Chemical potential
Surface tension
Heat capacity
None of these
C. Heat capacity
A homogeneous solution (say of phenol water) is formed
Mutual solubility of the two liquids shows a decreasing trend
Two liquids are completely separated into two layers
None of these
Ethyl chloride or methyl chloride
Freon-12
Propane
NH3 or CO2
0
1
∞
None of these
A gas may have more than one inversion temperatures
The inversion temperature is different for different gases
The inversion temperature is same for all gases
The inversion temperature is the temperature at which Joule-Thomson co-efficient is infinity
Surface tension
Free energy
Specific heat
Refractive index
Low pressure and high temperature
Low pressure and low temperature
Low temperature and high pressure
High temperature and high pressure
ds = 0
ds < 0
ds > 0
ds = Constant
Accomplishes only space heating in winter
Accomplishes only space cooling in summer
Accomplishes both (A) and (B)
Works on Carnot cycle
Compressibility
Work done under adiabatic condition
Work done under isothermal condition
Co-efficient of thermal expansion
Increases
Decreases
Remains unchanged
Decreases linearly
Ideal
Real
Isotonic
None of these
Isothermal compression
Isothermal expansion
Adiabatic expansion
Adiabatic compression
2HI H2 + I2
N2O4 2NO2
2SO2 + O2 2SO3
None of these
Enhanced COP
Decreased COP
No change in the value of COP
Increased or decreased COP; depending upon the type of refrigerant
Departure from ideal solution behaviour
Departure of gas phase from ideal gas law
Vapour pressure of liquid
None of these
Work required to refrigeration obtained
Refrigeration obtained to the work required
Lower to higher temperature
Higher to lower temperature
T2/(T1 - T2)
T1/(T1 - T2)
(T1 - T2)/T1
(T1 - T2)/T2
Cp of monatomic 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
Only enthalpy change (ΔH) is negative
Only internal energy change (ΔE) is negative
Both ΔH and ΔE are negative
Enthalpy change is zero
In an isothermal system, irreversible work is more than reversible work
Under reversible conditions, the adiabatic work is less than isothermal work
Heat, work, enthalpy and entropy are all 'state functions'
Matter and energy cannot be exchanged with the surroundings in a closed system
H = E - PV
H = F - TS
H - E = PV
None of these
The concentration of each component should be same in the two phases
The temperature of each phase should be same
The pressure should be same in the two phases
The chemical potential of each component should be same in the two phases
(∂T/∂V)S = (∂p/∂S)V
(∂T/∂P)S = (∂V/∂S)P
(∂P/∂T)V = (∂S/∂V)T
(∂V/∂T)P = -(∂S/∂P)T
Increases, for an exothermic reaction
Decreases, for an exothermic reaction
Increases, for an endothermic reaction
None of these
Heat pump
Heat engine
Carnot engine
None of these
Is the most efficient of all refrigeration cycles
Has very low efficiency
Requires relatively large quantities of air to achieve a significant amount of refrigeration
Both (B) and (C)
Oxygen
Nitrogen
Air
Hydrogen
Gibbs-Duhem
Gibbs-Helmholtz
Maxwell's
None of these
Specific heat
Latent heat of vaporisation
Viscosity
Specific vapor volume
Adiabatic
Reversible
Isothermal
None of these