For the reaction $A_{2(g)} + B_{2(g)} \rightleftharpoons 2AB_{(g)}$; $\Delta H = +ve$,which of the following statements is correct regarding the effect of pressure?

$aA \rightleftharpoons mB + nC$,$\Delta H = + x \ kcal$. If $m + n < a$,then conditions favouring forward reaction will be

The formation of nitric oxide by the reaction $N_2 + O_2 \rightleftharpoons 2NO$ with $\Delta H = +43.200 \ kcal$ is favoured by:

In which of the following gaseous equilibrium will an increase in pressure increase the yield of the products?

Consider the equilibrium $CO_{(g)} + 3H_{2(g)} \rightleftharpoons CH_{4(g)} + H_2O_{(g)}$. If the pressure applied over the system increases by two-fold at constant temperature,then which of the following statements are correct?
$(A)$ Concentration of reactants and products increases.
$(B)$ Equilibrium will shift in the forward direction.
$(C)$ Equilibrium constant increases since the concentration of products increases.
$(D)$ Equilibrium constant remains unchanged as the concentration of reactants and products remain the same.
Choose the correct answer from the options given below:

Consider the heterogeneous equilibrium in a closed container:
$NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$
If more $NH_4HS_{(s)}$ is added to the equilibrium,what will be the effect on the system?