1
AIEEE 2007
+4
-1
Assuming that water vapour is an ideal gas, the internal energy change $$\left( {\Delta U} \right)$$ when $$1$$ mol of water is vapourised at $$1$$ bar pressure and $${100^ \circ }C$$ (Given : molar enthalpy of vapourisation of water at $$1$$ bar and $$373$$ $$K$$ $$= 41\,kJ\,mo{l^{ - 1}}\,$$
and $$R = 8.3\,J\,mo{l^{ - 1}}\,{K^{ - 1}}$$ )
A
$$41.00\,kJ\,mo{l^{ - 1}}$$
B
$$4.100\,kJ\,mo{l^{ - 1}}$$
C
$$3.7904\,kJ\,mo{l^{ - 1}}$$
D
$$37.904\,kJ\,mo{l^{ - 1}}$$
2
AIEEE 2006
+4
-1
An ideal gas is allowed to expand both reversibly and irreversibly in an isolated system. If Ti is the initial temperature and Tf is the final temperature, which of the following statements is correct?
A
(Tf)irrev > (Tf)rev
B
(Tf)rev = (Tf)irrev
C
Tf > Ti for reversible process but Tf = Ti for irreversible process
D
Tf = Ti for both reversible and irreversible processes
3
AIEEE 2006
+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
4
AIEEE 2006
+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
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