Chemistry Unit #7: Kinetics and Equilibrium .... Test on April 5, 2017 Flashcards
(196 cards)
1
Q
What is the chemical equation of the ignition of nitroglycerin?
A
C₃H₅N₃O₉(l) ===> 12CO₂(g) + 10H₂O(g) + O₂(g) + 6N₂(g) + energy
2
Q
Meaning of Q’s value
A
- if Kc > Q: forward rxn favored - vice versa
3
Q
Write the equilibrium constant expressions for the following reactions at equilibrium. C) C₂H₅OH(l) + CH₃COOH(l) ⇌ CH₃COOC₂H₅(l) + H₂O(l)
A
Kc = [CH₃COOC₂H₅] [H₂O] / [C₂H₅OH] [CH₃COOH]
4
Q
Reversible reactions do not reach an ____. 3
A
End Never go to completion Final observation in not 100% of product
5
Q
A catalyst increases the rate of forward and reverse reactions equally.
A
A catalyst increases the rate of forward and reverse reactions _______.
6
Q
What is a device that can be used to measure the amount of light absorbed at a particular wavelength — the darker the colour of the sample, the more light is absorbed
A
A colorimeter
7
Q
Write the equilibrium constant expressions for the following reactions at equilibrium. A.) 2NH₃(g) + H₂SO₄(g) ⇌ (NH₄)₂SO₄(g)
A
Kc = [(NH₄)₂SO₄] / [NH₃]² [H₂SO₄]
8
Q
What does Kc mean?
A
Equilibrium constant at a particular temperature
9
Q
What does Nitrogen Fixation naturally? 3
A
Bacteria do this naturally Good for plants Because it is needed for growth (fertilizer)
10
Q
Was nitroglycerin, C₃H₅N₃O₉(l) dangerous to handle on its own?
A
Yes, it was
11
Q
State the four factors that affect the reaction rate and one that only affects if particle are gases.
A
Break up solid reactants to increase the Surface area Increase Concentration or Shrink container Increasing the Temperature Adding/Using a Catalyst Increase the number of particles or increase pressure
12
Q
Slope in a graph _______ as reactant as used up.
A
Decreases
13
Q
For the following equilibrium constants, predict which would exist in higher quantities — reactants or products. D) 1.00
A
Neither reactants or products
14
Q
What three main things happen when the Reverse reaction is favoured?
A
Reaction shifts towards the left side More reactants form Amount of products reduced
15
Q
Reaction rate is the ______ of the reaction
A
Speed
16
Q
For an endothermic reaction, the value of the equilibrium constant _________ as the temperature is increased. Why?
A
For an endothermic reaction, the value of the equilibrium constant increases as the temperature is increased.
Endothermic’s process is A + B + heat = C + D
We treat heat a reactant and because we have more reactants, we make more products, thus shifting the equilibrium to the right/forward
17
Q
What happens to the Chemicals during Dynamic Equilibrium?
A
Chemicals shift between reactant side and product side
18
Q
Is Equilibrium limited to chemical reactions?
A
No, it is not limited to chemical reactions
19
Q
State two general ways, according to the collision theory, the reaction rate could be increased.
A
1) Increase the frequency of collisions (If Obinna’s chance of success is 1%, he will get 1 date from asking 100 women. He can increase his chances by asking 1000 women, with which he will get 10 dates.) 2) Increase the energy with which they collide in a certain time. (Get more Attractive)
20
Q
State the only factor that when changed will alter the equilibrium constant. Kc
A
Temperature
21
Q
Given: C₂H₅OH(l) + CH₃COOH(l) ⇌ CH₃COOC₂H₅(l) + H₂O(l) In which direction will the equilibrium shift if: B) more alcohol is added
A
Stress: Favoured: Direction: right/forward
22
Q
How is O₂(g) obtained for the Contact Process reaction of 2SO₂(g) + O₂(g) ⇌ 2SO₃(g) ∆H°= -197 kJ/mol??
A
From fractional distillation of liquid (compressed) air
23
Q
In reversible reactions, sometimes products will collide and lead to the reforming of ________
A
In reversible reactions, sometimes products will collide and lead to the reforming of reactants
24
Q
How does Nitrogen Fixation happen?
A
Changing N₂(g) to a nitrogen compound
25
State two way the rate of a reaction may be defined.
-Increase of concentration of products per unit time -Decrease of concentration of products per unit time
26
What is the yield rate of the Contact Process under the 3 conditions for the optimum yield of sulfuric acid, H₂SO₄(aq)?
99%
27
Why must a fire in a fireplace be started with paper and kindling instead of lighting the logs directly?
A match does not put out enough energy to get a log up to the temperature where it will burn. It's easiest to start the fire with something that is easier to light; something thin that has a lot of surface area to react with oxygen and cannot conduct the heat of the match away quickly enough to prevent it from reaching combustion temperature.
