Chemical Equilibrium Questions

Phosphoric acid ionizes in three steps with their ionization constant values $K_{a1}$, $K_{a2}$ and $K_{a3}$, respectively, while $K$ is the overall ionization constant. Which of the following statements are true?A. $\log K=\log K_{a1}+\log K_{a2}+\log K_{a3}$ B. ${\text{H}}_3{\text{PO}}_4$ is a stronger acid than ${\text{H}}_2{\text{PO}}_4^{-}$ and ${\text{HPO}}_4^{2-}$ C. $K_{a1}>K_{a2}>K_{a3}$ D. $K_{a1}=\frac{K_{a3}+K_{a2}}{2}$ Choose the correct answer from the options given below:

For the reaction $\text{A}(\text{g})\rightleftharpoons 2\text{B}(\text{g})$, the backward reaction rate constant is higher than the forward reaction rate constant by a factor of $2500$, at $1000\text{K}$.[Given : $R=0.0831{\text{L atm mol}}^{-1}{\text{K}}^{-1}$ ]$K_p$ for the reaction at $1000\text{K}$ is:

For the reaction ${\text{N}}_2(\text{g})+{\text{O}}_2(\text{g})\rightleftharpoons 2\text{NO}(\text{g})$, the equilibrium constant is $K_1$. The equilibrium constant is $K_2$ for the reaction $2\text{NO}(\text{g})+{\text{O}}_2(\text{g})\rightleftharpoons 2{\text{NO}}_2(\text{g})$. What is $K$ for the reaction ${\text{NO}}_2(\text{g})\rightleftharpoons \frac{1}{2}{\text{N}}_2(\text{g})+{\text{O}}_2(\text{g})$?

For reaction, $2{\text{NOCl}}_{(g)}\rightleftharpoons 2{\text{NO}}_{(g)}+{\text{Cl}}_{2(g)}$, $K_c$ at $427^{\circ }\text{C}$ is $3\times 10^{-6}{\text{L mol}}^{-1}$. The value of $K_p$ is nearly:

For the chemical equilibrium, ${\text{CaCO}}_{3(s)}\rightleftharpoons {\text{CaO}}_{(s)}+{\text{CO}}_{2(g)}$, $\Delta H_r^{\circ }$ can be determined from which one of the following plots?

The following equilibrium constants are given:

The value of equilibrium constant of the reaction $HI(g)\rightleftharpoons \frac{1}{2}{H}_2(g)+\frac{1}{2}{I}_2(g)$ is $8.0$. The equilibrium constant of the reaction $H_2(g)+I_2(g)\rightleftharpoons 2HI(g)$ will be:

For the reactions $X\rightleftharpoons 2Y$ and $A\rightleftharpoons 2B$, the equilibrium constants are $K_{p1}$ and $K_{p2}$ in the ratio $9:1$. If degree of dissociation is equal, the ratio of total pressures is:

If the concentration of ${\text{OH}}^{-}$ ions in the reaction ${\text{Fe(OH)}}_3(s)\rightleftharpoons {\text{Fe}}^{3+}(aq)+3{\text{OH}}^{-}(aq)$ is decreased by $1/4$ times, then equilibrium concentration of ${\text{Fe}}^{3+}$ will increase by:

The dissociation equilibrium of a gas ${\text{AB}}_2$ is ${\text{2AB}}_2(g)\rightleftharpoons \text{2AB}(g)+{\text{B}}_2(g)$. The expression relating degree of dissociation ($x$) with $K_P$ and total pressure $P$ is:

In which of the following equilibrium $K_c$ and $K_p$ are not equal?

Given that the equilibrium constant for the reaction $2{\text{SO}}_{2(\text{g})}+{\text{O}}_{2(\text{g})}\rightleftharpoons 2{\text{SO}}_{3(\text{g})}$ has a value of $278$ at a particular temperature. What is the value of the equilibrium constant for the following reaction at the same temperature:
$${\text{SO}}_{3(\text{g})}\rightleftharpoons {\text{SO}}_{2(\text{g})}+\frac{1}{2}{\text{O}}_{2(\text{g})}$$

Given the reaction between $2$ gases represented by ${\text{A}}_2$ and ${\text{B}}_2$ to give the compound ${\text{AB}}_{(\text{g})}$. At equilibrium, the concentration of:$[{\text{A}}_2]=3.0\times 10^{-3}\text{M}$$[{\text{B}}_2]=4.2\times 10^{-3}\text{M}$$[\text{AB}]=2.8\times 10^{-3}\text{M}$ If the reaction takes place in a sealed vessel at $527^{\circ }\text{C}$, then the value of $K_c$ for the reaction ${\text{A}}_2+{\text{B}}_2\rightleftharpoons 2\text{AB}$ will be:

If the equilibrium constant for ${\text{N}}_2(g)+{\text{O}}_2(g)\rightleftharpoons 2\text{NO}(g)$ is $K$, the equilibrium constant for $\frac{1}{2}{\text{N}}_2(g)+\frac{1}{2}{\text{O}}_2(g)\rightleftharpoons \text{NO}(g)$ will be:

Consider the following liquid – vapour equilibrium: $\text{Liquid}\rightleftharpoons \text{Vapour}$. Which of the following relations is correct?