Chemical equilibrium and Le Chatelier's principle $$\ce{energy + 2KClO3 (s) &lt;=&gt; 2KCl(s) + 3O2 (g)}$$

The reaction will be more active in the reverse direction if:


$\ce{O_2}$ is added   
more $\ce{KCl}$ salt is added.  
More $\ce{KClO3}$ is added  
Increasing the temperature.


My thoughts:

I think (1) and (2) are both right. But the book states that only (1) works and I can't find reason for that searching google was useless.

$K_c = [\ce{O2}]^3$, so if we increased $\ce{KCl}$ or decreased $\ce{KClO3}$ it won't affect the equilibrium?



$$\ce{Fe(OH)(s) &lt;=&gt; Fe^{2+}  + 2OH^-}$$ The reaction will be more active in the reverse direction if : ... is added


$\ce{KOH}$
$\ce{Na_2S}   $
$\ce{Fe(OH)_2}  $ 
$\ce{Fe(NO3)2}$


Won't it be (1) and (4)? The book says it's (4) only.
1) Increasing Oxygen pressure will increase the reverse rate because to reestablish equilibrium some of the oxygen should be consumed.
2) Out of system due to precipitation.
3) Out of system due to precipitation.
4) This is endothermic reaction. So increasing temperature will increase the forward rate to consume the added heat.