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  

• A

  Addition of ‘A’ has no effect on equilibrium state

• B

  Removal of ‘C’ has no effect on equilibrium state

• C

  Pressure has no effect on equilibrium state

• D

  Formation of ‘C’ is an exothermic process