Continuation from previous task:

Use le Chatelier's principle to determine what happens to the following equilibrium of the given changes under

When some hydrogen gas is removed, the equilibrium will be shifted towards

When something C(s) is added, the equilibrium will be shifted towards the

When more H2O(g) is added, the equilibrium will be shifted towards

When the pressure increases by reducing the volume (assuming the temperature is kept constant), the equilibrium will be shifted towards the

When the gas mixture cools, the equilibrium will be shifted towards the

When a catalyst is added

C(s) + H2O (9) + CO (9) + H2 (9) C s)+ (g) ) = 131 kJ