19 Introduction and Quick Prep In the illustration, N is color-coded as blue and O is color-coded as red.
Gas
8388.8
Fusion (Melting
Solid
Liquid
Freezing
What kind of change is represented by thi illustation? F usion
Is energy absorbed or released when this change occurs?bso be
DH nin ESH (products)-EDH(reactants) Using standard hcats of formation, calculatc thc standard cnthalpy change for the following reaction. *[(0)+1(-29u.8]-[(-20.0)+2(-285.2)] . -296.1 295.4 3Hg+SOg reactants 7producis [295.4k]
to be-2847.8
motes;
"speties pYO&UCTS 4 CO 6 Hq0 reactants CHv 0
AHF -393.5 - 241.8 ?. 0
2CH+7O 4CO+6HO(
.5Jmol
DHnnEH(products)-EH(reactan+s) [4CO+6H0]-[iCqH1O]-2847.8 CqH=(-2847.8-[4(-393.5)+0(-241.1)+1(o)]]x, CqH-88.5
Write the equilibrium constant expression, K, for the following reaction i cither the numerate ominator is 1.please enter I
aA+bB cC t dD
PCIg+CIgPCIg
K-[c]"[0]] a{3][v]
[Pcis]
[pc][ci]
19.1a The First and Second Laws of Thermodynamics first law of tmermodunamics: me total eneray ot me oniverse is constant The internal energy of an isolated system is constant(Eolnted=constant The total energy of the universe is constant (Euniverse=constant). The change in the energy of the universe is zeroEmivese =0 For a closed systemE=q+ internal renergy: me sum of me potential and Kinetic energies of me particles in me system
19.1b Entropy and the Second Law of Thermodynamics Second law of +nermodynamics: tme total entropy of the universe is continually incriacing tentropu S: -ameasure of me dispersal of energu in a system
All physical and chemical changes occur such that the total entropy of the univer
Sunve=Systen+Srronding>0 for a spontaneous process19.1
The entropy of an isolated system never
Solbeed 0
19.1c Entropy and Microstates
S=kglnW
(19.2)
K* Bo\tzmann's constant =1.381x 10-13 3/K Ws numbex of microstates
aA gas is held in one bulb of a 2-fask system the flask on the right is empty racuum.bWhen the stopcock is openedthe gas expands tofil the empty sp