For a gaseous reaction : ${\text{A}}_{\left(\text{g}\right)}\rightleftharpoons {\text{\hspace{0.17em}3B}}_{\left(\text{g}\right)}{\text{\hspace{0.17em}+\hspace{0.17em}C}}_{\left(\text{g}\right)}\text{,\hspace{0.17em}ΔH}$ is positive and the reaction attains equilibrium at

1 bar total pressure and 400K. Identify the incorrect statements regarding the above reaction.

$\Delta G°=0$ for the above reaction at equilibrium

On increase of temperature, equilibrium will be shifted in forward direction 

When inert gas is introduced into a rigid container containing above equilibria equilibrium

 shifts towards left         

If volume of vessel containing the above equilibria is increased without change in temperature

then partial pressure of B decreases as compared to original equilibrium partial pressure of B.