1
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
2
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
3
AIEEE 2005
+4
-1
For the reaction 2NO2 (g) $$\leftrightharpoons$$ 2NO (g) + O2 (g), (Kc = 1.8 $$\times$$ 10-6 at 184oC) (R = 0.0831 kJ/(mol. K))
When Kp and Kc are compared at 184oC , it is found that :
A
Kp is greater than Kc
B
Kp is less than Kc
C
Kp = Kc
D
Whether Kp is greater than, less than or equal to Kc depends upon the total gas pressure
4
AIEEE 2005
+4
-1
An amount of solid NH4HS is placed in a flask already containing ammonia gas at a certain temperature and 0.50 atm. Pressure. Ammonium hydrogen sulphide decomposes to yield NH3 and H2S gases in the flask. When the decomposition reaction reaches equilibrium, the total pressure in the flask rises to 0.84 atm. The equilibrium constant for NH4HS decomposition at this temperature is :
A
0.30
B
0.11
C
0.17
D
0.18
EXAM MAP
Medical
NEET