Increase
Decrease
Remain unaltered
Increase or decrease; depends on the particular reaction
C. Remain unaltered
More
Less
Same
Unpredictable; depends on the particular reaction
At constant pressure, solubility of a gas in a liquid diminishes with rise in temperature
Normally, the gases which are easily liquefied are more soluble in common solvents
The gases which are capable of forming ions in aqueous solution are much more soluble in water than in other solvents
At constant pressure, solubility of a gas in a liquid increases with rise in temperature
Shift the equilibrium towards right
Give higher yield of NH3
Both (B) and (C)
Neither (A) nor (B)
Reversible and isothermal
Isothermal and irreversible
Reversible and adiabatic
Adiabatic and irreversible
Heating occurs
Cooling occurs
Pressure is constant
Temperature is constant
Cp/Cv
Cp/(CP-R)
1 + (R/CV)
All (A), (B) and (C)
Logarithmic
Arithmetic
Geometric
Harmonic
CV
Enthalpy change
Free energy change
None of these
3
4
5
6
Increased COP
Same COP
Decreased COP
Increased or decreased COP; depending upon the type of refrigerant
(atm)Δx, when Δx is negative
(atm)Δx, when Δx is positive
Dimensionless, when Δx = 0
(atm)Δx2, when Δx > 0
(∂T/∂V)S = (∂p/∂S)V
(∂T/∂P)S = (∂V/∂S)P
(∂P/∂T)V = (∂S/∂V)T
(∂V/∂T)P = -(∂S/∂P)T
Zero
Negative
More than zero
Indeterminate
Less than
More than
Equal to or higher than
Less than or equal to
TVγ-1 = constant
p1-γ.TY = constant
PVγ = constant
None of these
Reversible and isothermal
Irreversible and constant enthalpy
Reversible and constant entropy
Reversible and constant enthalpy
Doubling the absolute temperature as well as pressure of the gas
Reducing pressure to one fourth at constant temperature
Reducing temperature to one fourth at constant pressure
Reducing the temperature to half and doubling the pressure
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
Unity
Activity
Both (A) & (B)
Neither (A) nor (B)
(∂T/∂V)S = - (∂P/∂S)V
(∂S/∂P)T = - (∂V/∂T)P
(∂V/∂S)P = (∂T/∂P)S
(∂S/∂V)T = (∂P/∂T)V
Helmholtz
Gibbs
Both a & b
Neither 'a' nor 'b'
Heat capacity of a crystalline solid is zero at absolute zero temperature
Heat transfer from low temperature to high temperature source is not possible without external work
Gases having same reduced properties behaves similarly
None of these
ΔF = ΔH + T [∂(ΔF)/∂T]P
ΔF = ΔH - TΔT
d(E - TS) T, V < 0
dP/dT = ΔHvap/T.ΔVvap
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
Rectangle
Rhombus
Trapezoid
Circle
Enthalpy remains constant
Entropy remains constant
Temperature remains constant
None of these
Stirling
Brayton
Rankine
None of these
Equal to its density
The reciprocal of its density
Proportional to pressure
None of these
Isothermal
Adiabatic
Isentropic
None of these
Molar volume, density, viscosity and boiling point
Refractive index and surface tension
Both (A) and (B)
None of these