For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,in which direction will the equilibrium shift if an inert gas is added at constant pressure?

Formation of $SO_3$ takes place according to the reaction:
$2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g); \,\, \Delta H = -45.2 \, kcal$
Which of the following factors favours the formation of $SO_3$?

For the reaction,$A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)} + D_{(g)}$; $\Delta H = Q \ kJ$,the equilibrium constant cannot be disturbed by

The standard state Gibbs free energy change for the given isomerization reaction $cis-2-pentene \rightleftharpoons trans-2-pentene$ is $-3.67 \ kJ/mol$ at $400 \ K$. If more $trans-2-pentene$ is added to the reaction vessel,then:

The equilibrium $SO_2Cl_{2(g)} \rightleftharpoons SO_{2(g)} + Cl_{2(g)}$ is attained in a closed vessel at $25 \, ^\circ C$. If an inert gas,$He$,is added at constant volume,which of the following statement$(s)$ is/are correct?

For the formation of $NH_{3(g)}$ from its constituent elements,the favourable conditions for its formation are