厦门大学：《物理化学 Physical Chemistry》课程电子教案（PPT教学课件，英文版）chapter05 Standard Thermodynamic Functions of Reaction

Physical chemistr Chapter 5 Chapter 5 Standard Thermodynamic Functions of reaction

Chapter 5 Standard Thermodynamic Functions of Reaction Physical Chemistry Chapter 5

1 hysical Chemistry Chapter 5 aStandard Thermodynamic Functions of Reaction Standard states of pure substances Standard state p=l bar Solid or liquid: P=l bar, T Gas: P=l bar. T' gas ideal The standard-state pressure is denoted by P≡1bar.T The standard state of a substance at a specified temperature is its pure form at l bar

Standard States of Pure Substances Standard state P ＝ 1 bar Gas: P = 1 bar, T, gas ideal The standard-state pressure is denoted by P o : P o 1 bar, T Solid or liquid：P ＝ 1 bar, T The standard state of a substance at a specified temperature is its pure form at 1 bar. Standard Thermodynamic Functions of Reaction Physical Chemistry Chapter 5

Physical Chemistry Chapter 5 Standard Enthalpy of reaction For a chemical reaction aA+bB→cC+dD Standard enthalpy(change)of reaction AHT ( Sometime,△, ht is used for△H) AHT=CHm(C)+dHm(D)-aHm(A)-bHm7(B) Molar enthalpy of substance(C)in standard state at T Hm(C T For the general reaction(Eq (4.94) 0→>v;A en AHP=∑H (5.3)

Standard Enthalpy of Reaction For a chemical reaction Then →  i 0  i Ai aA + bB → cC + dD Molar enthalpy of substance (C) in standard state at T ( ) ( ) ( ) ( ) H cH , C dH , D aH , A bH , B o m T o m T o m T o m T o  T  + − − Standard enthalpy (change) of reaction o HT (Sometime, is used for ) o HT o r HT For the general reaction (Eq. (4.94))  (5.3)*   i i Hm,T,i o o HT  ( ) H , C o m T Physical Chemistry Chapter 5

Physical Chemistry Chapter 5 Standard Enthalpy of reaction 一→ For example 2CH6)+1502⑧)→12C02(g)+6HO() AHT =12Hm7(C02,8)+HMT(H2O, 7)-2HMT(CH6, 1)-15Hm7(O2, g) AHo depends on how the reaction is written C6H6()+7.502(g)→6C02(g)+3H2O( △H=6Hmn7(CO2,g)+3Hm(H2O,1)-Hm7(C6H6,1)-7.5Hm(O2,g) Then △H0=2△H

Standard Enthalpy of Reaction For example Then Hodepends on how the reaction is written 12 ( , ) 6 ( , ) 2 ( , ) 15 ( , ) H H , CO2 g H , H2 O l H , C6 H6 l H , O2 g o m T o m T o m T o m T o  T = + − − 2 ' o T o HT = H 2 C6H6 (l) + 15 O2 (g) → 12 CO2 (g) + 6 H2O (l) C6H6 (l) + 7.5 O2 (g) → 6 CO2 (g) + 3 H2O (l) ' 6 ( , ) 3 ( , ) ( , ) 7.5 ( , ) H H , CO2 g H , H2 O l H , C6 H6 l H , O2 g o m T o m T o m T o m T o  T = + − − Physical Chemistry Chapter 5

Physical Chemistry Chapter 5 Standard Enthalpy of formation The reference form(reference phase) of an element at T' is usually taken as the form of the element that is most stable at T and l-bar pressure For example, A H307. H, co(&) for H2 Co(g) at 307K C(graphite, 307 K, po )+H2(ideal gas, 307 K, Po)+1202 (ideal gas, 307K, Po)>H,CO(ideal gas, 307K, Po) For an element in its reference form,A ho is zero For example, A H307graphite =0 C(graphite, 307K, Po)>c(graphite, 307K, Po) Nothing happens in this process however, boz. diamond to(a h3ozdiamond=1.9k/mol) C( graphite, 307K, Po )>C(diamond, 307 K, Po

