Dynamic Equilibrium
ICE Tables
Bronsted-Lowry & Arrhenius
Le Chatelier's Principle
100
Name three stressors that can be applied to an equilibrium system
1) Temperature
2) Concentration
3) Pressure/Volume
100
What does ICE stand for?
Initial, Change, Equilibrium
100
What is the Bronsted-Lowry definition of an acid and a base?
Acid: proton donor
Base proton acceptor
100
True or false: According to Le Chatelier's Principle, when a stressor is applied to a a system at equilibrium, the system will shift to oppose the change until a new equilibrium is established.
True
200
the Kc value if products are favorable
what is greater than 1?
200
why do we use ICE tables for?
going from initial concentration to equilibrium concentrations
200
Identify the bases in the following chemical equation
HSO4- (aq) + HPO42- (aq) <--> H2PO4- (aq) + SO42- (aq)
HPO42-
SO42-
200
If the concentration of HF(g) increased, which direction would the equilibrium shift and would this produce more or less product?
CCl4(l) + 2HF(g) <--> CCl2F2(g) + 2HCl(g)
Equilibrium would shift right and more product would be produced
300
Write the Equilibrium Law expression for the following equation
Zn(s)+Cu2+(aq)↔Cu(s)+Zn2+(aq)
Kc = Zn2+(aq) / Cu2+(aq)
300
Consider the reaction for the decomposition of hydrogen iodine at 448°C. The initial concentration of HI(g) was 1.00mmol/L. Once an equilibrium was established, the concentration of HI(g) was measured to be 0.078mmol/L. Calculate the equilibrium constant (Kc)
2HI(g) < --> H2(g) + I2(g)
2.7
300
The product/s of this reaction
O2-(aq) + H2O(l) ⇄
What is 2OH- ?
300
If the pressure of this system increased, which direction would the equilibrium shift?
2SO2(g) + O2(g) <--> 2 SO3(g)
right
400
In the following system: N2(g) + 3H2(g) ↔ 2NH3(g)
0.249 mol/L of N2(g), 3.21 X 10-2 mol/L of H2(g) and 6.42 X 10-4 mol/L of NH3(g) are combined in a 1.00 L vessel at 375°C.
What is the Kc value for the reaction and are the products or reactants favored?
what is 0.0500 ?
what is Reactants ?
400
If a 100 mL sample of 0.344 mol/L unknown acid has a pH of 4.1 at 30 degrees, then the Ka is?
Ka = 1.8 x 10^-8
400
Identify the conjugate acid base pairs from the following reaction
HCO3- (aq) + CN- (aq) < -- > CO32- (aq) + HCN (aq)
1. HCO3-(aq) & CO32-(aq)
2. CN-(aq) & HCN(aq)
400
If the volume of this system decreased, which direction would the equilibrium shift?
H2(g) + Cl2(g) < -- > 2HCl(g)
The equilibrium would not shift
500
what is C ?
500
A student measures the pH of a 0.25 mol/L solution of carbonic acid to be 3.48. Calculate the Ka for carbonic acid from this evidence
Ka = 4.39x10^-7
500
What will be the predominant reaction if nitric acid is mixed with potassium fluoride
H3O+(aq) + F-(aq) --> H2O(l) + HF(aq)
500
2NO + Cl2 <--> 2NOCl + Heat
temp up, Concentration Of NOCl up, Concentration of Cl2 down