1
AIEEE 2006
MCQ (Single Correct Answer)
+4
-1
The standard enthalpy of formation $$\Delta _fH^o$$ at 298 K for methane, CH4(g), is –74.8 kJ mol–1. The additional information required to determine the average energy for C – H bond formation would be :
A
the dissociation energy of H2 and enthalpy of sublimation of carbon
B
latent heat of vapourization of methane
C
the first four ionization energies of carbon and electron gain enthalpy of hydrogen
D
the dissociation energy of hydrogen molecule, H2
2
AIEEE 2006
MCQ (Single Correct Answer)
+4
-1
($$\Delta H - \Delta U$$) for the formation of carbon monoxide (CO) from its elements at 298 K is : (R = 8.314 J K–1 mol–1)
A
–1238.78 J mol–1
B
1238.78 J mol–1
C
–2477.57 J mol–1
D
2477.57 J mol–1
3
AIEEE 2005
MCQ (Single Correct Answer)
+4
-1
Consider the reaction: N2 + 3H2 $$\to$$ 2NH3 carried out at constant temperature and pressure. If $$\Delta H$$ and $$\Delta U$$ are the enthalpy and internal energy changes for the reaction, which of the following expressions is true?
A
$$\Delta H$$ > $$\Delta U$$
B
$$\Delta H$$ < $$\Delta U$$
C
$$\Delta H$$ = $$\Delta U$$
D
$$\Delta H$$ = 0
4
AIEEE 2005
MCQ (Single Correct Answer)
+4
-1
If the bond dissociation energies of XY, X2 and Y2 (all diatomic molecules) are in the ratio of 1:1:0.5 and $$\Delta H_f$$ for the formation of XY is -200 kJ mole-1. The bond dissociation energy of X2 will be :
A
100 kJ mol-1
B
200 kJ mol-1
C
300 kJ mol-1
D
800 kJ mol-1
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