_{1}/(T_{1}-T_{2})

_{2}/(T_{1}-T_{2})

_{1}/T_{2}

_{2}/R_{1}

A. T_{1}/(T_{1}-T_{2})

Isothermal

Adiabatic

Isobaric

Isometric

In which there is a temperature drop

Which is exemplified by a non-steady flow expansion

Which can be performed in a pipe with a constriction

In which there is an increase in temperature

^{Δx}, when Δx is negative

^{Δx}, when Δx is positive

Dimensionless, when Δx = 0

^{Δx2}, when Δx > 0

Maxwell's equation

Clausius-Clapeyron Equation

Van Laar equation

Nernst Heat Theorem

∞

+ve

0

-ve

∞

1

0

-ve

The energy change of a system undergoing any reversible process is zero

It is not possible to transfer heat from a lower temperature to a higher temperature

The total energy of system and surrounding remains the same

None of the above

Heat capacity

Molal heat capacity

Pressure

Concentration

Non-flow reversible

Adiabatic

Both (A) and (B)

Neither (A) nor (B)

Steam engine

Carnot engine

Diesel engine

Otto engine

Not a function of its pressure

Not a function of its nature

Not a function of its temperature

Unity, if it follows PV = nRT

Less pronounced

More pronounced

Equal

Data insufficient, can't be predicted

1

< 1

> 1

>> 1

Vapor pressure

Specific Gibbs free energy

Specific entropy

All (A), (B) and (C)

Accomplishes only space heating in winter

Accomplishes only space cooling in summer

Accomplishes both (A) and (B)

Works on Carnot cycle

100,000 kW

160,000 kW

200,000 kW

320,000 kW

Critical temperature

Melting point

Freezing point

Both (B) and (C)

Enhanced COP

Decreased COP

No change in the value of COP

Increased or decreased COP; depending upon the type of refrigerant

Reversible and isothermal

Isothermal and irreversible

Reversible and adiabatic

Adiabatic and irreversible

Enthalpies of all elements in their standard states are assumed to be zero

Combustion reactions are never endothermic in nature

Heat of reaction at constant volume is equal to the change in internal energy

Clausius-Clapeyron equation is not applicable to melting process

Gibbs-Duhem

Maxwell's

Clapeyron

None of these

Entropy

Internal energy

Enthalpy

Gibbs free energy

Non-uniformly

Adiabatically

Isobarically

Isothermally

RT d ln P

R d ln P

R d ln f

None of these

The chemical potential of a pure substance depends upon the temperature and pressure

The chemical potential of a component in a system is directly proportional to the escaping tendency of that component

_{i}) in an ideal gas mixture approaches zero as the pressure or mole fraction (x_{i}) tends to be zero at constant temperature

_{i}) is mathematically represented as,μ_{i} = ∂(nG)/∂ni]_{T,P,nj} where, n, n_{i} and n_{j} respectively denote the total number of moles, moles of i^{th} species and all mole numbers except ith species. 'G' is Gibbs molar free energy

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

No

Any real

Only ideal

Both (B) and (C)

2.73

28.3

273

283

Vapor pressure

Partial pressure

Chemical potential

None of these

_{2}^{2}

_{1}

_{2}

_{1}^{2}