Surface tension of a substance vanishes at critical point, as there is no distinction between liquid and vapour phases at its critical point
Entropy of a system decreases with the evolution of heat
Change of internal energy is negative for exothermic reactions
The eccentric factor for all materials is always more than one
D. The eccentric factor for all materials is always more than one
30554
10373
4988.4
4364.9
dP/dT = ΔH/TΔV
ln P = - (ΔH/RT) + constant
ΔF = ΔH + T [∂(ΔF)/∂T]P
None of these
Zero
50%
Almost 100%
unpredictable
1
2
3
4
2.73
28.3
273
283
Volume
Temperature
Pressure
None of these
Adiabatic
Isothermal
Isometric
None of these
Like internal energy and enthalpy, the absolute value of standard entropy for elementary substances is zero
Melting of ice involves increase in enthalpy and a decrease in randomness
The internal energy of an ideal gas depends only on its pressure
Maximum work is done under reversible conditions
Sublimation
Fusion
Transition
Vaporisation
Minimum
Zero
Maximum
Indeterminate
Pressure
Volume
Mass
None of these
Both the processes are adiabatic
Both the processes are isothermal
Process A is isothermal while B is adiabatic
Process A is adiabatic while B is isothermal
Adiabatic process
Isothermal process
Isobaric process
All require same work
ds = 0
ds <0
ds > 0
ds = Constant
Adiabatic expansion
Joule-Thomson effect
Both (A) and (B)
Neither (A) nor (B)
More than
Less than
Equal to
Not related to
Specific heat at constant pressure (Cp)
Specific heat at constant volume (Cv)
Joule-Thompson co-efficient
None of these
-19.4
-30.2
55.2
-55.2
CO2
H2
O2
N2
States that n1dμ1 + n2dμ2 + ....njdμj = 0, for a system of definite composition at constant temperature and pressure
Applies only to binary systems
Finds no application in gas-liquid equilibria involved in distillation
None of these
Isobaric
Adiabatic
Isenthalpic
Both (B) & (C)
(atm)Δx, when Δx is negative
(atm)Δx, when Δx is positive
Dimensionless, when Δx = 0
(atm)Δx2, when Δx > 0
Enthalpy
Pressure
Entropy
None of these
Less than
More than
Equal to or higher than
Less than or equal to
Amount of energy transferred
Direction of energy transfer
Irreversible processes only
Non-cyclic processes only
Equation of state
Gibbs Duhem equation
Ideal gas equation
None of these
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
4 J
∞
0
8 J
Accomplishes only space heating in winter
Accomplishes only space cooling in summer
Accomplishes both (A) and (B)
Works on Carnot cycle
P + F - C = 2
C = P - F + 2
F = C - P - 2
P = F - C - 2