For the process $\mathrm{A}\left(\mathrm{g}\right)+3\mathrm{B}\left(\mathrm{g}\right)\stackrel{ }{\rightleftharpoons }2\mathrm{C}\left(\mathrm{g}\right)$ at 750 K the value of equilibrium constant is  ${10}^2$. At 450K the value of equilibrium constant for the same reaction is $5\times {10}^2.$ Correct statement about the process is  

Addition or removal of gaseous  reactant or product always influences the equilibrium state .

$∆{\mathrm{n}}_{\mathrm{g}}< 0......$ high pressure favours forward reaction .

When temperature increases, ${\mathrm{K}}_{\mathrm{eq}}$ decreases for an exothermic reactions .