Simultaneous Equilibria

Two solid compounds $\mathrm{A}$ and $\mathrm{B}$ dissociate into gaseous products at $20°\mathrm{C}$ as:
$\mathrm{A}\left(\mathrm{s}\right)\rightleftharpoons {\mathrm{A}}^{\text{'}}\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right)$

$\mathrm{B}\left(\mathrm{s}\right)\rightleftharpoons {\mathrm{B}}^{\text{'}}\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right)$

At $20°\mathrm{C}$, the pressure over excess solid $\mathrm{A}$ is $50 \mathrm{mm}$ and that over excess solid $\mathrm{B}$ is $68 \mathrm{mm}$, find:

(a) The dissociation constant of $\mathrm{A}$ and $\mathrm{B}$

(b) Relative number of moles of $\mathrm{A}\text{'}$ and $\mathrm{B}\text{'}$ in the vapour phase over a mixture of solid $\mathrm{A}$ and $\mathrm{B}$.

Hydrazine was taken in a constant volume container at ${27}^0\mathrm{C}$ and $\text{1.0 atm}$ and equal moles of oxygen gas were introduced, sealed and heated. Following equilibria established.

${\text{N}}_2{\text{H}}_4+30_2\rightleftharpoons 2{\text{NO}}_2\left(\text{g}\right)+2{\text{H}}_2\text{O}\text{;}{\text{Kp}}_1=4$
$\begin{array}{c}{\text{N}}_2{\text{H}}_4\rightleftharpoons {\text{N}}_2+2{\text{H}}_2\text{;}{\text{Kp}}_2=\text{?}\\ {\text{N}}_2{\text{H}}_4+{\text{H}}_2\rightleftharpoons 2{\text{NH}}_3\text{;}{\text{Kp}}_3=\text{?}\end{array}$

The gaseous mixture on passing through moisture absorbent, a decrease of $360\mathrm{mm}$ in equilibrium pressure observed. The dried gaseous mixture passed through Ammonia absorber, a further decrease of $20\mathrm{mm}$ in equilibrium pressure observed. After calculating ${\mathrm{K}}_{{\mathrm{P}}_2}$, report the value of ${\mathrm{K}}_{{\mathrm{P}}_3}$$\left({\mathrm{K}}_{{\mathrm{P}}_3}=\mathrm{n}\times {10}^{-3}\right)$. Find value of n after round-off in integer.

${\mathrm{ \; K}}_{\mathrm{c}}$ for the reaction; $\left[\mathrm{A}\mathrm{g}{\left(\mathrm{C}\mathrm{N}\right)}_2\right]–\mathrm{ }\mathrm{A}{\mathrm{g}}^{+}\rightleftharpoons \mathrm{ }+\mathrm{ }2\mathrm{C}{\mathrm{N}}^{–}$ , the equilibrium constant at $25°\mathrm{C}$ is

$4.0\mathrm{ }\times \mathrm{ }{10}^{–19}$, then the silver ion concentration in a solution which was originally $0.1$ molar in $\mathrm{K}\mathrm{C}\mathrm{N}$ and $0.03\mathrm{ }\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{a}\mathrm{r}$ in ${\mathrm{A}\mathrm{g}\mathrm{N}\mathrm{O}}_3$ is -

Two system ${\text{PCl}}_5\left(\text{g}\right)\rightleftharpoons {\text{PCl}}_3\left(\text{g}\right)+{\text{Cl}}_2\left(\text{g}\right)$ and ${\text{COCl}}_2\left(\text{g}\right)\rightleftharpoons \text{CO}\left(\text{g}\right)+{\text{Cl}}_2\left(\text{g}\right)$ are simultaneously in equilibrium in a vessel at constant volume. If some CO is introduced into the vessel then at new equilibrium the concentration of –

Calculate the partial pressure of carbon monoxide from the following datas

$\mathrm{C}\mathrm{a}\mathrm{C}{\mathrm{O}}_3\mathrm{(s)}\stackrel{∆}{\to }\mathrm{C}\mathrm{a}\mathrm{O}\left(\mathrm{s}\right)+\mathrm{C}{\mathrm{O}}_2(g)K_p=8\times {10}^{-2}$

${\mathrm{CO}}_2\left(\mathrm{g}\right)+\mathrm{C}\left(s\right)\to 2\mathrm{C}\mathrm{O}\left(\mathrm{g}\right), K_p=2$

$\mathrm{A}{\mathrm{g}}^{+}+\mathrm{N}{\mathrm{H}}_3\rightleftharpoons {\left[\mathrm{A}\mathrm{g}\left(\mathrm{N}{\mathrm{H}}_3\right)\right]}^{+}; K_1=3.5\times {10}^{-3}$

${\left[\mathrm{A}\mathrm{g}\left(\mathrm{N}{\mathrm{H}}_3\right)\right]}^{+}+\mathrm{N}{\mathrm{H}}_3\rightleftharpoons {\left[\mathrm{A}\mathrm{g}{\left({\mathrm{N}\mathrm{H}}_3\right)}_2\right]}^{+};\mathrm{ }$

