P ∝ 1/V, when temperature is constant
P ∝ 1/V, when temperature & mass of the gas remain constant
P ∝ V, at constant temperature & mass of the gas
P/V = constant, for any gas
B. P ∝ 1/V, when temperature & mass of the gas remain constant
dE = Tds - PdV
dQ = CvdT + PdV
dQ = CpdT + Vdp
Tds = dE - PdV
The amount of work needed is path dependent
Work alone cannot bring out such a change of state
The amount of work needed is independent of path
More information is needed to conclude anything about the path dependence or otherwise of the work needed
If an insoluble gas is passed through a volatile liquid placed in a perfectly insulated container, the temperature of the liquid will increase
A process is irreversible as long as Δ S for the system is greater than zero
The mechanical work done by a system is always equal to∫P.dV
The heat of formation of a compound is defined as the heat of reaction leading to the formation of the compound from its reactants
dE = CpdT
dE = CvdT
dQ = dE + pdV
dW = pdV
Cv.dT
Cp.dT
∫ Cp.dT
∫ Cv.dT
Zero
Unity
Infinity
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
Isochoric
Isobaric
Adiabatic
Isothermal
H = E - PV
H = F - TS
H - E = PV
None of these
Steam engine
Carnot engine
Diesel engine
Otto engine
Mole fraction
Fugacity at the same temperature and pressure
Partial pressure
None of these
Heat pump
Heat engine
Carnot engine
None of these
Two
One
Zero
Three
Are more or less constant (vary from 0.2 to 0.3)
Vary as square of the absolute temperature
Vary as square of the absolute pressure
None of these
Adiabatic process
Isothermal process
Isobaric process
All require same work
TVγ-1 = constant
p1-γ.TY = constant
PVγ = constant
None of these
RT ln K
-RT ln K
-R ln K
T ln K
Helmholtz
Gibbs
Both a & b
Neither 'a' nor 'b'
Number of intermediate chemical reactions involved
Pressure and temperature
State of combination and aggregation in the beginning and at the end of the reaction
None of these
Internal energy
Enthalpy
Entropy
All (A), (B) & (C)
d ln p/dt = Hvap/RT2
d ln p/dt = RT2/Hvap
dp/dt = RT2/Hvap
dp/dt = Hvap/RT2
Closed
Open
Isolated
Non-thermodynamic
F = A + PV
F = E + A
F = A - TS
F = A + TS
Zero
Unity
Infinity
Negative
-19.4
-30.2
55.2
-55.2
Less
More
Same
More or less depending upon the extent of work done
Zeroth
First
Second
Third
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
Prediction of the extent of a chemical reaction
Calculating absolute entropies of substances at different temperature
Evaluating entropy changes of chemical reaction
Both (B) and (C)
Entropy
Gibbs free energy
Internal energy
All (A), (B) & (C)