unit 2.1 Thermochemistry

Cards (16)

exothermic
give out heat as they proceed
endothermic
takes heat from surrounding
exothermic reactions
temperature of surroundings increases
energy decreases
endothermic reactions
temperature of surroundings decreases
energy increases
enthalpy change
heat change at constant pressure, varies with conditions
formation enthalpy
enthalpy change when one mole of a substance is made from its constituent elements under standard conditions
why cant you measure enthalpy change directly
can make a multitude of products not only the one you want
combustion enthalpy
enthalpy change when one mole of a substance is completely combusted in oxygen in standard conditions
whats the equation for internal energy
Q=mc $\Delta$ T
whats a calorimeter
measures energy change
how to improve an enthalpy change prac
insulate the prac
copper calorimeter instead of glass
enthalpy hcange equation
$\frac{Q}{n}$
Hess' law
no matter the route taken for a reaction the overall enthalpy change will remain the same
what is bond enthalpy
change that takes place when breaking one mole of a given bond in the molecule of a gaseous species
average bond enthalpy
average enthalpy change that takes place when breaking by homolytic fission 1 mole of a given type of bond in molecules in gaseous state
to find $\Delta$ T on a graph  
extrapolate graph