Chapter 5 - Thermochemistry Flashcards
Specific heat of water
4.18 J/g K
Density of water
1 g/mL
Heat (q) =
the amount of energy transferred from one object to another because of a difference of temperature
Enthalpy (H) =
the amount of energy transferred from one object to another because of a difference of temperature at a constant pressure!
q = mC∆T
heat (Joules) = mass(g) x Specific Heat x Change in Temperature
Used when temperature is changing
q = -q when someone absorbs and other releases energy
q = m∆H
heat (kilojoules) = mass(g) x ∆H(corresponding to the phase change ie evaporation, condensation, fusion, etc)
Used when changing state of matter
Hess’s law
∆H is directly proportional to the number of moles, therefore if you increase or decrease the chemical reaction, the ∆H will also change by the same factor. You can also reverse the equation, which would also reverse the value of ∆H (make it negative)
Standard Enthalpy of Formation
ΔH° = Σ(n × ΔHf°) (products) - Σ(n × ΔHf°) (reactants)
1 atm and 25 C