28
What is the main reaction of sulfuric acid? (before mixed with water)?
2SO₂(g) + O₂(g) ⇌ 2SO₃(g) ∆H°= -197 kJ/mol
29
What is a collision called when it results in a reaction?
Successful Or Effective
30
Define the term "Homogenous reaction".
A reaction in which all reactants and products are in same phase.
31
Define Dynamic Equilibrium 3 + example
- Reverse reaction and forward reaction occur simultaneously - the rate of forward reaction is equal to the rate of the reverse reaction - concentrations of reactants and products remains constant Macroscopic properties are constant (concentrations of all reactants and products remains constant) the rate of forward reaction is equal to the rate of the reverse reaction Chemicals shift between reactant side and product side Example: walking up an escalator moving down, still moving but no progress made Exam tip: When asked to define dynamic equilibrium you must address both the "dynamic" and the "equilibrium" part.
32
What are the requirements to form a dynamic equilibrium? 1 + 4 points on example
Reaction must be reversible and form a closed system --- No matter and energy can leave Material (& energy) can neither enter nor leave the container Example: Consider a reversible reaction that forms a gaseous product If the gaseous product escapes to the air, equilibrium cannot be reached Because products will not collide with each other to form the reactants in a certain time. By putting a lid to contain the gas formed, reverse reaction will occur
33
Describe what is "equal" in a chemical reaction at "equilibrium".
It refers to the rate of forward and reverse reactions.
34
difference between Kc and Q
Kc: describes rxn at equilibrium Q: describes rxn not at equilibrium
35
If K is a large number, it means that the equilibrium concentration of the reactants is \_\_\_\_\_\_\_. In this case, the reaction as written will proceed to the \_\_\_\_\_\_\_
If K is a large number, it means that the equilibrium concentration of the reactants is small. In this case, the reaction as written will proceed to the left (resulting in an decrease in the concentration of products)
36
Where can Equilibrium also exist, besides chemical reactions? 1 + 5 points on Example
physical equilibrium Equilibrium also exists in physical changes Example: Equilibrium between condensation rate & evaporation rate in a closed bottle An exchange of state with water between liquid and vapour Written as H₂O(l) ⇌ H₂O(g) Liquid water is "in equilibrium with" gaseous" gaseous water Water will not completely evaporate if bottle is kept sealed
37
What was the energy put out by the main chemical reaction of the Haber Process?
N₂(g) + 3H₂(g) ===\> 2NH₃(g) ∆H°= -92 kJ/mol
38
State how changing the Surface area of solid reactants as one of the four factors that affect the reaction rate and provide: A) an explanation why it causes the rate to increase and B) an example of each 6
Reactions generally only occur at the surface of a solid. Making a solid more finely divided increases the surface area and therefore the number of particles exposed at the surface. The effective concentration of the particles of the solid has thus been increased and there is a greater chance of a particle of the other reactant colliding with a particle on the surface and reaction occurring. Powdered reactants react faster When there is a low surface area, only the particles on the outside are exposed on the surface and able to collide with the particles in a certain time. When there is a high surface area, all the particles are exposed and are able to collide with the particles in a certain time. Example: Dissolving sugar cubes vs sugar grains Melting ice cube vs. ice chips
39
Where are Catalysts written above?
written above the yield arrow
40
State the conditions needed for the optimum yield of ammonia in the Haber process. Justify why these conditions are used. 4
1) High concentrations of N₂(g) and H₂(g) ➽ The ratio is always maintained at a ratio of 1:3 to make sure there is no limiting reactant and effective collisions are increased. 2) Use of catalyst - heated powdered iron oxide ➽ Heated powdered iron oxide is used because being powdered increases surface area for the reaction and being heated means that particles have more energy and collide harder, thus making sure there are a lot of effective collisions in a certain time. 3) Removal of Ammonia ➽ This drives equilibrium forward. 4) Ideal temperature is 450°C ➽ This ideal temperature is balances between high equilibrium yield and a faster reaction rate.
41
How do you find the average rate of a reaction from looking at a graph?
Average Rate = (change in volume/mass/concentration) / (time)
42
Reversible reaction form an equilibrium \_\_\_\_\_\_
System
43
Given: 2NO(g) + O₂(g) ⇌ 2NO₂(g) ∆H°= -2.7 kJ/mol What will happen to the concentration of NO₂(g) for each of the following. A) adding more NO(g)
Stress: Favoured: concentration of NO₂(g) goes up
44
Given: 2NO(g) + O₂(g) ⇌ 2NO₂(g) ∆H°= -2.7 kJ/mol What will happen to the concentration of NO₂(g) for each of the following. B) temperature is increased
Stress: Favoured: concentration of NO₂(g) goes down
45
What is the kJ/mol energy of the triple bond of a molecule of nitrogen?
