Compare entropy in solids, liquids, and gases.
Solids: Low entropy (tightly packed) | Liquids: Medium entropy (more movement) | Gases: High entropy (particles move freely).
Differentiate between spontaneous and non-spontaneous processes.
Spontaneous: Occurs naturally, increases overall entropy | Non-spontaneous: Requires energy input, decreases overall entropy.
Compare the entropy of a tidy room vs. a messy room.
Tidy room: Low entropy, ordered | Messy room: High entropy, disordered.
Compare energy quality in different energy transformations.
High quality: Minimal energy lost as heat | Low quality: Significant energy lost as heat.
Compare the number of gas molecules on the reactant side vs. the product side when predicting the sign of ฮS.
More gas molecules on the reactant side: ฮS is positive | Fewer gas molecules on the reactant side: ฮS is negative.
What is Entropy (S)?
A measure of disorder or randomness in a system, reflecting the number of possible arrangements.
Define the Law of Conservation of Energy.
Energy cannot be created or destroyed; it only changes form. Total energy in an isolated system remains constant.
What is absolute zero?
0 K or -273.15ยฐC, the point at which entropy is zero and all molecular motion stops.
Define spontaneous process.
A process that occurs on its own without any external energy input.
What does a higher entropy indicate?
A more chaotic or disordered system.
What is the effect of increasing temperature on the spontaneity of an exothermic reaction?
Decreases spontaneity because the -TฮS term becomes more significant.
What happens to entropy as a substance changes from solid to liquid to gas?
Entropy increases.
What is the effect of energy changing form?
Some energy is lost as heat to the surroundings.
What happens when ฮG is negative?
The reaction is spontaneous.
What happens to entropy at absolute zero?
Entropy is zero.
