Di-hydrogen gas is obtained from natural gas by partial oxidation with steam as per following endothermic reaction:
$CH_4{_{(g)}}+H_2O_{(g)} \ce{<=>} CO_{(g)}+3H_2{_{(g)}}$
How will the values of $K_p$, $K_c$ and composition of equilibrium mixture be affected by increasing the pressure ?
Now,
1) According to this answer $K_c$ only changes on changing temperature i.e. unaffected by pressure.
2) According to Wikipedia the article "Pressure dependence" says, "...However, the composition at equilibrium will depend appreciably on pressure when:
1)the pressure is changed by compression or expansion of the gaseous reacting system, and
2)the reaction results in the change of the number of moles of gas in the system....."
here wiki is using term $K_p$ to denote equilibrium constant. Now the "composition of equilibrium" means $K_p$ and not $Q_p$ because its taking at equilibrium, so the $K_p$ changes with pressure.
3) I have studied that on increasing pressure the reaction shifts the side with less number of sum of gaseous atoms in the reaction formulae. I know from this question that composition of equilibrium is different from "the side at which the reaction shifts". So it seems my study isn't useful here in deciding the composition of equilibrium
So my question is how will the values of $K_p$, $K_c$ and composition of equilibrium mixture be affected by increasing the pressure ? Does one change and the other remains unaffected and isn't the composition of equilibrium directly related to $K_p$ and $K_c$
Are dependencies of $K_p$ and $K_c$ different for change in pressure.