-94 kcal
+94 kcal
> 94 kcal
< -94 kcal
B. +94 kcal
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
1
2
3
4
Enthalpy does not remain constant
Entire apparatus is exposed to surroundings
Temperature remains constant
None of these
Cold reservoir approaches zero
Hot reservoir approaches infinity
Either (A) or (B)
Neither (A) nor (B)
Addition of inert gas favours the forward reaction, when Δx is positive
Pressure has no effect on equilibrium, when Δn = 0
Addition of inert gas has no effect on the equilibrium constant at constant volume for any value of Δx (+ ve, - ve) or zero)
All 'a', 'b' & 'c'
Increase the partial pressure of H2
Increase the partial pressure of I2
Increase the total pressure and hence shift the equilibrium towards the right
Not affect the equilibrium conditions
Specific heat
Latent heat of vaporisation
Viscosity
Specific vapor volume
Increase
Decrease
Not alter
None of these
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
Bomb
Separating
Bucket
Throttling
Two isothermal and two isentropic
Two isobaric and two isothermal
Two isochoric and two isobaric
Two isothermals and two isochoric
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
Surface tension
Free energy
Specific heat
Refractive index
Increases
Decreases
Remains unchanged
Decreases linearly
< 0
> 0
= 0
None of these
Internal energy
Enthalpy
Entropy
All (A), (B) & (C)
2
0
1
3
The net change in entropy in any reversible cycle is always zero
The entropy of the system as a whole in an irreversible process increases
The entropy of the universe tends to a maximum
The entropy of a substance does not remain constant during a reversible adiabatic change
0
+ve
-ve
∞
Sublimation
Vaporisation
Melting
Either (A), (B) or (C)
Zero
One
Infinity
Negative
Zero
Unity
Infinity
An indeterminate value
Not a function of its pressure
Not a function of its nature
Not a function of its temperature
Unity, if it follows PV = nRT
Increase
Decrease
Remain unchanged
First fall and then rise
Freon
Liquid sulphur dioxide
Methyl chloride
Ammonia
Steam engine
Carnot engine
Diesel engine
Otto engine
Chemical potential
Surface tension
Heat capacity
None of these
Zeroth
First
Second
Third
Kp2/Kp1 = - (ΔH/R) (1/T2 - 1/T1)
Kp2/Kp1 = (ΔH/R) (1/T2 - 1/T1)
Kp2/Kp1 = ΔH (1/T2 - 1/T1)
Kp2/Kp1 = - (1/R) (1/T2 - 1/T1)
Extensive property
Intensive property
Force which drives the chemical system to equilibrium
Both (B) and (C)