A strong triple bond (941 kJ/mol)
46
Catalysts do not appear as a ________ or \_\_\_\_\_\_\_\_\_
Catalysts do not appear as a reactant or product May be written above the yield arrow
47
State the conditions needed for the optimum yield of sulfuric acid in the Contact process. Justify why these conditions are used. 3
1) High pressure - 3 moles of gas forming two moles of gas …………………………- 2 atm used ↠ The production of H₂SO₄(aq) requires the reaction of 2SO₂(g) + O₂(g) ⇌ 2SO₃(g). Where SO₂(g) is obtained from burning sulfur or sulfide ores and O₂ is obtained from fractional distillation of liquid (compressed) air. Using high pressure shifts the reaction to the right, making more SO₃(g). SO₃(g) is then added with water to finally make H₂SO₄(aq). 2) Ideal temperature is 450°C ↠ 450°C is an ideal high temperature that favours the reverse reaction, which increase the reaction rate. 3) Adding vandaium (V) oxide as a catalyst ↠ Adding the catalyst increases rate without affecting equilibrium. ⇝ The yield rate at these conditions is 99%. Using a higher pressure would be uneconomical
48
situation where Kc won't apply
non-reversible rxns
49
Given: CO₂(g) + H₂(g) ⇌ CO(g) + H₂O(g) ∆H°= +41 kJ/mol In which direction will the equilibrium be shifted by each of the following changes? E) temperature is increased
Stress: Favoured: Direction: right/forward
50
A second order reaction will increase _______ 2
A second order reaction will increase non-linearly (quadruple) Increasing in a curve line
51
Given: CO₂(g) + H₂(g) ⇌ CO(g) + H₂O(g) ∆H°= +41 kJ/mol In which direction will the equilibrium be shifted by each of the following changes? D) increasing the pressure
Stress: Favoured: Direction: no effect
52
Given: 2NO(g) + O₂(g) ⇌ 2NO₂(g) ∆H°= -2.7 kJ/mol What will happen to the concentration of NO₂(g) for each of the following. C) increasing the pressure
Stress: Favoured: concentration of NO₂(g) goes up
53
Bond making releases or absorbs energy?
Bond making releases energy
54
Where is the activated complex or transition state found on an enthalpy level diagram?
It is found in the highest point along the curve
55
State how changing the Concentration as one of the four factors that affect the reaction rate and provide: A) an explanation why it causes the rate to increase and B) an example of each 3
With more particles in a certain volume, the particles collide more often (the collision frequency is higher) and therefore there is greater chance of a successful collision occurring in a certain time. When there is a lower concentration, the particles are further apart and collide less frequently in a certain time. When there is a higher concentration, the particles are closer together and collide more frequently in a certain time.
56
In reversible reactions, what is each collision forming a transition state called?
In reversible reactions, what is each collision forming a transition state called an Activated Complex
57
Given: 2NO(g) + O₂(g) ⇌ 2NO₂(g) ∆H°= -2.7 kJ/mol What will happen to the concentration of NO₂(g) for each of the following. F) lowering the temperature
Stress: Favoured: concentration of NO₂(g) goes up
58
For the reaction of wA + xB ⇌ yC + zD, what are the significance of the letters, w, x, y and z?
They are the coefficients
59
If Q \< Kc, then essentially we have ____ \_\_\_\_\_\_ product and the reaction will proceed to the\_\_\_\_\_\_\_
If Q \< Kc, then essentially we have too little product and the reaction will proceed to the right (to produce more product and decrease the concentration of reactant)
60
What was the results of nitroglycerin, C₃H₅N₃O₉(l) exploding? 2
Releases energy as triple bond formed Rapid increase in volume of gases (heat)
61
Consider the reaction: CaCO₃(s) + 2HCI(aq) ===\> CaCl₂(aq) + H₂O(l) + CO₂(g). What are two ways we can graph it against time?
Decrease in concentration of HCI Using a pH meter Increase in volume of CO₂
62
Changing N₂(g) to a nitrogen compound is called what?
Nitrogen Fixation
63
Given: C₂H₅OH(l) + CH₃COOH(l) ⇌ CH₃COOC₂H₅(l) + H₂O(l) In which direction will the equilibrium shift if: D) the ethanoic acid boils away
Stress: Favoured: Direction: left/reverse
64
If too much ammonia is added into the soil of farmer's fields, what develops?
Salts and it will destroy the yield of the farmer's crops
65
What suddenly causes nitroglycerin, C₃H₅N₃O₉(l), to suddenly explode? 2
Being ignited Or Impacted
66
What does Thermodynamics show us? What can't it show us? 2
Thermodynamics shows the energies involved in a reaction. Thermodynamics cannot show how long it takes to go to completion (or if it is ever complete!)
67
What are the characteristics of the reaction when K is larger than 1? 2
If K is larger than 1, the mixture contains mostly products. The reaction goes nearly to completion
68
Q = K No shift in reaction? Reaction will shift to the left? Reactants are greater?
