our spontaneous reaction spontaneous.

This will depend heavily on the temperature and as we get later in this

unit and talk about Gibbs free energy will be able to quantify that.

Next we're going to a more in-depth about what entropy really is.