Match List I (Equations) with List II (Type of processes) and select the correct option.
List I
List II
Equations
Type of processes
A.
Kp > Q
(i)
Non- spontaneous
B.
$$\Delta $$Go < RT ln Q
(ii)
Equilibrium
C.
Kp = Q
(iii)
Spontaneous and endothermic
D.
T > $${{\Delta H} \over {\Delta S}}$$
(iv)
Spontaneous
A
A - (i), B - (ii), C - (iii), D - (iv)
B
A - (iii), B - (iv), C - (ii), D - (i)
C
A - (iv), B - (i), C - (ii), D - (iii)
D
A - (ii), B - (i), C - (iv), D - (iii)
2
AIPMT 2010 Prelims
MCQ (Single Correct Answer)
+4
-1
For an endothermic reaction, energy of activation is Ea and enthalpy of reaction is $$\Delta $$H (both of these in kJ/mol). Minimum value of Ea will be
A
less than $$\Delta $$H
B
equal to $$\Delta $$H
C
more than $$\Delta $$H
D
equal to zero
3
AIPMT 2010 Prelims
MCQ (Single Correct Answer)
+4
-1
Standard entropies of X2, Y2 and XY3 are 60, 40 and 50 J K$$-$$1 mol$$-$$1 respectively. For the reaction
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
