Answer
(a) Shift to the left.
(b) Shift to the left.
(c) Remaing Unchanged.
(d) Remain Unchanged.
(e) Shift to the right.
(f) Remain Unchanged.
Work Step by Step
(a) Decreasing the concentration of a reactant shifts the equilibrium to the left.
(b) For a gas, increasing its partial pressure means increasing concentration. Increasing the concentration of a product shifts the equilibrium to the left.
(c) $C_6H_{12}O_6$ is a solid, so its concentration will not affect the equilibrium.
(d) The amount of moles of gases is equal in both sides, so the pressure does not affect the equilibrium.
(e) The reaction is endothermic, therefore, increasing the temperature shifts the equilibrium to the right.
(f) Catalysts do not affect equilibrium.