Q = K No shift in reaction
69
What acid is processed from Contact process?
Sulfuric Acid
70
reaction mechanism
sequence of steps in an observable reaction
71
For the following equilibrium constants, predict which would exist in higher quantities --- reactants or products. C) 1.09\*10⁴
Products
72
Rate of reaction tends to ________ as reaction proceeds
Decrease
73
What three main things happen when the Forward reaction is favoured?
Reaction shifts towards the right side More products form Amount of reactants decreases
74
K is less than Q No shift in reaction? Reaction will shift to the left? Reactants are greater?
K is less than Q Reaction will shift to the left
75
State the conditions needed for the optimum yield of ammonia in the Haber process. Justify why these conditions are used. 4
1) High concentrations of N₂(g) and H₂(g) ➽ The ratio is always maintained at a ratio of 1:3 to make sure there is no limiting reactant and effective collisions are increased. 2) Use of catalyst - heated powdered iron oxide ➽ Heated powdered iron oxide is used because being powdered increases surface area for the reaction and being heated means that particles have more energy and collide harder, thus making sure there are a lot of effective collisions in a certain time. 3) Removal of Ammonia ➽ This drives equilibrium forward. 4) Ideal temperature is 450°C ➽ This ideal temperature is balances between high equilibrium yield and a faster reaction rate
76
The rate of reaction is the ____ as the slope of the curve at any moment
Same
77
For the reaction of wA + xB ⇌ yC + zD, how can concentrations of the reactants and products be shown? 2
By putting a square bracket around the particles [A], [B], [C] & [D]
78
To make Ammonia, where did Fritz Haber get the hydrogen from? 2
Methane And steam
79
Given: 2NO(g) + O₂(g) ⇌ 2NO₂(g) ∆H°= -2.7 kJ/mol What will happen to the concentration of NO₂(g) for each of the following. E) increasing the volume of the container
Stress: Favoured: concentration of NO₂(g) goes down
80
Define temperature
The average kinetic energy of particles
81
For an exothermic reaction, the value of the equilibrium constant _________ as the temperature is increased. Why?
For an exothermic reaction, the value of the equilibrium constant decreases as the temperature is increased.
Exothermic's equation is: A + B = C + D + heat
We treat heat as a product and because there is more products, it makes more reactants, thus the equilibrium is shifted to the left/reverse
82
Define molecularity
Molecularity is the number of "molecules" that reacts in a particular step (usually the rate-determining step).
83
Who made handling nitroglycerin, C₃H₅N₃O₉(l), safer? How? What did it result? 3
Alfred Nobel He added the nitroglycerin, C₃H₅N₃O₉(l) to porous silica, which allowed safe handling Dynamite
84
Bond breaking releases or absorbs energy?
Bond breaking absorbs energy
85
What two things do Nitrogen Fixation? 2 and 4 (6)
Bacteria do this naturally Good for plants Because it is needed for growth (fertilizer) Automobile engines do it unintentionally Bad for air Nitrous oxides + water ===\> acid rain
86
Who developed the Haber Process?
Fritz Haber (1868-1934)
87
What element is used that is added with compounds to make explosives?
Nitrogen
88
State how changing the Temperature as one of the four factors that affect the reaction rate and provide: A) an explanation why it causes the rate to increase and B) an example of each 2 (7)
1) More collisions occur as average of kinetic energy More particles travel faster This means that the collision frequency increases, i.e. the particles collide more often. Not only do they collide more often, but they also collide harder in a certain time. 2) More collisions have energy larger than activation energy Each particle likely has more energy Small increase in temperature greatly increases number of particles above the threshold energy A 10K increase will roughly double the reaction rate Increasing the temperature has a major effect on the rate of the reaction. As the temperature increases, the rate of reaction increases exponentially. It is often said that as a rough rule of thumb, a rise in temperature of 10K causes the reaction rate to be approximately doubled. As the temperature increases, the molecules have more energy and therefore move faster. This means that the collision frequency increases, i.e. the particles collide more often. Not only do they collide more often, but they also collide harder, that is with more energy, so there is greater chance that a collision will result in a reaction in a certain time.
89
For the Equilibrium law of Kc = [C]ʸ [D]ᶻ / [A]ʷ [B]ˣ, what letters are the products and what letters are the reactants?
A and B are the Reactants C and D are the Products
90
What was the main chemical reaction of the Haber Process?
N₂(g) + 3H₂(g) ===\> 2NH₃(g) ∆H°= -92 kJ/mol
91
How is H₂SO₄(aq) made? 2
First, reaction of [2SO₂(g) + O₂(g) ⇌ 2SO₃(g) ∆H°= -197 kJ/mol] must happen Then water is added to SO₃(g) to form H₂SO₄(aq)
92
Equilibrium can be attained only in a ______ system.
Equilibrium can be attained only in a closed system.
