Equilibrium
Presentation
•
Chemistry
•
10th - 12th Grade
•
Practice Problem
•
Hard
Anthony Cooper-Percival
Used 42+ times
FREE Resource
6 Slides • 12 Questions
1
Equilibrium
Do you understand the concepts?
2
Multiple Select
Which of these are features of a Dynamic Equilibrium?
has to be in a closed system
The rate of the forward and reverse reactions are the same
the concentrations of the reactants and products are the same
the concentrations of the reactants and products remain constant
3
Fill in the Blanks
Type answer...
4
5
Multiple Select
2SO2 (g) + O2 (g) ↔ 2SO3 (g)
If concentration of SO2 is increased, equilibrium will shift...
Left
Right
stay the same
6
Multiple Select
2SO2 (g) + O2 (g) ↔ 2SO3(g) ΔH = −197 kJmol−1
If the temperature is increased, the equilibrium will shift ...
left
right
stay the same
7
Multiple Select
2SO2 (g) + O2 (g) ↔ 2SO3 (g)
If a catalyst is added, the equilibrium will shift...
left
right
stay the same
8
Multiple Select
2SO2 (g) + O2 (g) ↔ 2SO3 (g)
If the pressure is increased, equilibrium will shift ...
left
right
stay the same
9
10
Multiple Select
N2(g) + 3H2 (g) ↔ 2NH3 (g) ΔH =−92kJmol−1
Select the conditions that would favour the formation of a large amount of product
High Temperature
Low temperature
High pressure
Low pressure
11
Open Ended
Explain why low temperature and high pressure are the best conditions to produce maximum yield of ammonia
12
The haber process
N2(g)+3H2(g)↔2NH3(g)ΔH=−92kJmol−1
Low temperatures push eqm right because the reaction is exothermic in the forward direction.
High pressure pushes eqm right because there are fewer moles of gas on the right.
13
Multiple Select
What conditions are actually used for the haber process?
High Temperature
Low temperature
High Pressure
Low pressure
14
Open Ended
Why is a high temperature and pressure used for the haber process?
15
Compromise conditions are used for the Haber process
High temperatures will lower the yield of ammonia being made but will increase the rate of reaction
High pressures force eqm to the right, but not too high that it is too costly in terms of energy or specialist equipment.
An iron catalyst is used to further increase reaction rate and reduce energy costs.
16
The Equilibrium Constant Kc
The value of Kc is an indication of the position of equilibrium
If Kc = 1, the position of eqm lies in halfway between the reactants and products
if Kc > 1, eqm lies to the right/products
if Kc < 1, eqm lies to the left/reactants
The greater the value of Kc, the further to the right the position of eqm lies.
17
Multiple Choice
Which of these would be the correct expression of Kc for the Haber process?
Kc = [N2][H2]3[NH3]2
Kc = [N2]3[H2]2[NH3]
18
Fill in the Blanks
Type answer...
Equilibrium
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