Standard Enthalpy of Formation The reference form (reference phase) of an element at T is usually taken as the form of the element that is most stable at T and 1-bar pressure. For example, for H2CO(g) at 307 K C (graphite, 307 K, Po )＋H2 (ideal gas, 307 K, Po )＋½O2 (ideal gas, 307 K, Po ) → H2CO (ideal gas, 307 K, Po ) o f H307,H CO(g) 2  For an element in its reference form, is zero. For example, ＝0。 o  f HT o f H307,graphite C (graphite, 307 K, P o ) → C (diamond, 307 K, P o ) C (graphite, 307 K, P o ) → C (graphite, 307 K, P o ) Nothing happens in this “process” however, 0 ( )  307,  o f H diamond H kJ mol o f diamond 1.9 /  307, = Physical Chemistry Chapter 5

Physical Chemistry Chapter 5 The standard enthalpy change AHT for a chemical reaction △H0 ∑ T. (5.6)* Consider the reaction aA+bB→cC+dD Reactants aA+ bB Products cc +dD in their standard states in their standard states at T at T (2) Elements in their standard states at T

Consider the reaction aA＋b B → cC＋dD The standard enthalpy change for a chemical reaction o HT  =  i o i f T i o HT  H , (5.6)* Reactants aA + bB in their standard states at T Products cC + dD in their standard states at T Elements in their standard states at T (1) (2) (3) Fig. 5.1 Physical Chemistry Chapter 5

Physical Chemistry Chapter 5 aA+bB→cC+dD △H=△H1=AH2+A3 AH2=aHr(A)+b△,Hr(B +)AH3=c△,H(O)+△H(D) AHx=-a△H(4)-b,HF7(B)+C△,H(C)+a△,HF(D) Reactants aa +bB Products cC + dD in their standard states in their standard states at T' at T Elements in their standard states at T' Fig. 5.1

a A＋b B →c C＋d D H H1 o  T =  = H2 + H3 ( ) ( ) H2 a H A b H B o f T o − = f T +  ( ) ( ) H3 c H C d H D o f T o  = f T +  H a H (A) b H (B) c H (C) d H (D) o f T o f T o f T o f T o  T = −  −  +  +  +) Reactants aA + bB in their standard states at T Products cC + dD in their standard states at T Elements in their standard states at T (1) (2) (3) Fig. 5.1 Physical Chemistry Chapter 5

Physical Chemistry Chapter 5 Determination of 4 Ho and 4, Ho Read page 144 Use calorimetry When a reaction is carried out in a calorimeter The heat gained/lost The heat lost/gained by the calorimeter and by the reacting system Its contents Changes in heat content are calculated using △H=m·c·△T

Determination of f Ho and r Ho • Read page 144 • Use calorimetry H = mcT When a reaction is carried out in a calorimeter The heat lost/gained by the reacting system The heat gained/lost by the calorimeter and its contents = Changes in heat content are calculated using Physical Chemistry Chapter 5

Physical Chemistry Chapter 5 Enthalpies of combustion are measured in a 一 bomb calorimeter Ignition wires electrical Thermometer heater Stirrer ----- 耕 Adiabatic wall O2(g) Sample pellet Fig. 5.4

Enthalpies of combustion are measured in a bomb calorimeter. H2O O2 (g) Sample pellet Stirrer Electrical heater Thermometer Ignition wires Fig. 5.4 Adiabatic wall Physical Chemistry Chapter 5

Physical Chemistry Chapter 5 T thermochemistry The study of the heat produced or required by chemical reactions Calorimetetry Heat produced /adsorbed by a reaction 9=40 q=4H const (const

Thermochemistry The study of the heat produced or required by chemical reactions Calorimetetry Heat produced /adsorbed by a reaction q = U (const. V) q = H (const. P) Physical Chemistry Chapter 5