Equilibrium Tes...

For which of the following reactions at equilibrium at constant temperature doubling the volume will cause a shift to the right?

On heating a mixture of $${ SO }_{ 2 }{ Cl }_{ 2 }$$ and $$CO$$, two equilibria are simultaneously established:
$${ SO }_{ 2 }{ Cl }_{ 2 }\rightleftharpoons { SO }_{ 2 }+{ Cl }_{ 2 }$$
$$CO(g)+{ Cl }_{ 2 }(g)\rightleftharpoons CO{ Cl }_{ 2 }(g)$$
On adding more $${SO}_{2}$$ at equilibrium what will happen?

In which of the following equilibrium, change in the volume of the system does not alter the number of moles?

The % yield of ammonia as a function of time in the reaction, $${ N }_{ 2 }(g)+3{ H }_{ 2 }(g)\rightleftharpoons 2{ NH }_{ 3 }(g)$$ [$$\Delta H< 0$$] at $$\left( P,{ T }_{ 1 } \right) $$ is given above.
If the reaction is conducted at $$\left( P,{ T }_{ 2 } \right) $$ with $${ T }_{ 2 }>{ T }_{ 1 }$$, the % yield of ammonia as a function of time is represented by:

The equilibrium constants for the reaction, $${Br}_{2}\rightleftharpoons  2Br$$ at $$500K$$ and $$700K$$ are $$1\times { 10 }^{ -10 }$$ and $$1\times { 10 }^{ -5 }$$ respectively. The reaction is:

Le Chatelier's principle is not applicable to:

For the reaction,
$${ N }_{ 2 }(g)+3{ H }_{ 2 }(g)\rightleftharpoons 2{ NH }_{ 3 }(g)+Heat$$
When temperature increases, then:

Select the correct statements about the following reaction:
$$N_2(g)+3H_2(g)\rightleftharpoons 2NH_3(g); \Delta H=-22.4 \, kcal \, mol^{-1}$$

(A) pH of $$10^{-7}$$ M NaOH solution exists between 7 to 7.3 at $$25^o C$$.
(R) Due to common ion effect ionization of water is suppressed. 

 Equilibrium constants are given for the following two equilibria. 
$$(i) A_2(g)+ B_2 (g)\rightleftharpoons 2AB (g);$$          $$K=2 \times 10^{-4}$$
$$(ii) 2AB(g)+ C_2(g) \rightleftharpoons 2ABC (g);$$  $$K= 2\times 10^{-2}\, L \, mol^{-1}$$