kinetics class #1 ob: intro to kinetics and equilibrium chemistry. factors that affect the rate of...

Kinetics Class #1

OB: intro to kinetics and equilibrium chemistry. Factors that affect the rate of chemical equations, and some Potential Energy Diagrams (graphs) that show the energy of chemical reactions.

Some reactions are fast, like the very first one you saw on the first day.

Remember the synthesis of water?

1. Hydrogen gas + oxygen gas + energy _________ + ___________

Some are rather slow, remember the decomposition of hydrogen peroxide?

2. Hydrogen peroxide ______________ + _________________

That second one was SOOOOO SLOOWWWW it took a catalyst to make it happen!3. The catalyst was potassium iodide, a white salt. Where do we write it in that equation?

________________________________________________________________ (put it there now)

4. Kinetics is the part of chemistry that studies the __________ of _________________ 5. We will again examine reactions that absorb energy to occur, called

__________________________ reactions.

6. And their opposites, reactions that emit energy as a product, called

___________________________ reactions.

One of the simplest reactions we know is the combustion of methane.

CH4(G) + 2O2(G) → 2H2O(G) + CO2(G) + energy

We know a lot about this reaction too, let’s start naming things:This reaction is:

7. This reaction is: combustion, it’s _________________, the heat of reaction for this reaction is

_______________ from table I.

8. The energy is written with the __________.

9. The forward reaction is __________________ because energy is a product.

CH4(G) + 2O2(G) → 2H2O(G) + CO2(G) + energy

10. The mole ratio of this equation would be: __________________________

11. The thermochem mole ratio would be ______________________________

12. This reaction tends to be irreversible because? ___________________

_______________________________________________________________

________________________________________________________________.

This reaction is different:

2H2O(L) + energy → O2(G) + 2H2(G)

2H2O(L) + energy → O2(G) + 2H2(G)

14. For starters, since energy is a reactant, this reaction must be

_____________________ with a _______ΔH.

15. In fact, on table I, the actual ΔH is ____________________________(?)

16. Wait a second, is this reaction even on table I? ___________________

________________________________________________________________

17. What is the ΔH then? __________________

2H2O(L) + energy → O2(G) + 2H2(G)This reaction is

18. __________________, and the energy is written with the

____________________________________ (it’s absorbed).

19. It is also ______________________ because it has 1 chemical reactant.

On the next slide we will look at 7 reactions. You decide if they are exo or endothermic, PLUS you indicate a +ΔH, or a – ΔH

ReactionActual

ΔH

Exo or

endo

20 2C8H18(L) + 25O2(G) → 16CO2(G) + 18H2O(G)

21 N2(G) + O2(G) → 2NO(G)

22 2C(S) + H2(G) → C2H2(G)

23 4Al(S) + 3O2(G) → 2Al2O3(S)

24 C3H8(G) + 5O2(G) → 3CO2(G) + 4H2O(G)

25* CO2(G) → C(S) + O2(G)

26* NaOH(S) Na+1(AQ) + OH–1

(AQ)

H2O

Something special about #25 and #26. See if you can figure that out!

ReactionActual

ΔH

Exo or

endo

20 2C8H18(L) + 25O2(G) → 16CO2(G) + 18H2O(G) -10943 kJ/mole

exo

21 N2(G) + O2(G) → 2NO(G) +66.4kJ/mole

endo

22 2C(S) + H2(G) → C2H2(G) +227.4kJ/mole

endo

23 4Al(S) + 3O2(G) → 2Al2O3(S) -3351

kJ/moleexo

24 C3H8(G) + 5O2(G) → 3CO2(G) + 4H2O(G) -2219.2kJ/mole

exo

25* CO2(G) → C(S) + O2(G) +393.5kJ/mole

endo


(AQ)-44.51kJ/mole

exoH2O

Something special about #25 and #26. See if you can figure that out!

25* CO2(G) → C(S) + O2(G)


(AQ)

H2O

Something special about #25 and #26. See if you can figure that out!25* CO2(G) → C(S) + O2(G)

26* NaOH(S) Na+1

(AQ) + OH–1(AQ)

#25 is backwards on table I from the way it’s written here. On Table I the reaction that has carbon + oxygen forming into CO2 and it has a ΔH o f –393.5 kJoules/mole. Since this reaction is written in reverse, we reverse the ΔH also: the ΔH of this reaction is +393.5 kJ/mole.

#26 is NOT really a reaction, rather it is a phase change for the NaOH – from Solid Aqueous

H2O

First we will look over the 4 factors that affect the rate of reaction, but you don’t really know what rate of reaction means yet, so let’s tell a story…

Let’s talk about driving from our school to Johnson City High School. It’s 7.07 miles according to mapquest.com

If you drive there in 20 minutes, you are driving 7.07 miles in 0.33 hours.

