For the reaction,
2SO2(g) + O2(g) = 2SO3(g), $$\Delta $$H = –57.2 kJ mol–1
and KC = 1.7 × 1016 Which of the following statement is incorrect ?
A
The equilibrium will shift in forward direction as the pressure increase.
B
The addition of inert gas at constant volume will be not affect the equilibrium constant.
C
The equilibrium constant is large suggestive of reaction going to completion and so no catalyst is
required.
D
The equilibrium constant decreases as the temperature increase.
2
JEE Main 2019 (Online) 8th April Evening Slot
MCQ (Single Correct Answer)
+4
-1
For the following reactions, equilibrium
constants are given :
S(s) + O2(g) ⇋ SO2(g); K1 = 1052
2S(s) + 3O2(g) ⇋ 2SO3(g); K2 = 10129
The equilibrium constant for the reaction,
2SO2(g) + O2(g) ⇋ 2SO3(g) is :
A
10181
B
1025
C
1077
D
10154
3
JEE Main 2019 (Online) 12th January Morning Slot
MCQ (Single Correct Answer)
+4
-1
In a chemical reaction,
the initial concentration of B was 1.5 times of the
concentration of A, but the equilibrium concentrations of A and B were found to be equal. The equilibrium constant (K) for the aforesaid chemical reaction is -
A
16
B
1
C
1/4
D
4
4
JEE Main 2019 (Online) 12th January Morning Slot
MCQ (Single Correct Answer)
+4
-1
Two solids dissociate as follows –
The total pressure when both the solids dissociated simultaneously is -