It depends on type of reaction_
∆n>0 Increase in pressure shifts reaction in reactant sides.
∆N<0 Increase in Pressure shifts reaction in product side.
∆n=0 no effect.
Example ∆n= sum of coefficient of gaseous products--- sum of coefficient of gaseous reactant
- 1) H2 +I2 => 2HI ∆n=0
- 2)PCL3 +Cl2 => PCl5 ∆n<0
- 3)A2=> 2A ∆n>0
Temperature if it is endothermic then Increase in Temperature shifts reaction in Product side
and vice-versa.
If it is exothermic then increase in temperature shifts reaction towards reactant side.
On concentration if there is increase in concentration then reaction takes place in a direction in which it consume the increase in concentration.
Ps- Equilibrium constant means(K) changeg with change in temperature only.
It doesn't depends on concentration and pressure etc.
Hope that helps you :)
ty for those thanks star <3 can I call u shine..?