93
What is the yield rate of the Haber Process under the 4 conditions for the optimum yield
15%
94
Is a molecule of nitrogen, that has a triple bond, reactive or unreactive? Where is it mostly found?
Unreactive, (atmosphere)
95
Given: CO₂(g) + H₂(g) ⇌ CO(g) + H₂O(g) ∆H°= +41 kJ/mol In which direction will the equilibrium be shifted by each of the following changes? F) a suitable catalyst is added
Stress: Favoured: Direction: no effect
96
For the following equilibrium constants, predict which would exist in higher quantities --- reactants or products. A) 1530
Products
97
Write the equilibrium constant expressions for the following reactions at equilibrium. B) 2SO₂(g) + O₂(g) ⇌ 2SO₃(g)
Kc = [SO₃]² / [SO₂]² [O₂]
98
What is the equation that makes acid rain?
nitrous oxides + water ===\> acid rain
99
Who made handling nitroglycerin, C₃H₅N₃O₉(l), safer?
Alfred Nobel
100
Q is less than K No shift in reaction? Reaction will shift to the left? Reactants are greater?
Q is less than K Reactants are greater
101
What happens to the graph of the reactants during Dynamic Equilibrium?
Measurements plateau if graphed
102
Proposed mechanisms are often __________ from experimental reaction rate data.
Proposed mechanisms are often guessed from experimental reaction rate data.
103
Given the following reaction: H₂S(g) + I₂(s) ⇌ 2HI(g) + S(s). The concentrations of 0.5M for H₂S(g) and 0.2 M for HI, what is the value for Kc?
Kc=[HI]²/([H₂S]) Kc=0.2²/0.5 Kc=0.08
104
State the collision theory. Include three conditions that must be met for a reaction to occur.
Collision theory states that a reaction can only occur when: 1) Particles collide 2) Particles collide in the correct orientation 3) Particles collide with or more than a certain minimum amount of activation energy. E ⪰ Ea
105
closed system
- system in which neither matter nor energy is gained or lost from the system - this allows an equilibrium to be reached
106
Given: CO₂(g) + H₂(g) ⇌ CO(g) + H₂O(g) ∆H°= +41 kJ/mol In which direction will the equilibrium be shifted by each of the following changes? C) decreasing the pressure
Stress: Favoured: Direction: no effect
107
Who established the Nobel Peace Prize?
Alfred Nobel
108
For the following equilibrium constants, predict which would exist in higher quantities --- reactants or products. B) 2.34\*10⁻⁵
Reactants
109
Why was ammonia injected into soil of farmer's fields?
To increase the yield of the farmer's crops
110
What is Reaction Rate measured in?
mol dm⁻³ s⁻¹
111
The presence of a _______ does not affect the position of equilibrium or the value of the equilibrium constant; it only reduces the time taken to reach equilibrium.
The presence of a catalyst does not affect the position of equilibrium or the value of the equilibrium constant; it only reduces the time taken to reach equilibrium.
112
During Dynamic Equilibrium, [reactant] doesn't need to equal [\_\_\_\_\_\_\_]
During Dynamic Equilibrium, [reactant] doesn't need to equal [product]
113
What is the overall order from the rate law of: rate = k[A]¹ [B]²
The overall order is third order
114
If K is a large number, it means that the equilibrium concentration of the products is \_\_\_\_\_\_\_. In this case, the reaction as written will proceed to the \_\_\_\_\_\_\_\_\_
If K is a large number, it means that the equilibrium concentration of the products is LARGE. In this case, the reaction as written will proceed to the RIGHT (resulting in an increase in the concentration of products)
115
What was Ammonia used to synthesized?
Weapons of war like TNT and trinitrotoluene
116
What is a reaction called when products will collide in a certain time.and lead to the reforming of reactants?
Reversible reaction
117
You have a balanced reaction where K is more than 1. Which side of the equation does this equilibrium constant favor?
The products
118
How is SO₂(g) obtained for the Contact Process reaction of 2SO₂(g) + O₂(g) ⇌ 2SO₃(g) ∆H°= -197 kJ/mol? 2
From burning sulfur Or Sulfide ores
119
Given: C₂H₅OH(l) + CH₃COOH(l) ⇌ CH₃COOC₂H₅(l) + H₂O(l) In which direction will the equilibrium shift if: A) the ester is removed
Stress: Favoured: Direction: right/forward
120
What is the Equilibrium law for the reaction of wA + xB ⇌ yC + zD?
Kc = [A]ʷ [B]ˣ / [C]ʸ [D]ᶻ
121
temp (in k) is ______________ to avg KE of particles in a substance
temp (in k) is proportional to avg KE of particles in a substance
122
How do you find the unit of k?
Generally units of k are concentration⁽¹ ⁻ ᵒᵛᵉʳᵃˡˡ ᵒʳᵈᵉʳ⁾ time⁻¹
123
What are two graphically ways we can show rate of reaction?
