Keq

Question 1

Rules of Keq:

Answer 1

~Keq>1- more products than reactants at equilibrium(products favoured)
~Keq<1- more reactants than products at equilibrium(reactants favoured)
~Keq=1- [reactants]=[products]
~Keq has no units
~Keq value only changes with temp.

Question 2

Keq represents:

Answer 2

Position of equilibrium

Question 3

What doesn’t Keq use:

Answer 3

Liquids and solids

Question 4

Keq does use:

Answer 4

Aqueous and gas

Question 5

Keq doesn’t depend on:

Answer 5

Concentration

Catalysts

Question 6

Keq is dependent on:

Answer 6

Temp. Only

Question 7

Keq formula:

Answer 7

[products]
__________ each is raised to the number of
[reactants] moles(power of)

Question 8

Steps to figuring out Keq: step1
Ex. A mixture of 5.000x10-3 mol H2 & 1.000x10-2 mol I2 fills a 5L container at 448’c
Equilibrium mixture shows that the concentration of HI is 1.87x10-3 M. Calculate Keq.
H2(g) + I2(g) 2HI(g)

Answer 8

1: calculate known initial and equilibrium concentration of all species involved in the equilibrium
a) H2. b) 1.0x10-2/5L=2.0 x10-3 M
M= mol
—–
L
5.0x10-3 mol
—————-= 1.0x10-3
5 L

Question 9

Step2:

Answer 9

Calculate /\H=[HI final]-[HI initial]
@eq’m @start
/{HI}= 1.87x10-3

Question 10

Step 3: find change in concentration of all of other species

Answer 10

#mols of known concentration at eq'm
----------------------------------------------
Change of conc. of known 
=#mols of unknown at eq'm
---------------------------------
Change in conc. of unknown(x)

Question 11

Step 4:

Answer 11

a)H2=[initial]+[change]
=1.0x10-3 +(-9.35x10-4)
{H2}=6.5x10-5 M
b)I2=[initial]+[change]
=2x10-3+(-9.35x10-4)= 1.07x10-3 M

Question 12

Step 5:

Answer 12

Calculate Keq:
P
--
R
Keq=(1.87x10-3)2
         ---------------
      (6.5x10-5)(1.07x10-3)
Keq= 50.3(products favoured)