{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

Chapter 5 Notes

# Chapter 5 Notes - Enthalpy change for a reaction is equal...

This preview shows pages 1–2. Sign up to view the full content.

Chapter 5 Thermochemistry The First Law of Thermodynamics Energy is conserved Internal Energy ΔE=E final - E initial Relating E to Heat and Work ΔE= q + w When heat is added to a system or work is done ON a system, its internal energy increases Endothermic and Exothermic Processes Endothermic- absorbs heat Exothermic- loses heat State Functions Value of a state function depends on the present state of system, not on path the system took to reach that state Enthalpy w= -PΔV enthalpy accounts for heat flow in processes occurring at constant pressure when no forms of work are performed other than P-V work H= E+ PV ΔH=q p , change in enthalpy equals heat gained or lost at constant pressure Enthalpies of Reaction ΔH = H products - H reactants Enthalpy is an extensive property

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: Enthalpy change for a reaction is equal in magnitude, but opposite in sign, to ΔH for the reverse reaction The enthalpy change for a reaction depends on the state of the reactants and products Chapter 5 Thermochemistry Calorimetry Heat Capacity and Specific Heat Specific heat (s) = q/ (m*ΔT) q= mcΔT Constant Pressure Calorimetry q soln = -q rxn Bomb Calorimetry Hess’ Law If a reaction is carried out in a series of steps, ΔH for the overall reaction will equal the sum of the enthalpy changes for the individual steps Enthalpies of Formation ΔH˚ rxn = ΣnΔH˚ f (products) - ΣmΔH˚ f (reactants) Foods and Fuels Fuel value of a substance is heat released when 1 g is combusted...
View Full Document

{[ snackBarMessage ]}

### Page1 / 2

Chapter 5 Notes - Enthalpy change for a reaction is equal...

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document
Ask a homework question - tutors are online