Chapter 16 Spontaneity, entropy and free energy

Spontaneous l A reaction that will occur without outside intervention. l We cant determine how fast. l We need both thermodynamics and kinetics to describe a reaction completely. l Thermodynamics compares initial and final states. l Kinetics describes pathway between.

Thermodynamics l 1st Law- the energy of the universe is constant. l Keeps track of thermodynamics doesnt correctly predict spontaneity. l Entropy (S) is disorder or randomness l 2nd Law the entropy of the universe increases.

Entropy l Defined in terms of probability. l Substances take the arrangement that is most likely. l The most likely is the most random. l Calculate the number of arrangements for a system.

l 2 possible arrangements l 50 % chance of finding the left empty

l 4 possible arrangements l 25% chance of finding the left empty l 50 % chance of them being evenly dispersed

l 4 possible arrangements l 8% chance of finding the left empty l 50 % chance of them being evenly dispersed

Gases l Gases completely fill their chamber because there are many more ways to do that than to leave half empty. l S solid <S liquid <<S gas l there are many more ways for the molecules to be arranged as a liquid than a solid. l Gases have a huge number of positions possible.

Entropy l Solutions form because there are many more possible arrangements of dissolved pieces than if they stay separate. l 2nd Law S univ = S sys + S surr If S univ is positive the process is spontaneous. If S univ is negative the process is spontaneous in the opposite direction.

For exothermic processes S surr is positive. For endothermic processes S surr is negative. Consider this process H 2 O(l) H 2 O(g) S sys is positive S surr is negative S univ depends on temperature.

Temperature and Spontaneity l Entropy changes in the surroundings are determined by the heat flow. l An exothermic process is favored because by giving up heat the entropy of the surroundings increases. The size of S surr depends on temperature S surr = - H/T

S sys S surr S univ Spontaneous? ? +-? Yes No, Reverse At Low temp. At High temp.

Gibb's Free Energy l G=H-TS l Never used this way. G= H-T S at constant temperature l Divide by -T - G/T = - H/T- S - G/T = S surr + S - G/T = S univ If G is negative at constant T and P, the Process is spontaneous.

Lets Check For the reaction H 2 O(s) H 2 O(l) Sº = 22.1 J/K mol Hº =6030 J/mol Calculate G at 10ºC and -10ºC Look at the equation G= H-T S Spontaneity can be predicted from the sign of H and S.

G= H-T S H S Spontaneous? +- At all Temperatures ++ At high temperatures, entropy driven -- At low temperatures, enthalpy driven +- Not at any temperature, Reverse is spontaneous

Third Law of Thermo l The entropy of a pure crystal at 0 K is 0. l Gives us a starting point. l All others must be>0. l Standard Entropies Sº ( at 298 K and 1 atm) of substances are listed. Products - reactants to find Sº (a state function). l More complex molecules higher Sº.

Free Energy in Reactions Gº = standard free energy change. l Free energy change that will occur if reactants in their standard state turn to products in their standard state. l Cant be measured directly, can be calculated from other measurements. Gº= Hº-T Sº l Use Hesss Law with known reactions.

Free Energy in Reactions There are tables of Gº f. l Products-reactants because it is a state function. l The standard free energy of formation for any element in its standard state is 0. l Remember- Spontaneity tells us nothing about rate.

G= H-T S H S Spontaneous? +- At all Temperatures ++ At high temperatures, entropy driven -- At low temperatures, enthalpy driven +- Not at any temperature, Reverse is spontaneous

Third Law of Thermo l The entropy of a pure crystal at 0 K is 0. l Gives us a starting point. l All others must be>0. l Standard Entropies Sº ( at 298 K and 1 atm) of substances are listed. Products - reactants to find Sº (a state function) l More complex molecules higher Sº.

Free Energy in Reactions Gº = standard free energy change. l Free energy change that will occur if reactants in their standard state turn to products in their standard state. l Cant be measured directly, can be calculated from other measurements. Gº= Hº-T Sº l Use Hesss Law with known reactions.

Free Energy in Reactions There are tables of Gº f l Products-reactants because it is a state function. l The standard free energy of formation for any element in its standard state is 0. l Remember- Spontaneity tells us nothing about rate.

Free energy and Pressure G = Gº +RTln(Q) where Q is the reaction quotients (P of the products /P of the reactants). CO(g) + 2H 2 (g) CH 3 OH(l) l Would the reaction be spontaneous at 25ºC with the H 2 pressure of 5.0 atm and the CO pressure of 3.0 atm? Gº f CH 3 OH(l) = -166 kJ Gº f CO(g) = -137 kJ Gº f H 2 (g) = 0 kJ

How far? G tells us spontaneity at current conditions. When will it stop? l It will go to the lowest possible free energy which may be an equilibrium. At equilibrium G = 0, Q = K Gº = -RTlnK

Gº K =0=1 0 >0<0

Temperature dependence of K Gº= -RTlnK = Hº - T Sº ln(K) = Hº/R(1/T)+ Sº/R l A straight line of lnK vs 1/T

Free energy And Work l Free energy is that energy free to do work. l The maximum amount of work possible at a given temperature and pressure. l Never really achieved because some of the free energy is changed to heat during a change, so it cant be used to do work.