Question

Assuming that each of the following reversible reactions has reached a state of equilibrium, indicate with an arrow, showing direction of shift, the effect of each change upon the equilibrium. Assume that only one change is made at a time.

a) 2 Cl2(g) + 2 H2O(g) + heat  4 HCl(g) + O2(g) (1) Raise P (2)Raise T

b) Fe2O3(s) + 3 H2(g)  3 H2O(g) + 2 Fe(s) (1) Add Fe(s) (2) Raise P

c) 2 NH3(g) + heat  N2(g) + 3 H2(g) (1) Raise T (2) Lower P

d) CO(g) + H2O(g)  CO2(g) + H2(g) + heat (1) Lower T (2) Raise P

e) 2 SO2(g) + O2(g)  2 SO3(g) + heat (1) Raise T (2) Lower P

Answer 1

(a) Increase in pressure will shift the reaction to the reverse side. Increase in temperature will shift the reaction in the forward side.

(b) Adding Fe(s) will shift the reaction towards reverse direction. Increase in pressure has no effect.

(c) Increase in temperature will shift the reaction towards forward direction.Lowering the pressure will shift the equilibrium towards reverse direction.

(d) Lowering the temperature will shift the reaction in the forwards direction.In crease in pressure will have no eefect and the reaction will be in the forwarrds direction.

(e) Increase in temperature will shift the equilibrium in the reverse direction. Lowering the pressure will shift the equilibrium towards forward direction.