Q.1

Pick out the wrong statement.

  • Cp of monoatomic gases such as metallic vapor is about 5 kcal/kg.atom.
  • The heat capacity of solid inorganic substance is exactly equal to the heat capacity of the substance in the molten state.
  • There is an increase in entropy, when a spontaneous change occurs in an isolated system.
  • At absolute zero temperature, the heat capacity for many pure crystalline substances is zero.
Q.2

The principle applied in liquefaction of gases is

  • adiabatic expansion.
  • Joule-Thomson effect.
  • both (a) and (b).
  • neither (a) nor (b).
Q.3

Melting of ice exemplifies a/an

  • adiabatic process.
  • endothermic reaction.
  • exothermic reaction.
  • process involving a chemical reaction.
Q.4

Which of the following is not a reversible process ?

  • Expansion of an ideal gas against constant pressure.
  • Atmospheric pressure vaporisation of water at 100°C.
  • Solution of NaCl in water at 50°C.
  • None of these.
Q.5

In polytropic process (PVn = constant), if n =it means a/an __________ process.

  • adiabatic
  • reversible
  • isothermal
  • none of these
Q.6

High __________ is an undesirable property for a good refrigerant.

  • specific heat
  • latent heat of vaporisation
  • viscosity
  • specific vapor volume
Q.7

Pick out the wrong statement.

  • Phase rule variables are intensive properties.
  • Heat and work are both state function.
  • The work done by expansion of a gas in vacuum is zero.
  • CP and CV are state function.
Q.8

Fugacity is most helpful in

  • representing actual behaviour of real gases.
  • representing actual behaviour of ideal gases.
  • the study of chemical equilibria involving gases at atmospheric pressure.
  • none of these
Q.9

Any substance above its critical temperature exists as

  • saturated vapour
  • solid
  • gas
  • liquid
Q.10

Pick out the wrong statement.

  • Trouton's ratio of non-polar liquids is calculated using Kistyakowasky equation.
  • Thermal efficiency of a Carnot engine is always less than 1.
  • An equation relating pressure, volume and temperature of a gas is called ideal gas equation.
  • none of these.
Q.11

Work done in an adiabatic process between two states depends on the

  • rate of heat transmission
  • initial state only
  • end states only
  • none of these
Q.12

Which is not a refrigerant ?

  • SO2
  • NH3
  • CCl2F2
  • C2H4Cl2
Q.13

In a turbine, the fluid expands almost

  • isothermally
  • isobarically
  • adiabatically
  • none of these
Q.14

Grams of butane (C4H10) formed by the liquefaction oflitres of the gas (measured at (STP) would be

  • 580
  • 640
  • 1160
  • data insufficient; can't be computed
Q.15

The thermodynamic law, PVy = constant, is not applicable in case of

  • ideal compression of air.
  • free expansion of an ideal gas.
  • adiabatic expansion of steam in a turbine.
  • adiabatic compression of a perfect gas.
Q.16

Partial molar free energy of an element A in solution is same as its

  • chemical potential
  • activity
  • fugacity
  • activity co-efficient
Q.17

A refrigeration cycle is the same as a __________ cycle,

  • turbine
  • heat engine
  • reversed heat engine
  • none of these
Q.18

At __________ point, all the three phases (i.e.solid, liquid and gas) co-exist.

  • eutcetic
  • triple
  • plait
  • critical
Q.19

Pick out the wrong statement.

  • A closed system does not permit exchange of mass with its surroundings but may permit exchange of energy.
  • An open system permits exchange of both mass and energy with its surroundings.
  • The term microstate is used to characterise an individual, whereas macro-state is used to designate a group of micro-states with common characteristics.
  • none of the above.
Q.20

Partial molar free energy of an element A in solution is same as its

  • chemical potential
  • activity
  • fugacity
  • activity co-efficient
Q.21

Compressibility factor of a gas is

  • not a function of its pressure.
  • not a function of its nature.
  • not a function of its temperature.
  • unity, if it follows PV = nRT.
Q.22

A solid metallic block weighing 5 kg has an initial temperature of 500°C.kg of water initially at 25°C is contained in a perfectly insulated tank. The metallic block is brought into contact with water. Both of them come to equilibrium. Specific heat of block material is 0.4 kJ.kg-1. K-1. Ignoring the effect of expansion and contraction and also the heat capacity to tank, the total entropy change in kJ.kg-1 , K-1 is

  • -1.87
  • 0
  • 1.26
  • 3.91
Q.23

dW and dq are not the exact differential, because q and W are

  • state functions
  • path functions
  • intensive properties
  • extensive properties
Q.24

1st law of thermodynamics is nothing but the law of conservation of

  • momentum
  • mass
  • energy
  • none of these
Q.25

The energy of activation of exothermic reaction is

  • zero.
  • negative.
  • very large compared to that for en-dothermic reaction.
  • not possible to predict.
Q.26

Which of the following is an undesirable characteristics of a refrigerant ?

