Editing Physical Chemistry (section)

== <span style="color: #FFFFFF;">Analyzing</span> ==
{| class="wikitable"
|+ Spontaneity and Energy
! ΔH (Heat) !! ΔS (Disorder) !! Spontaneous? (ΔG < 0)
|-
| Negative (Exothermic) || Positive || Always (e.g., combustion)
|-
| Positive (Endothermic) || Negative || Never
|-
| Negative || Negative || At low temperatures
|-
| Positive || Positive || At high temperatures (e.g., ice melting)
|}

'''Le Chatelier's Principle''': If a system at equilibrium is disturbed, the system will shift its position to counteract the disturbance. If you add more reactant, the system makes more product. If you increase the pressure, it shifts toward the side with fewer gas molecules. This "logic of change" is used in industrial chemistry (like the Haber process for fertilizer) to maximize production.
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