Download GTU BE/B.Tech 2019 Summer 3rd Sem New 2132102 Metallurgical Thermodynamics Question Paper

Download GTU (Gujarat Technological University) BE/BTech (Bachelor of Engineering / Bachelor of Technology) 2019 Summer 3rd Sem New 2132102 Metallurgical Thermodynamics Previous Question Paper

1
Seat No.: ________ Enrolment No.___________

GUJARAT TECHNOLOGICAL UNIVERSITY

BE - SEMESTER ?III (NEW) EXAMINATION ? SUMMER 2019
Subject Code: 2132102 Date: 07/06/2019

Subject Name:Metallurgical Thermodynamics

Time: 02:30 PM TO 05:00 PM Total Marks: 70

Instructions:

1. Attempt all questions.

2. Make suitable assumptions wherever necessary.

3. Figures to the right indicate full marks.

Q.1 (a) What is Thermodynamics? Give importance of it. 03
(b) Explain different kinds of systems in thermodynamics. 04
(c) What is thermodynamic equilibrium? Compare extensive and
intensive properties.
07

Q.2 (a) Explain energy is a state property. 03
(b) State & Define 1st law of Thermodynamics & its significance. 04
(c) Justify: Cp >Cv. 07
OR
(c) Compare and contrast Hess? law and Kirchhoff?s law. 07
Q.3 (a) What is heat capacity? And derive 1
st
law thermodynamics in terms
of Enthalpy.
03
(b) Calculate standard enthalpy change for the given reaction at 473 K.
CO(g) + 1/2 O2(g) = CO2(g). Given that standard enthalpy change of
formation at 298 K EW -111kJ/mol for CO(g) and -394 kJ/mol for
CO2(g). Molar heat capacity of Cp is as follows. For CO(g) =30.0 +
0.0041 T J/K.mol, O2(g) =28.5 + 0.0042 T J/K.mol, CO2(g)= 44.2 +
0.0088 T J/K.mol.
04
(c) Derive combined expression of 1st and 2nd law of thermodynamics
in terms of internal energy, enthalpy, Helmholtz free energy and
Gibb?s free energy.
07
OR
Q.3 (a) Iron melts at 1536 ?C at 1 atmospheric pressure and its heat of fusion
is 14 kJ/mol. This is reversible process at constant temperature and
pressure. Calculate the change of entropy at melting point of Iron
03
(b) Calculate standard free energy change of reaction: Ni(S) + 1/2 O2(g)
= NiO(S). At 600 K from following data:?H298,NiO(S)=-240.6 KJ/mol,
S?298,Ni(S)= 29.8 J/K/mol, S?298, NiO(S) = 38.1 J/K/mol, S?298,O2(g) = 206
J/K/mol. Cp, Ni(S)=25.23 + 43.7 *10
-6
T
2
? 10
-3
T J/K/mol. Cp, O2(g)=
30 + 4.2 * 10
-3
T -1.67 * 10
-5
T
2
J/K/mol,
Cp, NiO(S) = 54 J/K/mol.
04
(c) Discuss important features of Ellingham diagram. 07

Q.4 (a) Give Maxwell?s relations. 03
(b) State 0
th
and 2
nd
law of thermodynamics. 04
(c) Explain Sivert?s and Raoult?s law. 07

OR
Q.4 (a) Write formula for Mol fraction and give definition of Molality,
Molarity and Normality
03
(b) Explain fugacity, activity and mole fraction. 04
(c) What is Free Energy? Explain concept of Gibb?s Free Energy. 07
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1
Seat No.: ________ Enrolment No.___________

GUJARAT TECHNOLOGICAL UNIVERSITY

BE - SEMESTER ?III (NEW) EXAMINATION ? SUMMER 2019
Subject Code: 2132102 Date: 07/06/2019

Subject Name:Metallurgical Thermodynamics

Time: 02:30 PM TO 05:00 PM Total Marks: 70

Instructions:

1. Attempt all questions.

2. Make suitable assumptions wherever necessary.

3. Figures to the right indicate full marks.

Q.1 (a) What is Thermodynamics? Give importance of it. 03
(b) Explain different kinds of systems in thermodynamics. 04
(c) What is thermodynamic equilibrium? Compare extensive and
intensive properties.
07

Q.2 (a) Explain energy is a state property. 03
(b) State & Define 1st law of Thermodynamics & its significance. 04
(c) Justify: Cp >Cv. 07
OR
(c) Compare and contrast Hess? law and Kirchhoff?s law. 07
Q.3 (a) What is heat capacity? And derive 1
st
law thermodynamics in terms
of Enthalpy.
03
(b) Calculate standard enthalpy change for the given reaction at 473 K.
CO(g) + 1/2 O2(g) = CO2(g). Given that standard enthalpy change of
formation at 298 K EW -111kJ/mol for CO(g) and -394 kJ/mol for
CO2(g). Molar heat capacity of Cp is as follows. For CO(g) =30.0 +
0.0041 T J/K.mol, O2(g) =28.5 + 0.0042 T J/K.mol, CO2(g)= 44.2 +
0.0088 T J/K.mol.
04
(c) Derive combined expression of 1st and 2nd law of thermodynamics
in terms of internal energy, enthalpy, Helmholtz free energy and
Gibb?s free energy.
07
OR
Q.3 (a) Iron melts at 1536 ?C at 1 atmospheric pressure and its heat of fusion
is 14 kJ/mol. This is reversible process at constant temperature and
pressure. Calculate the change of entropy at melting point of Iron
03
(b) Calculate standard free energy change of reaction: Ni(S) + 1/2 O2(g)
= NiO(S). At 600 K from following data:?H298,NiO(S)=-240.6 KJ/mol,
S?298,Ni(S)= 29.8 J/K/mol, S?298, NiO(S) = 38.1 J/K/mol, S?298,O2(g) = 206
J/K/mol. Cp, Ni(S)=25.23 + 43.7 *10
-6
T
2
? 10
-3
T J/K/mol. Cp, O2(g)=
30 + 4.2 * 10
-3
T -1.67 * 10
-5
T
2
J/K/mol,
Cp, NiO(S) = 54 J/K/mol.
04
(c) Discuss important features of Ellingham diagram. 07

Q.4 (a) Give Maxwell?s relations. 03
(b) State 0
th
and 2
nd
law of thermodynamics. 04
(c) Explain Sivert?s and Raoult?s law. 07

OR
Q.4 (a) Write formula for Mol fraction and give definition of Molality,
Molarity and Normality
03
(b) Explain fugacity, activity and mole fraction. 04
(c) What is Free Energy? Explain concept of Gibb?s Free Energy. 07
2
Q.5 (a) Define Atom fraction. Write conversion from weight % to atom %
or vice-versa.
03
(b) Write a short note on Clausius-Clapeyron equation. 04
(c) Derive and explain Gibb?s phase rule. 07
OR

Q.5 (a) Explain the function of slag 03
(b) Explain basicity index with suitable example. 04
(c) State and explain fugacity and activity. 07

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