1
AIEEE 2010
MCQ (Single Correct Answer)
+4
-1
The standard enthalpy of formation of NH3 is –46.0 kJ mol–1. If the enthalpy of formation of H2 from its atoms is –436 kJ mol–1 and that of N2 is –712 kJ mol–1, the average bond enthalpy of N–H bond in NH3 is :
A
–964 kJ mol–1
B
+352 kJ mol–1
C
+ 1056 kJ mol–1
D
–1102 kJ mol–1
2
AIEEE 2010
MCQ (Single Correct Answer)
+4
-1
For a particular reversible reaction at temperature T, ∆H and ∆S were found to be both +ve. If Te is the temperature at equilibrium, the reaction would be spontaneous when :
A
Te > T
B
T > Te
C
Te is 5 times T
D
T = Te
3
AIEEE 2009
MCQ (Single Correct Answer)
+4
-1
On the basis of the following thermochemical data :
($$\Delta _fG^oH^+_{(aq)}$$ = 0)

H2O(l) $$\to$$ H+(aq) + OH-(aq); $$\Delta H$$ = 57.32 kJ
H2(g) + $${1 \over 2} O_2(g) \to$$ H2O(l); $$\Delta H$$ = -286.20 kJ

The value of enthalpy of formation of OH ion at 25oC is :
A
-22.88 kJ
B
-228.88 kJ
C
+228.88 kJ
D
-343.52 kJ
4
AIEEE 2008
MCQ (Single Correct Answer)
+4
-1
Oxidising power of chlorine in aqueous solution can be determined by the parameters indicated below:
$${1 \over 2}C{l_2}(g)$$ $$\buildrel {{1 \over 2}{\Delta _{diss}}{H^\Theta }} \over \longrightarrow $$ $$Cl(g)$$ $$\buildrel {{\Delta _{eg}}{H^\Theta }} \over \longrightarrow $$ $$C{l^ - }(g)$$ $$\buildrel {{\Delta _{Hyd}}{H^\Theta }} \over \longrightarrow $$ $$C{l^ - }(aq)$$
(Using the data, $${\Delta _{diss}}H_{C{l_2}}^\Theta $$ = 240 kJ/mol, $${\Delta _{eg}}H_{Cl}^\Theta $$ = -349 kJ/mol, $${\Delta _{hyd}}H_{C{l^ - }}^\Theta $$ = - 381 kJ/mol) will be :
A
+152 kJ mol−1
B
−610 kJ mol−1
C
−850 kJ mol−1
D
+120 kJ mol−1
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