Question about change in pressure and change in temperature for system at equilibrium
For a general idea, see Le Chatelier's principle


  When any system at equilibrium for a long period of time is subjected to change in concentration, temperature, volume, or pressure,
  (1) the system changes to a new equilibrium and 
  (2) this change partly counteracts the applied change.




For the changes of $p, V$, read about equilibrium constant $K$ and Reaction quotient $Q$ and their relation.

Notice, how the Reaction quotient changes with increased pressure/decreased volume, if the reaction increases the molar amount of gases.
And how it changes if it decreases them.

For the former case, increasing pressure increases Q and the equilibrium shifts backwards to make Q  equal to K again.

For the latter case, increasing pressure decreases Q and the equilibrium shifts forwards to make Q equal to K again.



For the temperature effect, see van't Hoff equation:


  $$\frac{d}{dT} \ln K_\mathrm{eq} = \frac{\Delta H^\ominus}{RT^2}$$


Endothermic reaction direction has higher activation energy than the exothermic direction.

As the consequence,

the reaction rate of the endothermic reaction direction

raises with temperature faster

than the reaction rate of the exothermic reaction direction.

Faster endothermic then exothermic reaction means the equilibrium constant shifts at higher temperature in favour of the endothermic reaction.