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

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

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 reaction at equilibrium

 $\mathrm{A}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{B}\left(\mathrm{g}\right)+\frac{1}{2}\mathrm{C}\left(\mathrm{g}\right)$

 the relation between dissociation constant $\left(\mathrm{K}\right)$, degree of dissociation $\left(\mathrm{\alpha }\right)$ and equilibrium pressure $\left(\mathrm{p}\right)$ is given by :

For the reaction

${\mathrm{H}}_{2\left(\mathrm{g}\right)}+{\mathrm{CO}}_{2\left(\mathrm{g}\right)}\rightleftharpoons {\mathrm{CO}}_{\left(\mathrm{g}\right)}+{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{g}\right)},$ if the initial concentration of $\left[{\mathrm{H}}_2\right]=\left[{\mathrm{CO}}_2\right] = 1\mathrm{M}$ and $\mathrm{x}$ moles$/\mathrm{L}$ of ${\mathrm{H}}_2$ is consumed at equilibrium, the correct expression of ${\mathrm{K}}_{\mathrm{P}}$ is.

Which of the following statements is correct?

Among the following points indicated on the graph, which one represents equilibrium?