1
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
2
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
($$\Delta _fG^oH^+_{(aq)}$$ = 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
3
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
$${1 \over 2}C{l_2}(g)$$ $$\buildrel {{1 \over 2}{\Delta _{diss}}{H^\Theta }} \over \longrightarrow $$ $$Cl(g)$$ $$\buildrel {{\Delta _{eg}}{H^\Theta }} \over \longrightarrow $$ $$C{l^ - }(g)$$ $$\buildrel {{\Delta _{Hyd}}{H^\Theta }} \over \longrightarrow $$ $$C{l^ - }(aq)$$
(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
4
AIEEE 2008
MCQ (Single Correct Answer)
+4
-1
Standard entropy of X2, Y2 and XY3 are 60, 40 and 50 JK−1
mol−1 , respectively. For the reaction,
$${1 \over 2} X_2$$ + $${3 \over 2} Y_2 \to$$ XY3, $$\Delta H$$ = -30 kJ, to be at equilibrium, the temperature will be
$${1 \over 2} X_2$$ + $${3 \over 2} Y_2 \to$$ XY3, $$\Delta H$$ = -30 kJ, to be at equilibrium, the temperature will be
Questions Asked from Thermodynamics (MCQ (Single Correct Answer))
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