Q. No.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
1. \(\Delta \mathrm{q} \neq 0, \Delta \mathrm{~T}=0, \mathrm{~W}=0 \)
2. \(\Delta \mathrm{q}=0, \Delta \mathrm{~T}=0, \mathrm{~W}=0 \)
3. \(\Delta \mathrm{q}=0, \Delta \mathrm{~T}<0, \mathrm{~W} \neq 0 \)
4. \(\Delta \mathrm{q}=0, \Delta \mathrm{~T} \neq 0, \mathrm{~W}=0\)
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
Give 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 following reaction will be:
2. -243.6 kJ mol-1
3. -120.0 kJ mol-1
4. 553.0 kJ mol-1
The values of ΔH and ΔS for the given reaction are 170 kJ and 170 JK-1, respectively.
C(graphite) + CO2(g)→2CO(g)
This reaction will be spontaneous at:
1. 710 K
2. 910 K
3. 1110 K
4. 510 K
(I) q + W
(II) q
(III) W
(IV) H - TS
1. (I) and (IV)
2. (II), (III) and (IV)
3. (I), (II) and (III)
4. (II) and (III)
which of the following conditions is correct?
1. ΔH = 0 and ΔS < 0
2. ΔH > 0 and ΔS > 0
3. ΔH < 0 and ΔS < 0
4. ΔH > 0 and ΔS < 0
1. 93 kJ mol-1
2. - 245 kJ mol-1
3. -93 kJ mol-1
4. 245 kJ mol-1
Consider the following reactions:
| (i) | H+(aq) + OH-(aq) → H2O(l) ΔH = -x1 kJmol-1 |
| (ii) | H2(g) + 1/2O2(g) → H2O(l) ΔH = -x2 kJmol-1 |
| (iii) | CO2(g) + H2(g) → CO (g) + H2O(l) ΔH = -x3 kJmol-1 |
| (iv) | C2H2(g) + 5/2O2(g) → 2CO2 + H2O(l) ΔH = -x4 kJmol-1 |
Enthalpy of formation of H2O(l) is :
1.
2.
3.
4.
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