Applications of Equilibrium Constant

$\mathrm{A}\left(\mathrm{g}\right)\rightleftharpoons 2 \mathrm{B}( \mathrm{g})+\mathrm{C}\left(\mathrm{g}\right)$

For the given reaction, if the initial pressure is $450 \mathrm{mmHg}$ and the pressure at time $\mathrm{t}$ is $720 \mathrm{mmHg}$ at a constant temperature$\mathrm{T}$ and constant volume $\mathrm{V}$. The fraction of $\mathrm{A}\left(\mathrm{g}\right)$ decomposed under these conditions is $\mathrm{x}\times {10}^{-1}$. The value of $\mathrm{x}$ is (nearest integer)

For a chemical reaction $\mathrm{A}+\mathrm{B}\to$products, the order is one with respect to each A and B. The sum of x and y from the following data is

The equilibrium constant for the reaction

 ${\mathrm{CO}}_{\left(\mathrm{g}\right)}+{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{g}\right)}\iff {\mathrm{CO}}_{2\left(\mathrm{g}\right)}+{\mathrm{H}}_{2\left(\mathrm{g}\right)}$ is $4.0$ at $1000\mathrm{K}$. When equimolar mixtures of $\mathrm{CO} \mathrm{and} {\mathrm{H}}_2\mathrm{O}$ are heated to $1000\mathrm{K}$ the percentage of ${\mathrm{CO}}_2$ formed at equilibrium is 

$102 \mathrm{g}$ of solid ${\mathrm{NH}}_4\mathrm{HS}$ is taken in the $2 \mathrm{L}$ evacuated flask at $57°\mathrm{C}$. Following two equilibrium exist simultaneously.

$$\begin{gathered} {\mathrm{NH}}_4\mathrm{HS}\left(\mathrm{s}\right) \rightleftharpoons {\mathrm{NH}}_3\left(\mathrm{g}\right) + {\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right) \\ {\mathrm{NH}}_3\left(\mathrm{g}\right) \rightleftharpoons \frac{1}{2}{\mathrm{N}}_2\left(\mathrm{g}\right) + \frac{3}{2}{\mathrm{H}}_2\left(\mathrm{g}\right) \end{gathered}$$

One mole of the solid decomposes to maintain both the equilibrium and $0.75 \mathrm{mol}$ of ${\mathrm{H}}_2$ was found at the equilibrium then find the equilibrium concentration of all the species and ${\mathrm{K}}_{\mathrm{c}}$ for both the reaction.

What is the effect of volume change on equilibrium constant ?

$5$ moles of ${\mathrm{S}\mathrm{O}}_2$ and $5$ moles of ${\mathrm{O}}_2$ react in a closed vessel. At equilibrium $60\mathrm{\%}$ of the ${\mathrm{S}\mathrm{O}}_2$ is consumed. The total number of gaseous moles $(\mathrm{S}{\mathrm{O}}_2, {\mathrm{O}}_2\mathrm{ }\mathrm{a}\mathrm{n}\mathrm{d}\mathrm{ }\mathrm{S}{\mathrm{O}}_3)$ in the vessel is:

The equilibrium constant for the reaction between ${\mathrm{CH}}_4 \left(\mathrm{g}\right)$ and ${\mathrm{H}}_2\mathrm{S} \left(\mathrm{g}\right)$ to form ${\mathrm{CS}}_2 \left(\mathrm{g}\right)$ and ${\mathrm{H}}_2 \left(\mathrm{g}\right)$, at $1173 \mathrm{K}$ is $3.6$. For the following composition of the reaction mixture, decide which of the following option is correct?
$$\begin{gathered} \left[{\mathrm{CH}}_4\right]=1.07 \mathrm{M}, \left[{\mathrm{H}}_2\mathrm{S}\right]=1.20 \mathrm{M}, \\ \left[{\mathrm{CS}}_2\right]=0.90 \mathrm{M} , \left[{\mathrm{H}}_2\right]=1.78 \mathrm{M} \end{gathered}$$

A mixture of ${\mathrm{NO}}_2$ and ${\mathrm{N}}_2{\mathrm{O}}_4$ has a vapour density of $38.3$ at $300 \mathrm{K}$. What is the number of moles of ${\mathrm{NO}}_2$ in $100 \mathrm{g}$ of the mixture?

The equilibrium constant for the reaction between ${\mathrm{CH}}_4 \left(\mathrm{g}\right)$ and ${\mathrm{H}}_2\mathrm{S} \left(\mathrm{g}\right)$ to form ${\mathrm{CS}}_2 \left(\mathrm{g}\right)$ and ${\mathrm{H}}_2 \left(\mathrm{g}\right)$, at $1173 \mathrm{K}$ is $3.6$. For the following composition of the reaction mixture, decide which of the following option is correct?
$$\begin{gathered} \left[{\mathrm{CH}}_4\right]=1.07 \mathrm{M}, \left[{\mathrm{H}}_2\mathrm{S}\right]=1.20 \mathrm{M}, \\ \left[{\mathrm{CS}}_2\right]=0.90 \mathrm{M} , \left[{\mathrm{H}}_2\right]=1.78 \mathrm{M} \end{gathered}$$

What is the main purpose of practicing gratitude in the context of enhancing positive emotions?

What is the impact of a price floor set above the equilibrium price?

In a market with free entry and exit, what happens to economic profits in the long run?

What is the primary condition for market equilibrium in a market with a fixed number of firms?

When the market is in equilibrium with a fixed number of firms, what does the equilibrium price ensure?

In a market with a fixed number of firms, if the market price is above the equilibrium price, what would be the result?

What is the term used to describe the price at which the quantity demanded equals the quantity supplied?

If production technology improves, how is the market supply curve affected in a perfectly competitive market?

What does the market supply curve illustrate in a perfectly competitive market?

Which factor affecting depreciation is directly related to the usage of the asset?