Which of the following statements is correct for a reversible process in a state of equilibrium?
1. G = - 2.30RT log K
2. G = 2.30RT log K
3. Go = - 2.30RT log K
4. Go = 2.30RT log K
Which of the following statements is correct for the spontaneous adsorption of a gas ?
1. S is negative and therefore, H should be highly positive
2. S is negative and therefore, H should be highly negative
3. S is positive and therefore, H should be negative
4. S is positive and therefore, H should also be highly positive
Given the reaction :
X2O4(l) → 2XO2(g)
ΔU = 2.1 kcal, ΔS = 20 cal K–1 at 300 K
The value of ΔG is:
1. 2.7 kcal
2. -2.7 kcal
3. 9.3 kcal
4. -9.3 kcal
In which of the following reactions, standard reaction entropy change is positive and standard Gibb's energy change decreases sharply with increasing temperature?
The enthalpy of fusion of water is 1.435 kcal/mol. The molar entropy change for the melting of ice at 0 oC is:
1. 10.52 cal/(mol K)
2. 21.04 cal/(mol K)
3. 5.260 cal/(mol K)
4. 0.526 cal/(mol K)
Standard enthalpy of vaporization for water at 1000C is 40.66 Kj mol-1. The internal energy of vaporization of water at 1000C (in kJ mol-1) is
(Assume water vapour to behave like an ideal gas).
Which of the following is the correct option for free expansion of an ideal gas under adiabatic condition?
Given the following reaction:
The enthalpy change for the reaction is -869.6 kJ. The dissociation energy of the H-H bond is -
1. -869.6 kJ
4. -434.8 kJ
Standard entropies of X2, Y2 and XY3 are 60, 40 and 50JK-1mol-1 respectively. For the reaction
to be at equilibrium, the temperature should be
1. 750 K
2. 1000 K
3. 1250 K
4. 500 K