why energy flows in certain directions and in certain ways ?
a lot of the concepts described by thermodynamics seem like common sense but there
we won't get into the math but we should be able to describe these laws conceptually the first law described in the most basic way highlights conservation of energy .
it is not created or destroyed it only changes forms from potential energy to kinetic energy to heat energy etc.
while we have found this to be untrue on the quantum level for chemists it does just fine however there seems to be a preferred direction in which energy flows from one form to another.
in order to understand why we look at the second law the second law introduces a new easily describe entropy as disorder and the second law states that the sum of the entropy of a system and its surroundings must always increase in ,other words the entropy .
within a system there is also a tendency to go towards higher entropy the classic analogy is that your bedroom will over time become messy but it won't suddenly become neat.
another way to look at this is to say that entropy is a measure of how dispersed the energy of the system is amongst the ways that system .
an ionic solid compared to the same substance as a liquid clearly the solid state is more ordered and the liquid state is more disordered or higher in entropy to describe the solid state using computer.
the liquid state you would need to simply describe the volume of liquid and the shape of the vessel because the motion and configuration of the molecules are random that's far less information that needs encoding which is a way of rationalizing why increasing the entropy of a system is thermodynamic ally .
entropy influence heat will flow from a hot coffee cup into the table or your hand because the heat energy will be more disordered if more dispersed this is why heat spontaneously flows from hot to cold and not the other way around
entropy the third law states that are perfectly crystalline solid at Absolute Zero has an entropy of zero as this is the most ordered state the substance can be in entropy is measured in joules per Kelvin note .
that entropy is not a measure of energy itself but of how energy is distributed within a system it is enthrall the thermodynamic quantity we learned about before that is more accurately describing the energy of a system as we will see enthrall and entropy intricately relate to tell us something about the Gibbs free energy of a system .
whether a process will be spontaneous or not meaning if it will simply happen on its own change in Gibbs free energy is given by this equation which includes change in enthalpy change in entropy and temperature if Delta G is negative the process is spontaneous if positive it is non spontaneous .
favorable and delta s is positive which means an increase in entropy which is also favorable a negative minus a positive will always be negative or spontaneous.
two is favorable we have to do some math if Delta H is positive or endothermic that energetic unavailability could be outweighed by the other term if the process is en tropically favorable and since T is here this factor will increase with a larger T so tropically favorable processes are more likely to be spontaneous at higher temperatures conversely.
if it is energetically favorable but en tropically unfavorable the entropy unavailability will be minimized at lower temperatures this is a very important equation to understand because it describes all of the spontaneous processes in the universe.
there are those who incorrectly use entropy and the second law of thermodynamics to imply that order can't happen spontaneously .
they are miscible with polar water molecules but soap molecules have polar heads and long non polar tails which allows them to spontaneously form structures called micelles .
these are spheres where the soap molecules orient themselves with the polar heads facing out in order to maximize ion dipole.
interactions with water molecules that bring the system to a lower energy and the non polar tails will all face in trapping the dirt by making a network interactions the dirt trapped in the my cells washes away because the micelle as a whole is water-soluble .
due to the polar heads facing out that's how soap works and that's also how highly ordered structures can form spontaneously if by enthalpically favorable or energy storing processes in this way systems can defy entropy on the small scale.
the second law does hold true in that the entropy of the universe is always increasing let's check comprehension
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entropy is often described as a measurement of disorder that's a convenient image but it's unfortunately misleading for example which is more disordered a cup of crushed ice or a glass of room-temperature.
another way of thinking about it through probability this may be trickier to understand but take the time to internalize it and you'll have a much better understanding of entropy consider two small solids which are comprised of six atomic bonds each in this model .
it is turns out that there are numerous ways that the energy can be distributed like
two solids and still have the same total energy in each each of these options is called a micro state for 6 quanta of energy in solid a and 2 in solid B there are 9702 micro states of course .
there are other ways our eight quanta of energy can be arranged for example all of the energy could be in solid a and none in B or half in a and half in B if we assume that each micro state is equally likely we can see that some of the energy configurations have a higher probability of occurring than others that's due to their greater number of micro states.
entropy is a direct measure of each energy configurations probability what we see is that the energy configuration in which the energy is most spread out between the solids has the highest entropy .
so in a general sense entropy can be thought of as a measurement of this energy spread low entropy means the energy is concentrated.
high entropy means it's spread out to see why entropy is useful for explaining spontaneous processes like hot objects cooling down we need to look at a dynamic system where the energy moves in reality .
energy doesn't stay put it continuously moves between neighboring bonds as the energy moves the energy configuration can change because of the distribution of micro states.
there's a 21% chance that the system will later be in the configuration in which the energy is maximally spread out there's a 13% chance that it will return to its starting point and an 8% chance.
that a will actually gain energy again we see that because there are more ways to have dispersed energy and high entropy than concentrated energy .
the energy tends to spread out that's why if you put a hot object next to a cold one the cold one
will warm up and the hot one will cool down but even in that example…
there is an 8% chance that the hot object would get hotter why doesn't this ever happen in real life it's all about the size of
the system our hypothetical solids only had six bonds each let's scale the solids up to 6,000 bonds and 8,000 units of energy and again start the system with three-quarters of the energy .
there's no mysterious force nudging the system towards higher entropy it's just that higher entropy is always statistically more likely that's why entropy has been called times arrow if energy has the opportunity to spread out.