1
AIEEE 2008
+4
-1
For the following three reactions a, b and c, equilibrium constants are given:
a. CO (g) + H2O (g) $$\leftrightharpoons$$ CO2(g) + H2 (g) ; K1
b. CH4 (g) + H2O (g) $$\leftrightharpoons$$ CO(g) + 3H2 (g) ; K2
c. CH4 (g) + 2H2O (g) $$\leftrightharpoons$$ CO2(g) + 4H2 (g) ; K3
A
$${K_1}\sqrt {{K_2}} = {K_3}$$
B
K2K3 = K1
C
K3 = K1K2
D
K3.$$K_2^3$$ = $$K_1^2$$
2
AIEEE 2006
+4
-1
Phosphorus pentachloride dissociates as follows, in a closed reaction vessel
PCl5 (g) $$\leftrightharpoons$$ PCl3 (g) + Cl2 (g)
If total pressure at equilibrium of the reaction mixture is P and degree of dissociation of PCl5 is x, the partial pressure of PCl3 will be
A
$$\left( {{x \over {x + 1}}} \right)P$$
B
$$\left( {{2x \over {1 - x}}} \right)P$$
C
$$\left( {{x \over {x - 1}}} \right)P$$
D
$$\left( {{x \over {1 - x}}} \right)P$$
3
AIEEE 2006
+4
-1
The equilibrium constant for the reaction
SO3 (g) $$\leftrightharpoons$$ SO2 (g) + $$1 \over 2$$ O2 (g)
is Kc = 4.9 $$\times$$ 10–2. The value of Kc for the reaction
2SO2 (g) + O2 (g) $$\leftrightharpoons$$ 2SO3 (g) will be :
A
416
B
9.8 $$\times$$ 10-2
C
4.9 $$\times$$ 10-2
D
2.40 $$\times$$ 10-3
4
AIEEE 2005
+4
-1
The exothermic formation of ClF3 is represented by the equation:
Cl2 (g) + 3F2 (g) $$\leftrightharpoons$$ 2ClF3 (g); $$\Delta H$$ = -329 kJ
Which of the following will increase the quantity of ClF3 in an equilibrium mixture of Cl2, F2 and ClF3?
A
Increasing the temperature
B
Removing Cl2
C
Increasing the volume of the container
D