Question

(show work)

1) Given: CS2 (g) + 3 Cl2 (g) < = > CCl4 (g) + S2Cl2 (g) ΔH = – 238 kJ (5 pts)

Using arrows, predict which way the equilibrium will shift (“---->” to products,

“<----“ to reactants, or “no change”) AND what will happen to the value of Keq (“increase”, “decrease”, or “stays same”), Given the following perturbations:

DIRECTION OF SHIFT Value of Keq

a) A halving of the volume________________________________ ____________

b) Adding Ne gas to the vessel___________________________ ____________

c) Removing some CCl4___________________________________ ____________

d) Lowering the temperature____________________________ ____________

e) Adding some S2Cl2______________________________________ ____________

Answer 1

these all are the applications of LE CHATELIER'S PRINCIPLE-

A) as there are four moles in reactants side and two moles in product side so acc to LE CHATELIER'S PRINCIPLE, decrease in volume will shift the equilibrium ti that side in which number of moles decreases that means forward direction.(----->) AND value of keq will increase.

B) as reaction is taking place in closed vessel so there will be no effect of addition of inert gas (Ne) to closed vessel as it won't chamge concentration of reactants and products and no change in Keq

C) on removal of CCl4 the concentration of products will decrease so the equilibrium will shift in the forward direction(------>) and value of Keq increases

D) as the reaction is exothermic in nature so lowering the temperature will shift the equilibrium in forward direction acc to le chatlier principle and equilibrium will shift in forward direction (------->) and value of Keq will increase

E) on addition of S2Cl2 in product side the reaction will tend to shift in backward direction as product concentration increaszes and reactant will decreases. and direction of equilibrium(------<) and value of Keq decreases.