1. THERMODYNAMICS
3day inservvice course

2. FORMULA THERMODYNAMIC
U=q+w
W=Pex.(-V)= - Pex V= Pex(Vf-Vi)
W=-∫Pin dV
Wrev=-∫ Pex dV =-∫ (PmC dp) dV
Wrev =-∫ Pm dV

3. Wrev =-∫ nRT dV/V=-nRT In Vf/Vi
=-2.303nRT log Vf/Vi
qp=(U2+pV2)-(U1+pV1)
H=U+pV
H= U + pV
PV= ngRT

4. H= U + ngRT
q=c x m x ∆T=CT
H= U + RT
Cp-Cv=R
rH=(sum of enthalpies of product)-( sum of enthalpies of reactant)
=∑ai H products-∑bi H reactants
i i
rHº==∑ai jHºproducts-∑bi jHº reactants

5. rHº==∑ai jHºproducts-∑bi jHº reactants
rH= rH1+ rH2+ rH3
rHv=∑ bond enthalpies reactants-∑ bond enthalpies products
S= qrev/T
Stotal= Ssystem+ Ssuit>0

6. G=H-TS
G= H- TS
 G= H- TS<0
rGº=-2.303RTlogK
rGº= rHº- T rSº=-RTInK

7. Numericals on thermodynamics
In a process,701J of heat is absorbed by a system . what is the change in internal energy for the process?
Sol. Heat absorbed by the system (q)=+701J
Work done by the system (w)=-304J
Change in internal energy (∆U)=q+w= = 307J

8. Sol. ∆U=-742.7KJ/mol;∆n(g)=2-3/2=+0.5
The reaction of cyanamide, NH2CN with oxygen was affected in a bomb calorimeter and ∆U was found to be KJ /mol of cyanamide at 298K. Calculate the enthalpy change for the reaction at 288K.
NH2CN(s)+3/2O2(g) N2(g)+CO2(g)+H2O
Sol. ∆U=-742.7KJ/mol;∆n(g)=2-3/2=+0.5
R=8.314*10-3kJ/K/mol;T=298.5K
∆H= *8.314*10-3 *298.15
= kJ= kJ

9. Calculate the number of kJ necessary to rise the temperature of 60ginium from 35 to 55 C molar heat capacity of Al is 24J/mol/K
Sol. Moles of Al(n)=60/27=2.22mol
Molar heat capacity (Cm)=24J/mol/K
∆T=55-35=20K
q=Cm*n*∆T
=24*2.22*20= J

10. Sol. The freezing process is represented as
Calculate the enthalpy change on freezing of 1.0 mol of water at -10 C to ice at-10C .∆fus=6.03kJ /mol at 0 C. Cp[H2o(l)]=75.3J /mol/k :Cp[H2o(s)]=36.8J /mol/K .
Sol. The freezing process is represented as
H2O(l) H2O(s) T1=-10 C =263.15K;
T2=0 C=273.15K;∆T=T2-T1=10K
Now according to Kirchoff’s equation ,
(∆H2-∆H1)/T2-T1=Cp (ice)-Cp (water)
(-6030-∆H1)/10=
-6030-∆H1=10*38.5
∆H1= 5625J /mol

11. Sol. The combustion eq is
Enthalpy of combustion of carbon to carbon dioxide is kJ /mol . Calculate the heat released upon formation of 35.2g of Co2 from carbon to oxygen gas .
Sol. The combustion eq is
C(s) + O2 (g) Co2(g);∆cH=-393.5kJ/mol
Heat released in the formation of 44g of Co2=393.5kJ
Heat released in the formation of 35.2g of Co2=(393.5*35.2)/44=314.8kJ

12. Sol. ∆fH for the given reaction is given as
The enthapy of formation of Co(g),N2O(g) are -110,393,81 and 9.7kJ /mol respectively. Find the value of ∆fH for the reaction,N2O4(g)+3CO(g) N2O(g)+3CO2(g).
Sol. ∆fH for the given reaction is given as
∆fH= ∑∆fH(products)-∑∆fH(reactants)
=∆fH (CO2)+ ∆fH (N2O) -3 ∆fH (CO)- ∆fH (N2O4)
=3(-393)+81-3(-110)-9.7
= = kJ /mol

13. The eqilibrium constant fpr the vreaction is 10
The eqilibrium constant fpr the vreaction is 10.caculate the value of ∆G;given R=8J/K/mol;T=300K.
Sol. ∆G=-2.303RT log K
Here R =8J/K/Mol; T=300K ;K=10
∆G=-2.303*8*300*log 10
= -5527J/mol
Calculate the entropy change in surroundings when 1 mol of H2o(l) formed under standard conditions. Given ∆fH=-286kJ/mol .
Sol. ∆fH of H2O(l)=-286kJ/mol which refers to heat lost to surrounds
q(surr)=- ∆fH of H2O(l)=-(-286)=+286kJ/mol
∆Ssurr=q(surr)/t=(+286*10³)/298.15= J/K/mol

14. Fir the reaction;2A(g)+B(g) 2D(g) ∆U298=-10.5kJ and ∆S=-44.1J
Calculate ∆G298 for the reaction and predict whether the reaction is spontaneous or not.
Sol. ∆H= ∆U+ ∆n(g)RT
∆ n(g)=2- ∆ 3=-1mol;T=298K; U=10.5kJ
R=8.314kJ/K/mol
∆H=-10.5+[-1*8.314*10-³*298]
=12.298kJ
∆G= ∆H-T∆S
= *0.044
=+0.134kJ/mol
Since ∆G is positive, the reaction is spontaneous ∆

15. For a reaction at 298K; 2A+B C
H=400KJ/mol and ∆S=2kJ/mol.
At what temperaturewill be the reaction become spontaneous considering ∆Hand ∆S to be constant over the temperature range.
Sol. ∆G= ∆H-T∆S
At equilibrium, ∆G=0 ,
Therefore , ∆H=T∆ S
T=400/2=200K
Thus reaction will be in astate of equilibrium at 200K and will become spontaneous as the temperature becomes>200K.