Equilibrium Tes...

For the reaction, $$H_2(g)+I_2(g)\rightleftharpoons 2HI(g)$$, the equilibrium constant $$K_p$$ changes with :

The equilibrium constant K for the reaction $$2HI(g)\rightleftharpoons H_2(g)+I_2(g)$$ at room temperature is $$2.85$$ and that at $$698K$$ is $$1.4\times 10^{-2}$$. This implies :

According to le-Chatelier 's principle, adding heat to a solid and liquid in equilibrium will cause the :

$$CaCO_3(s)\rightleftharpoons CaO(s)+CO_2(g)$$ in closed container at equilibrium. What would be the effect of addition of $$CaCO_3$$ on the equilibrium concentration of $$CO_2$$ :

For a reaction $$A(g)\rightleftharpoons B(g)+C(g). K_p$$ at $$400^oC$$ is $$1.5\times 10^{-4}$$ and $$K_p$$ at $$600^oC$$ is $$6\times 10^{-3}$$. Which statement is incorrect?

In the formation of nitric acid, $$N_2$$ and $$O_2$$ are made to combine. Thus, $$N_2+O_2\rightleftharpoons 2NO-Heat$$ which of the following condition will favour the formation of $$NO$$?

In which of the following reaction, the yield of the products does not increase by increase in the pressure?

Which of the following will not change the concentration of ammonia in the equilibrium?
$$N_2(g)+3H_2(g)\rightleftharpoons 2NH_3(g); \Delta H=-x kJ$$

Which of the following factors will favour the reverse reaction in a chemical equilibrium?

Le Chatelier's principle is applicable to what  equilibrium.