Imagine a room. In one corner, there's a hot cup of cocoa; in the other, an ice-cold soda. Entropy helps us understand what's happening between them!

• Entropy (S) is all about order and disorder. Cool objects are more orderly, while hot ones are a bit chaotic!
• It can be viewed from two angles: the big view (macroscopic) and the tiny view (microscopic).

Entropy is represented by S. When something reversible happens, we use the formula: ΔS=\(\frac {ΔQ}{T}\)​ Here:

• ΔS = change in entropy
• ΔQ = energy transferred into a system
• T = temperature when the transfer happens
• Units alert! Entropy's unit is Joule per Kelvin (JK⁻¹).
• It’s like temperature or internal energy—it's a system's property.
• If a process is reversible, the entropy doesn't change! This means Δ=0ΔS=0.

🔍 Real-life Scenario: Picture a gas moving in a pipe. Before a narrowing (constriction), it's in a certain state. After the constriction? If no energy goes in or out, it's the same! No change in entropy. But! If there was friction, energy would move from the gas to the surroundings. We’d have a change in entropy!