(R/ΔH) (1/T1 - 1/T2)
(ΔH/R) (1/T1 - 1/T2)
(ΔH/R) (1/T2 - 1/T1)
(1/R) (1/T1 - 1/T2)
(p + a/V2)(V - b) = nRT
PV = nRT
PV = A + B/V + C/V2 + D/V3 + ...
None of these
its internal energy (U) decreases and its entropy (S) increases
U and S both decreases
U decreases but S is constant
U is constant but S decreases
Expansion valve
Condenser
Refrigerator
Compressor
Decreases
Increases
Remain same
May increase or decrease; depends on the nature of the gas
+ve
-ve
0
∞
Increases
Decreases
Remains unchanged
First decreases and then increases
More stable
Less stable
Not at all stable (like nascent O2)
Either more or less stable; depends on the compound
With pressure changes at constant temperature
Under reversible isothermal volume change
During heating of an ideal gas
During cooling of an ideal gas
Minimum
Zero
Maximum
Indeterminate
Closed
Open
Isolated
Non-thermodynamic
Isothermal
Adiabatic
Isobaric
Isochoric
Expansion in an engine
Following a constant pressure cycle
Throttling
None of these
Rate of change of vapour pressure with temperature
Effect of an inert gas on vapour pressure
Calculation of ΔF for spontaneous phase change
Temperature dependence of heat of phase transition
Endothermic
Exothermic
Isothermal
Adiabatic
Ethyl chloride or methyl chloride
Freon-12
Propane
NH3 or CO2
Matter
Energy
Neither matter nor energy
Both matter and energy
Low temperature and high pressure
Low temperature and low pressure
High temperature and high pressure
High temperature and low pressure
Superheated vapour
Partially condensed vapour with quality of 0.9
Saturated vapour
Partially condensed vapour with quality of 0.1
Zero
Negative
More than zero
Indeterminate
Tds = dE - dW = 0
dE - dW - Tds = 0
Tds - dE + dW < 0
Tds - dT + dW < 0
Adiabatic
Isothermal
Isometric
None of these
The same
Less than
Greater than
Different than
Fugacity
Activity co-efficient
Free energy
None of these
(∂T/∂V)S = - (∂P/∂S)V
(∂S/∂P)T = - (∂V/∂T)P
(∂V/∂S)P = (∂T/∂P)S
(∂S/∂V)T = (∂P/∂T)V
Enthalpy does not remain constant
Entire apparatus is exposed to surroundings
Temperature remains constant
None of these
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'
Eutectic
Triple
Plait
Critical
Pressure
Temperature
Volume
Molar concentration
Minimum number of degree of freedom of a system is zero
Degree of freedom of a system containing a gaseous mixture of helium, carbon dioxide and hydrogen is 4
For a two phase system in equilibrium made up of four non-reacting chemical species, the number of degrees of freedom is 4
Enthalpy and internal energy change is zero during phase change processes like melting, vaporisation and sublimation