The correct statement for a reversible process in a state of equilibrium is:
1. G = – 2.30RT log K
2. G = 2.30RT log K
3. Go = – 2.30RT log K
4. Go = 2.30RT log K
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, the standard reaction entropy change
is positive, and standard Gibb's energy change
decreases sharply with increasing temperature?
1. | C(graphite) + \(\frac{1}{2}\)O2(g) → CO(g) |
2. | CO(g) + \(\frac{1}{2}\)O2(g) → CO2(g) |
3. | Mg(s) + \(\frac{1}{2}\)O2(g) → MgO(s) |
4. | \(\frac{1}{2}\)C(graphite) + \(\frac{1}{2}\)O2(g) → \(\frac{1}{2}\)CO2(g) |
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)
The standard enthalpy of vaporization for water at 100 oC is 40.66 kJ mol-1.
The internal energy of vaporization of water at 100 oC (in kJ mol-1) is:
(Assume water vapour behaves like an ideal gas.)
1. +37.56
2. -43.76
3. +43.76
4. +40.66
Identify which of the following is the correct option for free expansion of an ideal gas under adiabatic condition.
1.
2.
3.
4.
Given the following reaction:
\(4H(g)\)→ \(2 H_{2}\)\((g)\)
The enthalpy change for the reaction is -869.6 kJ. The dissociation energy of the H-H bond is:
1. -869.6 kJ
2. +434.8kJ
3. +217.4kJ
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
From the following bond energies:
H—H bond energy: 431.37 kJ mol-1
C=C bond energy: 606.10 kJ mol-1
C—C bond energy: 336.49 kJ mol-1
C—H bond energy: 410.50 kJ mol-1
Enthalpy for the reaction,
will be:
1. | 1523.6 kJ mol-1 | 2. | -243.6 kJ mol-1 |
3. | -120.0 kJ mol-1 | 4. | 553.0 kJ mol-1 |