CBSE
Multiple Choice QuestionsWhich 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
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
A reaction having equal energies of activation for forward and reverse reactions has
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
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
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)
Which of the following statement is correct for the spontaneous absorption of a gas?
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
Which of the following is the correct option for free expansion of an ideal gas under an adiabatic condition?