Decrease in reactant with time Increase in product with time
124
why does only temp change Kc? 7
- pressure and conc affect Q (NOT Kc) - the equilibrium shifts to oppose the change - this results in equal rates on both sides again, leaving Kc unchanged - however, activation energies differ between forward and backward rxn - and the energy change is not the same on both sides - altering temp allows one rxn to proceed faster than the other - this alters Kc
125
What did Alfred Nobel created when he added the nitroglycerin, C₃H₅N₃O₉(l) to porous silica, which allowed safe handling?
Dynamite
126
State the four factors that affect the reaction rate and provide: A) an explanation why it causes the rate to increase and B) an example for each
Reactions generally only occur at the surface of a solid. Making a solid more finely divided increases the surface area and therefore the number of particles exposed at the surface. The effective concentration of the particles of the solid has thus been increased and there is a greater chance of a particle of the other reactant colliding with a particle on the surface and reaction occurring. Powdered reactants react faster When there is a low surface area, only the particles on the outside are exposed on the surface and able to collide with the particles in a certain time. When there is a high surface area, all the particles are exposed and are able to collide with the particles in a certain time. Example: Dissolving sugar cubes vs sugar grains Melting ice cube vs. ice chips Concentration With more particles in a certain volume, the particles collide more often (the collision frequency is higher) and therefore there is greater chance of a successful collision occurring in a certain time. When there is a lower concentration, the particles are further apart and collide less frequently in a certain time. When there is a higher concentration, the particles are closer together and collide more frequently in a certain time. Temperature 1) More collisions occur as average of kinetic energy More particles travel faster This means that the collision frequency increases, i.e. the particles collide more often. Not only do they collide more often, but they also collide harder in a certain time. 2) More collisions have energy larger than activation energy Each particle likely has more energy Small increase in temperature greatly increases number of particles above the threshold energy A 10K increase will roughly double the reaction rate Increasing the temperature has a major effect on the rate of the reaction. As the temperature increases, the rate of reaction increases exponentially. It is often said that as a rough rule of thumb, a rise in temperature of 10K causes the reaction rate to be approximately doubled. As the temperature increases, the molecules have more energy and therefore move faster. This means that the collision frequency increases, i.e. the particles collide more often. Not only do they collide more often, but they also collide harder, that is with more energy, so there is greater chance that a collision will result in a reaction in a certain time. Catalyst 5 (4 and 1 example) A substance that provides an alternate reaction pathway of a lower activation energy Speeds up the a reaction (increases the rate) Remains unchanged at the end Lowers the activation energy for a reaction In a Maxwell-Boltzmann, the shaded represents the # of particles with energy greater than or equal to the activation energy for the uncatalysed reaction. The checked area represents the # of particles with energy greater than or equal to the activation energy for the catalysed reaction. A larger # of particles have energy greater than the activation energy; ∴ a greater proportion of collison result in reaction and the reaction rate increases.
127
Many compounds containing nitrogen decompose quickly or slowly?
Many compounds containing nitrogen decompose QUICKLY (Explosively)
128
What is sulfuric acid, H₂SO₄(aq), used in? 5
1) Fertilizers 2) Paints 3) Detergents 4) Fibres 5) Production of other chemicals
129
Define the term "rate determining step".
The slowest step in a reaction mechanism
130
What type of bond does a molecule of nitrogen contain?
A strong triple bond (941 kJ/mol)
131
A first order reaction will increase _______ 2
A first order reaction will increase linearly (double) Increasing in a straight line
132
Given: CO₂(g) + H₂(g) ⇌ CO(g) + H₂O(g) ∆H°= +41 kJ/mol In which direction will the equilibrium be shifted by each of the following changes? A) increasing the concentration of CO(g)
Stress: Favoured: Direction: left/reverse
133
To make Ammonia, where did Fritz Haber get the nitrogen from?
From the air
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What factor will not affect the equilibrium within a solution but will affect the equilibrium of gases?
Pressure
135
For the question; Given the following reaction: H₂S(g) + I₂(s) ⇌ 2HI(g) + S(s). The concentrations of 0.5M for H₂S(g) and 0.2 M for HI, what is the value for Kc? This is the answer; Kc=[HI]²/([H₂S]) Kc=0.2²/0.5 Kc=0.08 If you were to reverse the previous reaction, what would the Kc value be?
Kc=1/0.08 Kc = 12.5
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If K is a small number, it means that the equilibrium concentration of the reactants is \_\_\_\_\_\_\_\_. In this case, the reaction as written will proceed to the \_\_\_\_\_\_\_\_
If K is a small number, it means that the equilibrium concentration of the reactants is large. In this case, the reaction as written will proceed to the left (resulting in an increase in the concentration of reactants)
137
What does Nitrogen Fixation unintentionally? 3
Automobile engines do it unintentionally Bad for air nitrous oxides + water ===\> acid rain
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In reversible reactions, each collision forming may go on to form ________ or reform \_\_\_\_\_\_\_
In reversible reactions, each collision forming may go on to form PRODUCTS OR reform REACTANTS
139
State Le Chatelier's Principle.
