Bond dissociation enthalpy of H2,CI2 and HCI are 434, 242 and 431 kJ mol-1 respectively. Enthalpy of formation of HCI is
93 kJ mol-1
-245 kJ mol-1
-93 kJ mol-1
245 kJ mol-1
The enthalpy of combustion of H2, cyclohexene (C6H10) and cyclohexane (C6H12) are - 241, -3800 and -3920 kJ per mol respectively. Heat of hydrogenation of cyclohexene is
- 121 kJ per mol
+ 121 kJ per mol
+ 242 kJ per mol
- 242 kJ per mol
The enthalpy and entropy change for the reaction
Br2 (l) + CI2 (g) → 2BrCI (g)
are 30 kJ mol-1 and 105 JK mol-1 respectively. The temperature at which the reaction will be in equilibrium is
285.7 K
273 K
450 K
300 K
Heat of combustion ΔHo for C(s), H2(g) and CH4(g) are -94, -68 and -213 kcal/mol. Then, ΔHo for C(s) + 2H2(g)→ CH4 (g) is
-17 kcal
-111 kcal
-170 kcal
-85 kcal
For which one of the following equations equal to for the product ?
Xe(g) + 2F2 (g) → XeF4 (g)
2CO(g) + O2 (g) → 2CO2 (g)
N2(g) + O3 (g) → N2 O3(g)
CH4(g) + 2CI2 (g) → CH2 CI2 (l) + 2HCI (g)
The correct relationship between free energy and equilibrium constant K of a reaction is
Go = - RT In K
G = RT In K
Go = RT In K
G = - RT In 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
1523.6 kJ mol-1
-243.6 kJ mol-1
-120.0 kJ mol-1
553.0 kJ mol-1
For the reaction,
C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(l) at constant temperature, H - E is
+ 3RT
- RT
+ RT
- 3RT
The molar heat capacity 'C' of water at constant pressure is 75 JK-1 mol-1, when 1.0 kJ of heat is supplied to 100 g of water which is free to expand, the increase in temperature of water is
4.8 K
6.6 K
1.2 K
2.4 K
Change in enthalpy for reaction
2H2O2(l) → 2H2O(l) + O2 (g)
if heat of formation of H2O2(l) and H2O(l) are -188 and -286 kJ/mol respectively is,
-196 kJ/mol
+ 196 kJ/mol
+ 948 kJ/mol
-948 kJ/mol