  • It should be non-explosive.
  • It should have a sub-atmospheric vapor pressure at the temperature in refrigerator coils.
  • Its vapor pressure at the condenser temperature should be very high.
  • None of these.
Q.27

Which of the following decreases with increase in pressure ?

  • Melting point of ice
  • Melting point of wax
  • Boiling point of liquids
  • none of these
Q.28

The number of degree of freedom for an azeotropic mixture of ethanol and water in vapour-liquid equilibrium, is

  • 3
  • 1
  • 2
  • 0
Q.29

Trouton's ratio of __________ liquids is calculated using Kistyakowsky equation.

  • polar
  • non-polar
  • both (a) & (b)
  • neither (a) nor (b)
Q.30

The partial pressure of each constituent present in an alloy is __________ the total vapor pressure exerted by the alloy.

  • less than
  • equal to
  • more than
  • either (b) or (c); depends on the type of alloy
Q.31

The unity of Planck's constant 'h' in the equation, E = hv is

  • J/s
  • J.S
  • J/kmol
  • kmol/J
Q.32

Free energy change at equilibrium is

  • zero
  • positive
  • negative
  • indeterminate
Q.33

Kopp's rule is used to calculate the heat capacity of

  • solids
  • liquids
  • gases
  • all (a), (b) & (c)
Q.34

__________ explains the equilibrium constant for any chemical reaction.

  • Henry's law
  • Law of mass action
  • Hess's law
  • none of these
Q.35

Which of the following exemplifies an adiabatic process ?

  • Melting of ice.
  • Condensation of alcohol vapor.
  • Sudden bursting of a cycle tube.
  • Evaporation of water.
Q.36

Entropy, which is a measure of the disorder of a system is

  • independent of pressure.
  • independent of temperature.
  • zero at absolute zero temperature for a perfect crystalline substance.
  • all (a), (b) & (c)
Q.37

Which of the following is not an extensive property ?

  • Free energy
  • Entropy
  • Refractive index
  • None of these
Q.38

"The rate at which a substance reacts is proportional to its active mass and the rate of a chemical reaction is proportional to the product of active masses of the reacting substances". This is the

  • Lewis-Randall rule.
  • statement of Vant-Hoff equation.
  • Le-Chatelier's principle.
  • none of these.
Q.39

In polytropic process (PVn = constant), if n =it means a/an __________ process.

  • adiabatic
  • reversible
  • isothermal
  • none of these
Q.40

Isentropic process means a constant __________ process.

  • enthalpy
  • pressure
  • entropy .
  • none of these
Q.41

When a gas is subjected to adiabatic expansion, it gets cooled due to

  • decrease in velocity.
  • decrease in temperature.
  • decrease in kinetic energy.
  • energy spent in doing work.
Q.42

Joule-Thomson effect i.e., a throttling process is a constant __________ process.

  • entropy
  • temperature
  • internal energy
  • enthalpy
Q.43

The internal energy of an ideal gas is a function of its __________ only.

  • molecular size
  • volume
  • pressure
  • temperature
Q.44

Activity co-efficient is a measure of the

  • departure from ideal solution behaviour.
  • departure of gas phase from idea] gas law.
  • vapour pressure of liquid.
  • none of these.
Q.45

Heat is added at constant pressure in an ideal __________ cycle.

  • Stirling
  • Brayton
  • Rankine
  • both (b) and (c)
Q.46

Specific/molar Gibbs free energy for a pure substance does not change during

  • sublimation
  • vaporisation
  • melting
  • either (a), (b) or (c)
Q.47

Heat pump

  • accomplishes only space heating in winter.
  • accomplishes only space cooling in summer.
  • accomplishes both (a) and (b).
  • works on Carnot cycle.
Q.48

The temperature at which both liquid and gas phases are identical, is called the __________ point.

  • critical
  • triple
  • freezing
  • boiling
Q.49

Critical temperature is defined as the temperature above which a gas will

  • not liquify (barring exceptions).
  • immediately liquify.
  • never liquify however high the pressure may be.
  • none of these.
Q.50

Enthalpy of a gas depends upon its

  • temperature
  • mass
  • volume
  • pressure
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