Le Chatelier's Principle states that if a system at equilibrium is subjected to some change, the position of equilibrium is shift in order to minimize the effect of change.
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How did Alfred Nobel made handling nitroglycerin, C₃H₅N₃O₉(l), safer?
He added the nitroglycerin, C₃H₅N₃O₉(l) to porous silica, which allowed safe handling
141
Write the equilibrium constant expressions for the following reactions at equilibrium. D) 2NO(g) + 2H₂(g) ⇌ N₂(g) + 2H₂O(g) + 664 kJ
Kc = [N₂] [H₂O]² / [NO]² [H₂]²
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What is the Haber process used currently?
To peacefully convert N₂(g) to ammonia for fertilizers Then injected into soil of farmer's fields
143
At the same temperature, _________ particles travel faster than ________ ones
At the same temperature, lighter particles travel faster than heavier ones
144
State the conditions needed for the optimum yield of sulfuric acid in the Contact process. Justify why these conditions are used. 3
1) High pressure - 3 moles of gas forming two moles of gas …………………………- 2 atm used ↠ The production of H₂SO₄(aq) requires the reaction of 2SO₂(g) + O₂(g) ⇌ 2SO₃(g). Where SO₂(g) is obtained from burning sulfur or sulfide ores and O₂ is obtained from fractional distillation of liquid (compressed) air. Using high pressure shifts the reaction to the right, making more SO₃(g). SO₃(g) is then added with water to finally make H₂SO₄(aq). 2) Ideal temperature is 450°C ↠ 450°C is an ideal high temperature that favours the reverse reaction, which increase the reaction rate. 3) Adding vandaium (V) oxide as a catalyst ↠ Adding the catalyst increases rate without affecting equilibrium. ⇝ The yield rate at these conditions is 99%. Using a higher pressure would be uneconomical
145
Given: C₂H₅OH(l) + CH₃COOH(l) ⇌ CH₃COOC₂H₅(l) + H₂O(l) In which direction will the equilibrium shift if: C) sulfuric acid catalyst is added
Stress: Favoured: Direction: no effect
146
What are the characteristics of the reaction when K is less than 1?
If K is less than 1, the mixture contains mostly reactants. The reaction hardly proceeds at all
147
The _________ Is the energy needed to overcome repulsions, to start breaking bonds, to deform molecules and to allow rearrangement of atoms, electrons etc.
The Activation Energy Is the energy needed to overcome repulsions, to start breaking bonds, to deform molecules and to allow rearrangement of atoms, electrons etc.
148
What happens to the concentration of the reactants during Dynamic Equilibrium?
Concentrations of reactants and products do not change
149
If K is a small number, it means that the equilibrium concentration of the products is \_\_\_\_\_\_\_. In this case, the reaction as written will proceed to the \_\_\_\_\_\_\_\_
If K is a small number, it means that the equilibrium concentration of the products is small. In this case, the reaction as written will proceed to the right (resulting in an decrease in the concentration of reactants)
150
Describe three specific ways to increase the rate of the following reaction from lab #11 "Production of copper": Mg(s) + CuSO₄(aq) ===\> Cu(s) + MgSO₄(aq)
1) use a Mg powder instead of strips 2) increase [CuSO₄] or [Mg] 3) heat the CuSO₄(aq) or Mg(s) 4) add a catalyst
151
What type of bond does N₂(g) have?
A strong triple bond (941 kJ/mol)
152
In practice, ________ is measured using any properties that differ between reactants and \_\_\_\_\_\_\_\_?
Concentration, Products
153
State how adding a Catalyst as one of the four factors that affect the reaction rate and provide: A) an explanation why it causes the rate to increase and B) an example of each 5 (4 and 1 example)
A substance that provides an alternate reaction pathway of a lower activation energy Speeds up the a reaction (increases the rate) Remains unchanged at the end Lowers the activation energy for a reaction In a Maxwell-Boltzmann, the shaded represents the # of particles with energy greater than or equal to the activation energy for the uncatalysed reaction. The checked area represents the # of particles with energy greater than or equal to the activation energy for the catalysed reaction. A larger # of particles have energy greater than the activation energy; ∴ a greater proportion of collison result in reaction and the reaction rate increases.
154
What is the molecular formula of nitroglycerin?
C₃H₅N₃O₉(l)
155
technique to detect change in rxn
stopwatch - i.e. using something observable as an arbitrary endpoint for when to stop the watch
156
a rise in temperature of 10K causes the reaction rate to be approximately \_\_\_\_\_\_\_\_\_\_.
a rise in temperature of 10K causes the reaction rate to be approximately doubled.
