Equilibrium Tes...

The equilibrium constant in reversible reaction at a given temperature-

$$PCl_5$$ dissociates as $$PCl_{5}(g)\rightleftharpoons  PCl_{3} (g) + Cl_{2}(g)$$. If $$PCl_{5}$$ is 10% dissociated at 1 atm, then the percentage of dissociation at 4 atm is:

A reversible chemical reaction having two reactants in equilibrium. If the concentration of the reactants are doubled, then the equilibrium constant will______.

The equilibrium constant for the reaction $$H_{2}+I_{2}  \rightleftharpoons  2HI$$ is 50. If the volume of the container is reduced to half of its original value, the value of  the equilibrium constant will be:

Increase in pressure shifts the equilibrium of the reaction

$$N_{2}(g) + 3H_{2}(g) \rightarrow 2NH_{3}(g)$$

The following reaction is at equilibrium in a given cylinder of constant volume.
                     $$N_2 (g) + 3 H_2 (g) \Leftrightarrow 2NH_3 (g)$$
Addition of argon gas to the cylinder will

When $$NaNO_3$$ is heated in a closed vessel, oxygen is liberated and $$NaNO_2$$ is left behind. At equilibrium:

The following equilibrium in a closed container $$N_2O_4(g)\rightleftharpoons 2NO_2(g)$$
At a fixed temperature, the volume of the reaction container is halved. For this change, which of the following statements holds true regarding the equilibrium constant $$(K_p)$$ and degree of dissociation?

A 10L container at 300 K contains CO$$_2$$ gas at a pressure of 0.2 atm and an excess solid CaO (neglect the volume of solid CaO). The volume of a container is now decreased by moving the movable piston fitted in the container. What will be the maximum volume of a container when a pressure of CO$$_2$$ attains its maximum value? 

Which of the following statements is incorrect?