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Chemical Engineering
Chemical Engineering Thermodynamics
Quiz 9
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Q.1
In polytropic process (PV
n
= constant), if n = 1; it means a/an __________ process.
Adiabatic
Reversible
Isothermal
None of these
Q.2
Mollier diagram is a plot of
Temperature vs. enthalpy
Temperature vs. enthalpy
Entropy vs. enthalpy
Temperature vs. internal energy
Q.3
PV
y
= constant, holds good for an isentropic process, which is
Reversible and isothermal
Isothermal and irreversible
Reversible and adiabatic
Adiabatic and irreversible
Q.4
The internal energy of an ideal gas is a function of its __________ only.
Molecular size
Volume
Pressure
Temperature
Q.5
Gibbs free energy at constant pressure and temperature under equilibrium conditions is
∞
0
Maximum
Minimum
Q.6
An isentropic process is carried out at constant
Volume
Pressure
Temperature
All of the above
Q.7
What is the degree of freedom for two mis-cible (non-reacting) substances in vapor-liquid equilibrium forming an azeotrope?
0
1
2
3
Q.8
At __________ point, all the three phases (i.e.solid, liquid and gas) co-exist.
Eutcetic
Triple
Plait
Critical
Q.9
Melting of ice is an example of an __________ process.
Adiabatic
Isothermal
Isometric
None of these
Q.10
Claude's liquefaction process employs the cooling of gases by
Expansion in an engine
Following a constant pressure cycle
Throttling
None of these
Q.11
A domestic refrigerator has a/an __________ cooled condenser.
Water
Air
Evaporative
Gas
Q.12
Mollier chart is a __________ plot.
Pressure vs enthalpy
Pressure vs volume
Enthalpy vs entropy
Temperature vs entropy
Q.13
Free energy change at equilibrium is
Zero
Positive
Negative
Indeterminate
Q.14
Which of the following is a widely used refrigerant in vapour compression refrigeration system (using large centrifugal compressor)?
Freon
Liquid sulphur dioxide
Methyl chloride
Ammonia
Q.15
Keeping the pressure constant, to double the volume of a given mass of an ideal gas at 27°C, the temperature should be raised to __________ °C.
270
327
300
540
Q.16
Filling of gas from a high pressure cylinder into small bottles is an example of a/an __________ process.
Equilibrium
Adiabatic
Steady
Unsteady
Q.17
With increase in temperature, the internal energy of a substance
Increases
Decreases
Remains unchanged
May increase or decrease; depends on the substance
Q.18
y = specific heat ratio of an ideal gas is equal to
C
p
/C
v
C
p
/(C
P
-R)
1 + (R/C
V
)
All of the above
Q.19
Critical compressibility factor for all substances
Are more or less constant (vary from 0.2 to 0.3)
Vary as square of the absolute temperature
Vary as square of the absolute pressure
None of these
Q.20
One ton of refrigeration is defined as the heat rate corresponding to melting of one ton of ice in one
Hour
Day
Minute
Second
Q.21
The unit of fugacity is the same as that of the
Pressure
Temperature
Volume
Molar concentration
Q.22
Claussius-Clayperon equation gives accurate result, when the
Vapour pressure is relatively low and the temperature does not vary over wide limits
Vapour obeys the ideal gas law and the latent heat of vaporisation is constant
Volume in the liquid state is negligible compared with that in the vapour state
All of the above
Q.23
Pressure-enthalpy chart is useful in refrigeration. The change in internal energy of an ideal fluid used in ideal refrigeration cycle is
Positive
Negative
Zero
Infinity
Q.24
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.25
For an isothermal reversible compression of an ideal gas
Only ΔE = 0
Only ΔH =0
ΔE = ΔH = 0
DQ = dE
Q.26
Boyle's law for gases states that
P ∝ 1/V, when temperature is constant
P ∝ 1/V, when temperature & mass of the gas remain constant
P ∝ V, at constant temperature & mass of the gas
P/V = constant, for any gas
Q.27
Which of the following is not an intensive property?
Volume
Density
Temperature
Pressure
Q.28
The standard Gibbs free energy change of a reaction depends on the equilibrium
Pressure
Temperature
Composition
All of the above
Q.29
In the ammonia synthesis reaction, N₂ + 3H₂ ⇋ 2NH₃ + 22.4 kcal, the formation of NH₃ will be favoured by
High temperature
Low pressure
Low temperature only
Both low temperature and high pressure
Q.30
Joule-Thomson experiment is
Isobaric
Adiabatic
Isenthalpic
Both B & C
Q.31
If the internal energy of an ideal gas decreases by the same amount as the work done by the system, then the
Process must be isobaric
Temperature must decrease
Process must be adiabatic
Both B and C
Q.32
Vapour which is at a pressure smaller than the saturation pressure for the temperature involved is called a __________ vapour.
Superheated
Desuperheated
Non-condensable
None of these
Q.33
The enthalpy change when ammonia gas is dissolved in water is called the heat of
Solution
Formation
Dilution
Combustion
Q.34
During adiabatic expansion of gas
Pressure remains constant
Pressure is increased
Temperature remains constant
None of these
Q.35
1/V (∂V/∂T)
p
is the mathematical expression
Joule-Thomson co-efficient
Specific heat at constant pressure (C
p
)
Co-efficient of thermal expansion
Specific heat at constant volume (C
V
)
Q.36
C
p
- C
v
= R is valid for __________ gases.
Ideal
All
Very high pressure
Very low temperature
Q.37
In case of steady flow compression polytropic process (PV
n
= constant), the work done on air is the lowest, when
N = y = 1.4
N = 0
N = 1
N = 1.66
Q.38
In case of a reversible process (following pv
n
= constant), work obtained for trebling the volume (v₁ = 1 m³ and v₂ 3 m³ ) is max imum, when the value of 'n' is
0
1
1.44
1.66
Q.39
In an adiabatic process, the
Heat transfer is zero
Temperature change is zero
Work done is a path function
Enthalpy remains constant
Q.40
Which of the following identities can be most easily used to verify steam table data for superheated steam.
(∂T/∂V)
S
= (∂p/∂S)
V
(∂T/∂P)
S
= (∂V/∂S)
P
(∂P/∂T)
V
= (∂S/∂V)
T
(∂V/∂T)
P
= -(∂S/∂P)
T
Q.41
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
C
P
and C
V
are state function
Q.42
A liquid under pressure greater than its vapour pressure for the temperature involved is called a __________ liquid.
Subcooled
Saturated
Non-solidifiable
None of these
Q.43
The point at which all the three (solid, liquid and gas) phases co-exist, is known as the __________ point.
Freezing
Triple
Boiling
Boyle
Q.44
The expression, nRT In P₁/P₂ , is for the____of an ideal gas.
Compressibility
Work done under adiabatic contition
Work done under isothermal condition
Co-efficient of thermal expansion
Q.45
Which of the following is not an intensive property?
Chemical potential
Surface tension
Heat capacity
None of these
Q.46
Compound having large heat of formation is
More stable
Less stable
Not at all stable (like nascent O₂)
Either more or less stable ; depends on the compound
Q.47
The equation DU = Tds - PdV is applicable to infinitesimal changes occuring in
An open system of constant composition
A closed system of constant composition
An open system with changes in composition
A closed system with changes in composition
Q.48
The change in Gibbs freee energy for vaporisation of a pure substance is
Positive
Negative
Zero
May be positive or negative
Q.49
The chemical potential for a pure substance is __________ its partial molal free energy.
More than
Less than
Equal to
Not related to
Q.50
Which of the following is not an extensive property?
Free energy
Entropy
Refractive index
None of these
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