help plz

What would happen to the position of the equilibrium when the following changes are made to the equilibrium system below? 2503(g) | 2502(g) + O2(g) Adding sulfur dioxide causes the system to shift to the Adding sulfur trioxide causes the system to shift to the Adding oxygen causes the system to shift to the + 2HgO(s) = Hg(0) + O2(g) Adding mercury oxide causes the system to shift to the Increasing the pressure will cause the system to shift to the 4HCl(g) + O2(g) + 2H2O(g) + 2Cl2(g) Increasing the volume of gas will cause the system to shift to the Please answer all parts of the question. Predict the effect of decreasing the volume of the container for each equilibrium. 2H2O(g) + N2(g) = 2H2(g) + 2NO(g) Shifts to produce SiOz(s) + 4HF(g) = SiF4(g) + 2H2O(g) Shifts to produce CO(g) + H2(g) = C(s) + H2O(g) Shifts to produce