A mixture of $3.8$ moles of $NO$ and $0.924$ moles of $C{O}_2$ was allowed to react in a $1.0L$ container. The equilibrium mixture contains $0.124$ mole of $C{O}_2$. Calculate $K_c$ for the reaction:
$N{O}_{\left(g\right)}+C{O}_{\left(2\right(g)}\rightleftharpoons N{O}_{2\left(g\right)}+C{O}_{\left(g\right)}$.

Q. At $675K$, $H_2\left(g\right)$ and $C{O}_2\left(g\right)$ react to form $CO\left(g\right)$ and $H_{2}O\left(g\right),K_p$ for the reaction is $0.16$. If a mixture of $0.25$ mole of $H_2$(g) and $0.25$ mole of $C{O}_2$ is heated at $675K$, mole percentage of $CO\left(g\right)$ in equilibrium mixture is:

Q. At $675$K, $H_2\left(g\right)$ and $C{O}_2\left(g\right)$ react to form $CO\left(g\right)$ and $H_{2}O\left(g\right)$, $K_p$ for the reaction is $0.16$. If a mixture of $0.25$ mole of $H_2\left(g\right)$ and $0.25$ mol of $C{O}_2$ is heated at $675$K, mole $\%$ of $CO\left(g\right)$ in equilibrium mixture is:

Q. At a certain temperature, the following equilibrium is established, $CO\left(g\right)+N{O}_2\left(g\right)\leftrightharpoons C{O}_2\left(g\right)+NO\left(g\right)$. One mole of each of four gases in mixed in a one-litre container and the reaction is allowed to reach an equilibrium state. When an excess of baryta water is added to the equilibrium mixture, the weight of white precipitate obtained is 236.49 g. The equilibrium constant $K_c$ of the reaction is

Q. In an experiment, $onemole$ of acetic acid and $onemole$ of alcohol were allowed to react until equilibrium was established. The equilibrium mixture was found to contain $2/3mole$ of the ester. Calculate the equilibrium constant of the reaction.

Q. A mixture of $3$ moles of ${SO}_2$, $4$ moles of ${NO}_2$ and $4$ moles of $NO$ is placed in a $2.0L$ vessel.