CBSE Class 11 Chemistry Thermodynamics Notes Set 05

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THERMODYNAMICS”

Brief Summary of the chapter:

1. Thermodynamics: Science which deals with study of different forms of energy and quantitative relationship.

2. System & Surroundings: The part of universe for study is called system and remaining portion is surroundings.

3. State of system & state function: State of system is described in terms of T, P, V etc. The property which depends only on state of system not upon path is called state function eg. P, V, T, E, H, S etc.

4. Extensive & Intensive Properties: Properties which depends on quantity of matter called extensive prop. eg. mass, volume, heat capacity, enthalpy, entropy etc. The properties which do not depends on matter present depends upon nature of substance called Intensive properties. eg. T,P, density, refractive index, viscosity, bp, pH, mole fraction etc.

5. Internal energy: The total energy with a system.

i.e. U = Ee + En + Ec + Ep + Ek + ------

ΔU = U2 – U1 or UP – UR & U is state function and extensive properly. If U1 > U2 energy is released.

6. Heat (q): It I a form of energy which is exchanged between system and surrounding due to difference of temperature. Unit is Joule (J) or Calorie (1 Calorie = 4.18 μ J). 

7. First Law of Thermodynamics: It is law of conservation energy. Energy can neither be created not destroyed, it may be converted from one from into another.

Mathematically  ΔU = q + w, w = –p. ΔV (work of expansion)

ΔU = q – p. ΔV or q = ΔU + p.ΔV, q,w are not state function. 

But U is state function.

8. Enthalpy (H): At constant volume V = 0, qv = ΔU

So H = U + p. ΔV, qp = H2 H1 = ΔH

=>H = U + P. ΔV.

9. Relationship between qp, qv i.e. ΔH&ΔU It is H = U+ng.RT or qp = qv + ng.RT

10. Exothermic and Endothermic reactions: H = –Ve for exothermic and H = +Ve for endothermic reaction i.e. evolution and absorption of heat.

Eg C+O2  →CO2 + 393.5 KJ, H = –393.5 KJ (exothermic)

N2 + O2 2NO – 180.7 KJ, H = 180.7 KJ (Endothermic)

11. Enthalpy of reaction (rH): The amount of heat evolved or absorbed when the reaction is completed.

12. Standard Enthalpy of reaction (rH0) at 1 bar pressure and specific temp. (290K) i.e. standard state.

13. Different types of Enthalpies of reactions:

(i) Enthalpy of combustion (ΔcH),                     (ii) Enthalpy of formation (ΔfH)

(iii) Enthalpy of neutralization                         (iv) Enthalpy of solution

(v) Enthalpy of atomization(ΔaH),                    (vi)Enthalpy of Ionisation (ΔiH)

(vii) Enthalpy of Hydration (Δhyol.H)                (viii) Enthalpy of fusion (Δfus.H)

(ix) Enthalpy of vaporization (Δvap.H)             (x)Enthalpy of sublimation (Δsub.H)

          (Δsub.H) = Δ fus.(H) -  Δvap(H)

14. Hess’s Law of constant heat summation: The total amount of heat change is same whether the reaction takes place in one step or in several steps.

i.e. H =Δ H1 + ΔH2 + ΔH3 + -------- 

15. Bond enthalpy: It is amount of energy released when gaseous atoms combines to form one mole of bonds between them or heat absorbed when one mole of bonds between them are broken to give free gaseous atoms.
Further ΔrH = B.E. (Reactants) - B.E. (Products)
 
16. Spontaneous & Non Spontaneous Processes: A process which can take place by itself is called spontaneous process. A process which can neither take place by itself or by initiation is called non Spontaneous.
 
17. Driving forces for spontaneous process: (i) Tendency for minimum energy state. (ii) Tendency for maximum randomness.
 
18. Entropy (S): It is measure of randomness or disorder of system.
i.e. Gas>Liquid>Solid.
Entropy change ( ΔS) = q(rev.)/T  J.K-1 .mol-1
 
19. Spontaneity in term of ( S)
ΔS(total) = ΔS(universe) = ΔS(system) + ΔS(surrounding)
If ΔS(total) is +ve, the process is spontaneous.
If ΔS(total) is –ve, the process is non spontaneous.
 
20. Second Law of thermodynamics: In any spontaneous process, the entropy of the universe always increases. A spontaneous process cannot be reversed.
 
21. Gibb’s free energy (G): defined as G = H – T.S & ΔG = ΔH – T. ΔS (Gibb’s Helmholts equation) it is equal useful work i.e. - G = W(useful) = W(max.)
If ΔG = ve, process is spontaneous.
 
22. Effects of T on spontaneity of a process: ΔG = ΔH – T. ΔS.
(i) For endothermic process may be non spontaneous at law temp.
(ii) For exothermic process may be non spontaneous at high temp. and spontaneous at law temp.
 
23. Calculation of ( ΔrG0)
ΔrG0 =∑Δ fG0 (p) -∑Δ fG0 (r)
 
24. Relationship between ( rG0) & equilibrium constant (k)
ΔG = ΔG0 + RTlnQ & ΔG0 = –2.303RT logk.
 
25. Calculation of entropy change:
ΔrS0 =∑ ΔS0 (p) - ∑S0 (r)
 
ONE MARK QUESTIONS:
 
1. State First Law of thermodynamics.
 
2. What is a thermodynamic state function?
 
3. Give enthalpy (H) of all elements in their standard state.
 
4. From thermodynamic point to which system the animals and plants belong?
 
5. Predict the sign of S for the following reactions.
                             heat 
CaCO3(s) + CO2(g)    →  CaO(s) + CO2(g)
 
6. For the reaction 2Cl(g) Cl2(g), What will be the sign of H and S?
 
7. State Hess’s Law for constant heat summation?
 
8. What is Gibb’s Helmhaltz equation?
 
9. Define extensive properties.
 
10. Give relationship between H, U for a reaction in gaseous state.

 

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Revision Notes and Key Concepts for Class 11 Chemistry Chapter 05 Thermodynamics

Key Concepts and Summary for Class 11 Chemistry Chapter 05 Thermodynamics

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