• ΔH⦵ is all about HEAT (think of a 🔥)! It's the heat transferred when reactions occur at a constant pressure under standard conditions.
• Imagine you're basking under the sun, absorbing its warmth; that's like a reaction taking in heat. But sometimes, reactions can give out heat like a campfire on a chilly night.
• Units? It's measured in kJ mol−1.

• To determine the villainous ΔH⦵, you need to track the heat either released (like a dragon breathing fire) or absorbed (like a sponge soaking up water) during a reaction.
• Measure the change in temperature of a pure substance to/from which this heat moves. Think of it like a thermometer in your soup; you watch the temp go up as it gets hotter!

• What is it? It's the heat required to raise the temp of 1 kg of a substance by 1 °C or 1 K.
• Example: Ethanol's specific heat capacity is 2.44 kJ kg−1 K−1. Imagine you've got a 1 kg pot of ethanol (don't drink it!). You'd need 2.44 kJ of energy to make it just 1 K hotter!
• Fun Fact: The smaller the "c" value, the quicker our substance heats up when given the same amount of heat.

Specific heat capacity doesn't care how big or small something is. A tiny piece of copper and a HUGE block of copper both have the same "c". What matters is:

• The substance's identity (is it water, copper, gold?).
• Its mass (heavy or light?).
• The heat given (how fierce is that dragon’s fire?).