Ch 6 - Thermochemistry Flashcards
endothermic
positive ΔH, heat in
exothermic
negative ΔH, heat out
specific heat capacity (c)
of water?
quantity of heat required to change the temperature of 1g of an object by 1K
4.184 J/g*K
qlost +qgain = 0 can be turned into
qrxn + qH2O + qcal = 0
ΔH definition and equation
change in enthalpy
related to coefficients, proportional to amount of substance
ΔHrxn = qrxn/mol of product
ccal
container gains/loses heat
qcal = ccal * ΔT
q=
q=cmassΔT
heat of formation (ΔHf)
1 mol of a compound forms from its elements in their most stable form
usually exothermic (-)
ΔHrxn = (coefficients)
ΔHrxn = ΣcoeffΔHfproducts - ΣcoeffHfreactants
ΔHcomb
how much energy you can get per 1 mole of fuel reactant
ΔHfus
endothermic, melting, solid to liquid
ΔHvap
endothermic, liquid to gas