Question

2. Based on the K, will there be more product or reactant when the following reactions reach equilibrium? HCN(aq) -→ H++CN. a. Ke 6 10 2.2 1025 Keq 1.4*104 c. Al(OH)3(s) AI+3+ 3 OH. +_+ 3. For the reaction at equilibrium: Pb+2 + 2 cr ←→ PbClas) Which direction (forward or reverse) would the reaction shift if: c. Product removed?- b. Chloride ion added? a. Lead ion removed?

Answer 1

2)

Keq = [ products] / [ reactants]

If Keq > 1 , higher amount of [products] than [reactants] , that is reaction favors products

If Keq < 1,  higher amount of [reactants] than [products] , that is reaction favors reactants

a) HCN (aq) <----> H+ (aq) + CN- (aq) Keq < 1 , so reaction favors reactants side.

b) 2 K(s) + 2 H2O (l) <----> 2 KOH (aq) + H2 (g) Keq >1 so reaction favors products side.

c) Al(OH)3 (s) <-----> Al3+ + 3 OH- Keq < 1 , so reaction favors reactants side.

3) According to Lechatlier principle

for an equilibrium reaction addition of reactant or removal of product will shift the reaction to products side

and addition of products or removal of reactants will shift the reaction to reactants side.

Pb2+ + 2 Cl- <----> PbCl2

a) Pb2+ removed ? reverse

b) Cl- added ? forward

c) product removed? forward