$\mathrm{ }{K}_2=1.7\times {10}^{-3}$

Then the formation constant of ${\left[\mathrm{A}\mathrm{g}{\left({\mathrm{N}\mathrm{H}}_3\right)}_2\right]}^{+}$ is

When N₂O₅ is heated at certain temperature, it dissociates as

          ${\text{N}}_2{\text{O}}_5\left(\text{g}\right)\rightleftharpoons {\text{N}}_2{\text{O}}_3\left(\text{g}\right)+{\text{O}}_2\left(\text{g}\right),K_{\text{c}}=\text{2.5}$

at the same time N₂O₃ also decomposes as ${\text{N}}_2{\text{O}}_3\left(\text{g}\right)\rightleftharpoons {\text{N}}_2\text{O}\left(\text{g}\right)+{\text{O}}_2\left(\text{g}\right)$
In initially 4 mol of N₂O₅ are taken in 1 L flask and allowed to dissociate, concentration of O₂ at equilibrium is 2.5 M, equilibrium concentration of N₂O₃ will be

The two equilibrium, $\text{AB}\rightleftharpoons {\text{A}}^{+}+{\text{B}}^{-}$  and  $\text{AB}+{\text{B}}^{-}\rightleftharpoons {\text{AB}}_2^{-}$  are simultaneously maintained in a solution with equilibrium constants, K₁ and K₂ respectively. The ratio of  [A⁺] and $\left[{\text{AB}}_2^{-}\right]$  in the solution is

Hydrazine was taken in a constant volume container at 27^oc and 1.0 atm and equal moles of oxygen gas were introduced, sealed and heated following equlibria established

${\text{N}}_2{\text{H}}_4+30_2\rightleftharpoons 2{\text{NO}}_2\left(\text{g}\right)+2{\text{H}}_2\text{O}\text{;}{\text{Kp}}_1=4$

$\begin{array}{c}{\text{N}}_2{\text{H}}_4\rightleftharpoons {\text{N}}_2+2{\text{H}}_2\text{;}{\text{Kp}}_2=\text{?}\\ {\text{N}}_2{\text{H}}_4+{\text{H}}_2\rightleftharpoons 2\text{N}{\text{H}}_3\text{;}{\text{Kp}}_3=\text{?}\end{array}$

The gaseous mixture on passing through moisture absorbent, a decrease of 360 mm in equilibrium pressure observed. The dried gaseous mixture passed through Ammonia absorber, a further decrease of 20 mm in equilibrium pressure observed. After calculating Kp₂, report the value of Kp₃

Ammonium sulphide and ammonium selenide on heating dissociates as
(NH₄)₂S(s) $\rightleftharpoons$ 2NH₃(g)+ H₂S(g); K_p1 = 9 × 10^-3 atm³
(NH₄)₂Se(s) $\rightleftharpoons$ 2NH₃(g) + H₂Se(g); K_p2 = 4.5 × 10^-3 atm³
The total pressure over the solid mixture at equilibrium is:

When $\mathrm{NO} \text{and }{\mathrm{NO}}_2$ are mixed, the following equilibrium are readily obtained, $2{\text{NO}}_2\rightleftharpoons {\text{N}}_2{\text{O}}_4\text{,}{\text{K}}_{\text{p}}=6·8{\text{ atm}}^{-1}$ and $\text{NO}+{\text{NO}}_2\rightleftharpoons {\text{N}}_2{\text{O}}_3$. In an experiment when$\mathrm{NO} \text{and }{\mathrm{NO}}_2$  are mixed in the ratio of 1 : 2, the final total pressure was 5.05 atm and the partial pressure of N₂O₄ was 1.7 atm. Calculate (a) the equilibrium partial pressure of NO, (b) K_p for, $\text{NO}+{\text{NO}}_2\rightleftharpoons {\text{N}}_2{\text{O}}_3$

When ${\mathrm{N}}_2{\mathrm{O}}_5$ is heated at a certain temperature, it dissociates as ${\text{N}}_2{\text{O}}_5\left(\text{g}\right)\rightleftharpoons {\text{N}}_2{\text{O}}_3\left(\text{g}\right)+{\text{O}}_2\left(\text{g} \right)$; ${\mathrm{K}}_{\mathrm{c}}=2.5$. At the same time, ${\mathrm{N}}_2{\mathrm{O}}_3$ also decomposes as : ${\text{N}}_2{\text{O}}_3\left(\text{g}\right)\rightleftharpoons {\text{N}}_2\text{O}\left(\text{g}\right)+{\text{O}}_2\left(\text{g} \right)$. If initially, $4.0\mathrm{moles}$ of ${\mathrm{N}}_2{\mathrm{O}}_5$ are taken in $1.0\mathrm{litre}$ flask and allowed to dissociate, the concentration of ${\mathrm{O}}_2$ at equilibrium is $2.5\mathrm{M}$. Equilibrium concentration of ${\mathrm{N}}_2{\mathrm{O}}_5$ is: