Enumerate the main applications of Materials thermodynamics.
[3 marks]Explain homogeneous and heterogeneous system.
[4 marks]Explain reversible and irreversible changes.
[7 marks]Explain specific heat.
[3 marks]Explain different equilibrium systems.
[4 marks]Explain 1st law thermodynamics with its significances.
[7 marks]Explain specific heat and prove that Cp > Cv.
Explain latent heat.
[3 marks]Justify-Entropy is a state property.
[4 marks]Explain 2nd law of thermodynamics with respect to irreversible change.
[7 marks]Explain work.
[3 marks]Explain Roult’s law of solutions.
[4 marks]Explain Hess’s law of thermodynamics.
[7 marks]State zeroth law of thermodynamics.
[3 marks]Explain Sievert’s law of solutions.
[4 marks]Explain Kirchhoff’s law of thermodynamics.
[7 marks]Explain F=0, F=1 and F=2 conditions with respect to Gibb’s phase rule.
[3 marks]Abrass contain 70 wt. % of Copper and rest of Zinc. Calculate atom %. Atomic weights of Cu and Zn are 63.54 and 65.38.
[4 marks]Derive Gibb’s phase rule.
[7 marks]Expalin 3rd law of themodynamics.
[3 marks]For the reaction: CO + 1/2O = CO Calculate the standard enthalpy
[4 marks]2 (g) 2 (g). change for the above reaction at 500 K, given that the standard enthalpy change of formation at 298 Kare -110.5 kJ/mol for CO and -393.5 kJ/mol for CO
[ marks]2 Molar heat capacities (Cp) are as follows: For CO = 30.0 + 0.0041 T
[ marks]. (g) J/K.mol, O = 28.5 + 0.0042 T J/K.mol, CO = 44.2 + 0.0088 T J/K.mol. 2 (g) 2 (g)
[ marks]Discuss important features of Ellingham diagram.1
[7 marks]Justify-Energy is the state property.
[3 marks]Calculate change of free energy for the following reduction reaction at 500 K. CuO (s) + H (g) = Cu (s) + H (g). Given ∆H° =88 kJ/mol and ∆S° =88 kJ/mol.
[4 marks]Derive Gibb’s Duhem equation.
[7 marks]