Question

Equilibrium - Investigation of Le Chatelier's Principle Pre-Lab Questions 1) Each of the components of the HC2H2O2 equilibrium system in Part A are clear and colorless. a) Briefly explain how you will determine the effects of the additions you make to this equilibrium b) What will you expect to observe if the H2O concentration is relatively high? c) What will you expect to observe if the H2O* concentration is relatively low?

Answer 1

2) List 3 ways we can distarb a chemical system at equilibrium in a laboratory 1) Concentration of either reactants or produits changing B) change in volume of the reaction mixture prevure change. o) change in Temperature of the reaction mixture ^2(0)+ 3 H₂(g) 2 NH3(g) a) chemical equations for the forward reaction Rate = rf [~2] [42]² Chemical equation * (g) + 3 h (3) → 2NH3 (9) 6) Chemical equation for reverse reaction. 2NH₃(g) N2(g) + 3 H₂G) c) Definition of equilibrium ; at is defined as the state of reaction at which where the rate of forward reaction is equal to the rate of backward reaction, HGH₂02 H2O Shoot + to a) change in concentration of either reactant or product will change the equilibrium in either forward or backward direction. b) on increasing dilution, the dissociation of and increases and produces more H₂o ions.(ar) increasing the more amount of and. . c) by adding strong aud, will decreases the dissociation of weak and there by decreases the concentration of the ins