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Thermochemistry
Study of energy exchange in chemical/physical changes.
Energy
Capacity to do work.
Potential Energy
Energy due to position or composition.
Kinetic Energy
Energy due to motion.
Thermodynamics
Study of energy and energy transformations.
System
Part of the universe being studied.
Surroundings
Everything outside the system.
Universe
System + Surroundings.
Internal Energy (E)
Sum of kinetic and potential energies in a system.
ΔE
Change in internal energy = Efinal - Einitial.
First Law of Thermodynamics
Energy is conserved; ΔEuniv = ΔEsys + ΔE_surr = 0.
Heat (q)
Energy transferred due to temperature difference.
Work (w)
Energy transfer by force/motion (e.g., expansion).
ΔE formula
ΔE = q + w
Sign of q
Sign of w
Energy unit
Joule (J)
1 J
1 J = 1 kg·m²/s²
Calorie
1 cal = 4.184 J
Nutritional Calorie
1 Cal = 1000 cal = 1 kcal
State Function
Property depending only on current state, not path (e.g., ΔE, T, P).
PV Work
w = –PΔV
Enthalpy (ΔH)
Heat change at constant pressure; ΔH = q_p.
ΔH formula
ΔH = Hproducts - Hreactants
Exothermic
Releases heat; ΔH < 0
Endothermic
Absorbs heat; ΔH > 0
Specific Heat (c)
Heat to raise 1 g of substance by 1°C or 1 K.
Molar Heat Capacity
Heat to raise 1 mol of substance by 1°C or 1 K.
Specific Heat of Water
c = 4.184 J/g·K = 1 cal/g·K
Heat Formula
q = c × m × ΔT
Calorimeter
qreaction = –qH₂O
Thermochemical Equation
Includes ΔH value in balanced equation.
Hess’s Law
ΔH_total = sum of ΔH of steps.