Equilibrium Tes...

At $$ 1000^0 C $$ and a pressure of 16 atm, the equilibrium constant of the reaction :
$$ CO_2(g) + C(s) \leftrightharpoons 2CO(g) $$
is such that for every nine moles of CO, there is one mole of $$ CO_2 $$ for what pressure of the mixture, is the ratio $$ CO : CO_2 = 4 :1 $$ ? the temperature remains $$ 1000^0 $$C

For the reaction : $$ 2NOBr(g) \leftrightharpoons 2NO(g) +Br_2(g) $$ the ratio $$ \dfrac {K_p}{P} $$ , where P is the total pressure of gases at equilibrium and $$ P_{Br_2} = \dfrac {P}{9} $$ at a certain temperature, is

In the equilibrium mixture: $$ H_2(g) +I_2(g)  \leftrightharpoons 2HI(g) $$, the mole ratios of gases are $$ \sqrt 2 : \sqrt 2 : 10 $$, respectively. What would be the effect on the mole ratio on adding 5 mole of inert gas at constant pressure?

The equilibrium : $$ SOCl_2(g) \leftrightarrow SO_2(g) +Cl_2(g) $$ is attained at $$ 25^0 C $$ in a closed container and helium gas is introduced. Which of the following statements is correct?

When pressure is applied to the equilibrium system: Ice $$ \leftrightharpoons $$ water, which of the following phenomenon will happen?

Which of the following hypothetical reactions is favoured by increases of temperature as well as pressure?

An amount of 16 moles $$H_2$$ and 4 moles of $$N_2$$ is confined in a vessel of volume one liter. The vessel is heated to a constant temperature unit the equilibrium, the pressure was found to be $$ 9/10^{Th} $$ of the initial pressure. The value of $$K_c$$ for the reaction: $$N_2(g) + 3H_2(g) \leftrightharpoons 2NH_3(g)$$ is:

When $$20 ml$$ of $$0.2 M - DCl$$ solution is mixed with $$80 ml$$ of $$0.1 M - NaOD$$ solution, $$pD$$ of the resulting solution becomes $$13.6$$. The ionic product of heavy water, $$D_{2}O$$, is

A $$40.0 ml$$ solution of weak base, $$BOH$$ is titrated with $$0.1 N - HCl$$ solution. The $$pH$$ of the solution is found to be $$10.0$$ and $$9.0$$ after adding $$5.0 ml$$ and $$20.0 ml$$ of the acid, respectively. The dissociation constant of the base is ($$log 2 = 0.3$$)

The process: $$ 2A(g) \rightleftharpoons A_2(g) $$ has $$ K_p = 8 \times 10^8  atm^{-1} .$$ If 'A' atoms are taken at 1 atm pressure, what should be the equilibrium pressure of 'A' ?