Chapter 5 Memory bank

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Last updated 11:33 AM on 8/4/26
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25 Terms

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U

internal energy

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ΔU

change in internal energy

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q

heat

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w

work

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H

enthalpy

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ΔH

enthalpy change

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m

mass

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c or s

specific heat capacity

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C_cal

calorimeter heat capacity

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ΔT

T_f - T_i

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ΔH_f^°

standard enthalpy of formation

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q > 0

the system absorbs heat

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q < 0

the system releases heat

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w > 0

work is done on the system

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w < 0

work is done by the system

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ΔH < 0

exothermic

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ΔH > 0

endothermic

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first law of thermodynamics

ΔU = q + w

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heating or cooling equation

q = mcΔT

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calorimeter equation

q_cal = C_calΔT

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energy-conservation equation

q_rxn = -q_surroundings

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formation-enthalpy equation

ΔH_rxn^° = ΣνΔH_f^°(products) - ΣνΔH_f^°(reactants)

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Hess's law: reverse a reaction

reverse the sign of ΔH

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Hess's law: multiply an equation

multiply ΔH by the same factor

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Hess's law: add equations

add their ΔH values