State Le Chatelier's Principle.

Dihydrogen gas is obtained from natural gas by partial oxidation with steam as per the following endothermic reaction:
$CH_{4(g)} + H_2O_{(g)} \rightleftharpoons CO_{(g)} + 3H_{2(g)}$
$(a)$ Write an expression for $K_p$ for the above reaction.
$(b)$ How will the values of $K_p$ and the composition of the equilibrium mixture be affected by:
$(i)$ increasing the pressure
$(ii)$ increasing the temperature
$(iii)$ using a catalyst?

The equilibrium constant $K$ and reaction quotient $Q$ are in the ratio $K : Q = 0.33 : 1$. This means that:

For the reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$,$\Delta H^o = -198 \, kJ$. According to Le Chatelier's principle,the favorable conditions for the forward reaction are:

In which of the following reactions will the amount of products not increase upon increasing the pressure?

The supply of oxygen to tissues by blood can be explained by: