CBSE
Multiple Choice QuestionsWhich of the following is the correct option for free expansion of an ideal gas under an adiabatic condition?
Which of the following statements is correct for a reversible process in a state of equilibrium?
ΔG = 2.303RT log K
ΔG0 = -2.303RT log K
ΔG0 = -2.303RT log K
If the enthalpy change for the transition of liquid water to steam is 30kJ mol-1 at 27oC, the entropy change for the process would be.
1.0 J mol- K-1
0.1 J mol-1 K-1
100 J mol-1 K-1
10 J mol-1 K-1
For the reaction X2O4 (l) --> 2XO2 (g) ΔU = 2.1 kcal, ΔS = 20 cal K-1 at 300 K hence ΔG is
2.7 kcal
-2.7kcal
9.3 kcal
9.3 kcal
Which of the following statement is correct for the spontaneous absorption of a gas?
In which of the following reactions, standard reaction entropy changes (ΔSo) is positive and standard Gibb's energy change (ΔGo) decreases sharply with increasing temperature?
C (graphite) +1/2 O2 (g) → CO (g)
CO (g) +1/2 (g) → CO2 (g)
Mg(s) +1/2O2 (g) → MgO (s)
Mg(s) +1/2O2 (g) → MgO (s)
A reaction having equal energies of activation for forward and reverse reactions has
Standard enthalpy of vaporisation ΔvapHθ for water for water at 100oC is 40.66 kJ mol-1. The internal energy of vaporisation of water at 100o C (in KJ mol-1) is
(Assume water vapour to behave like an ideal gas.)
+37.56
-43.76
+43.76
+43.76
The enthalpy of fusion of water is 1.435 Kcal/mol. The molar entropy change for the melting of ice of at 0o C is
10.52 cal/(mol K)
21.04 cal/(mol K)
5.260 cal/ (mol K)
5.260 cal/ (mol K)
The correct thermodynamic conditions for the spontaneous reaction at all temperatures is