157
What is the formula of kinetic energy
Kinetic energy=1/2 mv²
158
State the four factors that affect the reaction rate and provide: A) an explanation why it causes the rate to increase and B) an example of each
Reactions generally only occur at the surface of a solid. Making a solid more finely divided increases the surface area and therefore the number of particles exposed at the surface. The effective concentration of the particles of the solid has thus been increased and there is a greater chance of a particle of the other reactant colliding with a particle on the surface and reaction occurring. Powdered reactants react faster When there is a low surface area, only the particles on the outside are exposed on the surface and able to collide with the particles in a certain time. When there is a high surface area, all the particles are exposed and are able to collide with the particles in a certain time. Example: Dissolving sugar cubes vs sugar grains Melting ice cube vs. ice chips Concentration With more particles in a certain volume, the particles collide more often (the collision frequency is higher) and therefore there is greater chance of a successful collision occurring in a certain time. When there is a lower concentration, the particles are further apart and collide less frequently in a certain time. When there is a higher concentration, the particles are closer together and collide more frequently in a certain time. Temperature 1) More collisions occur as average of kinetic energy More particles travel faster This means that the collision frequency increases, i.e. the particles collide more often. Not only do they collide more often, but they also collide harder in a certain time. 2) More collisions have energy larger than activation energy Each particle likely has more energy Small increase in temperature greatly increases number of particles above the threshold energy A 10K increase will roughly double the reaction rate Increasing the temperature has a major effect on the rate of the reaction. As the temperature increases, the rate of reaction increases exponentially. It is often said that as a rough rule of thumb, a rise in temperature of 10K causes the reaction rate to be approximately doubled. As the temperature increases, the molecules have more energy and therefore move faster. This means that the collision frequency increases, i.e. the particles collide more often. Not only do they collide more often, but they also collide harder, that is with more energy, so there is greater chance that a collision will result in a reaction in a certain time. Catalyst 5 (4 and 1 example) A substance that provides an alternate reaction pathway of a lower activation energy Speeds up the a reaction (increases the rate) Remains unchanged at the end Lowers the activation energy for a reaction In a Maxwell-Boltzmann, the shaded represents the # of particles with energy greater than or equal to the activation energy for the uncatalysed reaction. The checked area represents the # of particles with energy greater than or equal to the activation energy for the catalyzed reaction. A larger # of particles have energy greater than the activation energy; ∴ a greater proportion of collison result in reaction and the reaction rate increases.
159
If Q = Kc, then the system is _______ at equilibrium
If Q = Kc, then the system is already at equilibrium
160
What does the Kinetic theory apply to reaction rates 2
Not only will particles collide with the container, but also each other These collisions sometimes result in reactions according to the collision theory
161
During Dynamic Equilibrium, [\_\_\_\_\_\_\_\_] doesn't need to equal [product]
During Dynamic Equilibrium, [reactant] doesn't need to equal [product]
162
If Q \> Kc, then essentially we have _______ \_\_\_\_\_\_\_ product and the reaction will proceed to the \_\_\_\_\_\_\_\_
If Q \> Kc, then essentially we have too much product and the reaction will proceed to the left (to reduce the concentration of product and increase the concentration of product)
163
Given: 2NO(g) + O₂(g) ⇌ 2NO₂(g) ∆H°= -2.7 kJ/mol What will happen to the concentration of NO₂(g) for each of the following. D) removal of some of the O₂(g)
Stress: Favoured: concentration of NO₂(g) goes down
164
State the conditions needed for the optimum yield of ammonia in the Haber process. Justify why these conditions are used. 4
1) High concentrations of N₂(g) and H₂(g) ➽ The ratio is always maintained at a ratio of 1:3 to make sure there is no limiting reactant and effective collisions are increased. 2) Use of catalyst - heated powdered iron oxide ➽ Heated powdered iron oxide is used because being powdered increases surface area for the reaction and being heated means that particles have more energy and collide harder, thus making sure there are a lot of effective collisions in a certain time. 3) Removal of Ammonia ➽ This drives equilibrium forward. 4) Ideal temperature is 450°C ➽ This ideal temperature is balances between high equilibrium yield and a faster reaction rate.
165
Given: CO₂(g) + H₂(g) ⇌ CO(g) + H₂O(g) ∆H°= +41 kJ/mol In which direction will the equilibrium be shifted by each of the following changes? B) decreasing the concentration of CO₂(g)
Stress: Favoured: Direction: left/reverse
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Explain what is meant by the term 'activated complex' and comment on the length of time it exists. 2
The term activated complex refers to the molecular compound or compounds that exist in the highest energy state during a chemical reaction.
An activated complex acts as a link between the reactants and the products of the reaction.
The energy of the activated complex is higher than that of reactants or the products, and the state is temporary. If there is not sufficient energy to sustain the chemical reaction, the activated complex can reform into the reactants in a backward reaction.
