Chapter 6 - Thermochemistry

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33 Terms

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Thermochemistry

Study of energy exchange in chemical/physical changes.

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Energy

Capacity to do work.

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Potential Energy

Energy due to position or composition.

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Kinetic Energy

Energy due to motion.

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Thermodynamics

Study of energy and energy transformations.

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System

Part of the universe being studied.

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Surroundings

Everything outside the system.

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Universe

System + Surroundings.

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Internal Energy (E)

Sum of kinetic and potential energies in a system.

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ΔE

Change in internal energy = Efinal - Einitial.

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First Law of Thermodynamics

Energy is conserved; ΔEuniv = ΔEsys + ΔE_surr = 0.

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Heat (q)

Energy transferred due to temperature difference.

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Work (w)

Energy transfer by force/motion (e.g., expansion).

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ΔE formula

ΔE = q + w

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Sign of q

  • if heat gained, - if heat lost.
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Sign of w

  • if work done on system, - if by system.
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Energy unit

Joule (J)

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1 J

1 J = 1 kg·m²/s²

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Calorie

1 cal = 4.184 J

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Nutritional Calorie

1 Cal = 1000 cal = 1 kcal

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State Function

Property depending only on current state, not path (e.g., ΔE, T, P).

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PV Work

w = –PΔV

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Enthalpy (ΔH)

Heat change at constant pressure; ΔH = q_p.

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ΔH formula

ΔH = Hproducts - Hreactants

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Exothermic

Releases heat; ΔH < 0

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Endothermic

Absorbs heat; ΔH > 0

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Specific Heat (c)

Heat to raise 1 g of substance by 1°C or 1 K.

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Molar Heat Capacity

Heat to raise 1 mol of substance by 1°C or 1 K.

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Specific Heat of Water

c = 4.184 J/g·K = 1 cal/g·K

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Heat Formula

q = c × m × ΔT

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Calorimeter

qreaction = –qH₂O

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Thermochemical Equation

Includes ΔH value in balanced equation.

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Hess’s Law

ΔH_total = sum of ΔH of steps.