1
AIPMT 2014
+4
-1
Using the Gibb's energy change, $$\Delta$$Go = +63.3 kJ, for the following reaction,

Ag2CO3(s) $$\rightleftharpoons$$ 2 Ag+(aq) + CO32$$-$$ (aq)
the Ksp of Ag2CO3(s) in water at 25oC is
(R = 8.314 J K$$-$$1 mol$$-$$1)
A
3.2 $$\times$$ 10$$-$$26
B
8.0 $$\times$$ 10$$-$$12
C
2.9 $$\times$$ 10$$-$$3
D
7.9 $$\times$$ 10$$-$$2
2
AIPMT 2014
+4
-1
For a given exothermic reaction, Kp and K'p are the equilibrium constants at temperatures T1 and T2, respectively. Assuming that heat of reaction is constant in temperature range between T1 and T2, it is readily observed that
A
Kp > K'p
B
Kp < K'p
C
Kp = K'p
D
Kp = $${1 \over {k{'_p}}}$$
3
AIPMT 2014
+4
-1
For the reversible reaction,
N2(g) + 3H2(g) $$\rightleftharpoons$$ 2NH3(g) + heat

The equilibrium shifts in forward direction
A
by increasing the concentration of NH3(g)
B
by decreasing the pressure
C
by decreasing the concentrations of N2(g) and H2(g)
D
by increasing pressure and decreasiing temperature.
4
AIPMT 2012 Mains
+4
-1
Given that the equilibrium constant for the reaction,
2SO2(g) + O2(g) $$\rightleftharpoons$$ 2SO3(g)
has a value of 278 at a particular temperature. What is the value of the equilibrium constant for the following reaction at the same temperature ?
SO3(g) $$\rightleftharpoons$$ SO2(g) + $${1 \over 2}$$ O2(g)
A
1.8 $$\times$$ 10$$-$$3
B
3.6 $$\times$$ 10$$-$$3
C
6.0 $$\times$$ 10$$-$$2
D
1.3 $$\times$$ 10$$-$$5
EXAM MAP
Medical
NEET