KANPUR INSTITUTE OF TECHNOLOGY & PHARMACY, KANPUR B.Pharm 2 Semester (Session 2010-11)

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KANPUR INSTITUTE OF TECHNOLOGY & PHARMACY, KANPUR

B.Pharm 2
nd

Semester (Session 2010
-
11)

Subject: Physical Chemistry (PHARM
-
121)

QUESTION BANK

-

UNIT


2



Section

A (1 mark for each)

Q. 1 The

apparatus used to measure heat changes during chemical reactions is called_____________.

Q. 2 For an endothermic reaction ΔH is _____________________.

Q. 3 The process of sublimation for a solid occurs t temperature below its_____________________.

Q. 4 Th
e bond energy depends upon ________________, _________________ & ____________________.

Q. 5 In an exothermic reaction the heat energy is ________________ while in endothermic reaction it
is___________________.

Q. 7 The enthalpy of system is defined by rela
tion _________________________.

Q. 8 In an exothermic reaction, the internal energy of the products is _______________ internal energy of
reactants.

Q. 9 Thermodynamics is applicable to __________________ systems only.

Q. 10 A gas contained in a cylinder
filled with a piston is an example of a _______________ system.

Q. 11 In an adiabatic process______________ can flow into or out of the system.

Q. 12 A spontaneous change is accomplained by __________________ of internal energy or enthalpy.

Q. 13 Mixing of

two or more than two gases is a ____________________________.

Q. 14 By convention, the standard heat of formation of all elements is assumed to be
______________.

State whether true or false:

Q. 1 The heat change when one mole of liquid is converted in
to vapour or gaseous state at its boiling point is
called

heat of vaporization.

Q. 2 Thermodynamics is concerned only with the initial and final states of the system.

Q. 3 A thermo flask is an example of isolated system.


Section

B (4
marks for each)


Q. 1 Derive Kirchoff’s reaction.

Q. 2 Define heat of reaction. Derive the relationship between heat of reaction at constant volume and at
constant pressure.

Q. 3 State and explain Heat of formation, Heat of Combustion with examples.

Q. 4 S
tate and explain First law of Thermodynamics.

Q. 5 What is the basic principle of Joule
-
Thompson effect?

Q. 6 Distinguish between

a) Isothermal and Adiabatic process

b) Reversible and Irreversible process

Q. 7 Describe
absolute temperature scale.

Q. 8 What is the main difference between thermochemistry and thermodynamics?

Q. 9 Explain Entropy and give its unit.

Q. 10 State and explain Second law of Thermodynamics.


Section

C (10 marks for each)


Q. 1 State Hess’s law of

a constant heat summation and describe its application.

Q. 2 Define and explain following terms:

a) Heat of formation

b) Standard heat of formation

c) Enthalpy of reaction

d) Heat of combustion

e) Heat of vaporization

f) Hess’s law

g)
Bond energy


Q. 3 Explain the following terms:

a) State of a system

b) Extensive properties

c) Closed system

d) Isothermal process

Q. 4 Define or explain the following terms:

a) Entrop
y

b) Second law of thermodynamics

c) Third law of thermodynamics

d
) Gibbs free energy

e) Gibbs Helmholtz equation

f) Spontaneous reactions

g) van’t Hoff isotherm

h) Carnot cycle