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
D. Not affect the equilibrium conditions
More stable
Less stable
Not at all stable (like nascent O2)
Either more or less stable; depends on the compound
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
∞
-ve
0
+ve
Eutectic
Triple
Plait
Critical
Low T, low P
High T, high P
Low T, high P
High T, low P
Temperature
Pressure
Volume
None of these
∞
0
Maximum
Minimum
F = E - TS
F = H - TS
F = H + TS
F = E + TS
Reverse Carnot cycle
Ordinary vapour-compression cycle
Vapour-compression process with a reversible expansion engine
Air refrigeration cycle
Chemical potential
Surface tension
Heat capacity
None of these
Volume
Mass
Critical temperature
None of these
Calorific value
Heat of reaction
Heat of combustion
Heat of formation
μ = (∂P/∂T)H
μ = (∂T/∂P)H
μ = (∂E/∂T)H
μ = (∂E/∂P)H
Heat pump
Heat engine
Carnot engine
None of these
Molecular size
Volume
Pressure
Temperature
Zero
Unity
Infinity
Negative
Positive
Negative
Zero
May be positive or negative
Mole fraction
Activity
Pressure
Activity co-efficient
Heating occurs
Cooling occurs
Pressure is constant
Temperature is constant
dP/dT = ΔH/TΔV
ln P = - (ΔH/RT) + constant
ΔF = ΔH + T [∂(ΔF)/∂T]P
None of these
F = A + PV
F = E + A
F = A - TS
F = A + TS
A real gas on expansion in vacuum gets heated up
An ideal gas on expansion in vacuum gets cooled
An ideal gas on expansion in vacuum gets heated up
A real gas on expansion in vacuum cools down whereas ideal gas remains unaffected
0
+ve
-ve
∞
Direction of energy transfer
Reversible processes only
Irreversible processes only
None of these
Vant-Hoff equation
Le-Chatelier's principle
Arrhenius equation
None of these
Joule-Thomson co-efficient
Specific heat at constant pressure (Cp)
co-efficient of thermal expansion
Specific heat at constant volume (CV)
Contracts
Expands
Does not change in volume
Either (A), (B) or (C)
T2/(T1 - T2)
T1/(T1 - T2)
(T1 - T2)/T1
(T1 - T2)/T2
0
∞
+ve
-ve
0
1
2
3