energetics Flashcards
enthalpy change
the heat energy change measured under conditions of constant pressure
standard enthalpy change
the standard conditions (e.g 100 KPA and 298 K)
standard enthaply of combustion
enthalpy change when 1 mole of a substance is completely burned in oxygen with all reactants and products in standards states under standard conditions
standard enthalpy of formation
the enthalpy change when one mole of a compound is formed from its elements with all products and reactants in their standard states under standard conditions
equations of energy change in water
q= mc deltat
(remember only include mass of water in equation calc)
energy change in water (q)
joules
mass of water (m)
grams
SHC (c)
4.18
temperature of water (delta t)
degrees C = K
enthalpy equation
-q over n
n = number of moles
units = KJ mol -1
hess’s law
states that the enthalpy change for a chemical reaction is independent of route taken
combustion
arrows DOWN
co2 + h2o at bottom of triangle (always)
formation
arrows UP
elements at bottom of triangle
Explain why the value given for the O=O bond enthalpy in part (b) is not a
mean value.
Oxygen is the only substance that has O=O bond
Give one reason why the bond enthalpy that you calculated in part (c) is
different from the mean bond enthalpy quoted in a data book
Data book value derived from (a number of) different compounds