That works to be about 21.1 miles per hour.

The time it takes is related to, but 27. TIME IS NOT THE SAME THING AS YOUR RATE OF SPEED.

If you drive there in just ten minutes, you are driving 7.07 miles in about 0.17 hours, or about 41.6 miles per hour!

Same distance, small change in time, crazy rate change.

28. Time ≠ rate. Not in driving, or in chemistry.

The time it takes for a chemical reaction to occur is measured in seconds.

29. The rate has a weird unit of seconds-1 or it can be understood to be:

1seconds

The 4 factors that affect the rate of a chemical reaction (NOT the time it takes)30. Increase in Temperature – hotter usually means the reaction will happen faster

31. Increase reactant surface area – which allows the reactants to react faster

32. Increase the concentration of the reactants – more stuff, more chance for a reaction to happen

33. Adding a catalyst

The first three of these will work because of ONE reason, the catalyst works a different way.

All of these four ways will increase the rate of a chemical reaction.

Rate of reaction does NOT equal the time it takes!

The first three factors are all related to making the particles that are in the reaction move faster. Why would more particle motion make for a faster reaction?

34. ____________________________________________

What actually happens at the invisible atomic level during a chemical reaction?

35. ______________________________________________

With _____________________________________and also

_______________________ _______________________.

Let’s use the hydrogen gas plus oxygen gas synthesize into water to fine tune our thoughts on this.

What happens???

When the two gases are released together, say by popping the balloon, no reaction happens. Why? The molecules can get together, but not with enough energy.

To react, particles must collide with other particles with both enough energy and proper orientation.

It’s like looking for love…

This guy is looking to fall in love, but no matter how he tries, he can’t seem to bump into the love of his life. No collisions, no chance at love.

36. When particles don’t collide, they don’t react.

These two fish (two molecules) missed each other, and any chance for romance.

When molecules don’t collide, they cannot react together.

And even if you collide, with the proper orientation, if you bump too hard, you can’t react, you bounce off of each other before you have the chance!

In order to react, particles must collide with sufficient energy, but not too much, in the proper orientation. If this happens, a reaction can happen.

In order for chemical reactions to occur, sufficient particles must collide with proper orientation, and proper energy, to start and sustain a reaction.

Any factors that increase the likelihood of collisions will increase the rate of a chemical reaction.

Let’s review those 4 factors right here, do they increase the likelihood of collisions??

37 Increase in Temperature – YES OR NO

38 Increase reactant surface area – YES OR NO

39. Increase the concentration of the reactants – YES OR NO

40. Adding a catalyst YES OR NO

That’s 3 yes votes in a row, but #4 is a big no here!

Let’s review

Increasing temp will speed up the particles, making them move faster will increase the power of collisions, and the speed will make them make more collisions (good).

When there’s more surface area, there are more places for the collisions to happen, so that too will work to speed up the rate of the reaction. (rate ≠ time!)

With more concentration, that will also increase the collisions, the stuff is everywhere! (not like being on a deserted island at all)

What about catalysts??? They do not increase collisions, but still speed up reactions, still increase the rate of reactions, but the reasons will remain unknown until tomorrow!

What’s a POTENTIAL ENERGY DIAGRAM?

41. Potential energy diagrams show the flow of energy in a chemical reaction, start to finish, and some of the neat “parts” of a chemical reaction too

42. They come in two flavors, one for the __________________ reactions with a _____ΔH

and another kind for the ______________________reactions with a _____ΔH.

41. We will draw on the next pages an exothermic potential energy diagram for the combustion of methane. All exothermic potential energy diagrams “look” similar, the only real difference is the Y axis scale. The exothermic reactions (think now) give off energy as a product, so they must START with more energy than the end up with since much energy is released into the Universe. It’s “lost” from the reaction, but hardly lost. The Law of Conservation of energy is:

43. Energy cannot be created or destroyed in any chemical reaction, but it can be transferred.

How to draw a potential energy diagram (we’ll do lots of these, don’t worry now)

Potential Energy

kJ/mole

The time of the reactionTime zero

End of reaction

0 kJ

Title goes here… this one will be called:

Potential energy diagram for combustion of methane

Potential Energy

kJ/mole


End of reaction

0 kJ


The reactants, in this case methane and oxygen, have some potential to explode. This “energy” is known, but for now, we’ll just use a line without exact kJ/mole.

Potential Energy

kJ/mole


End of reaction

0 kJ


You can carry around your methane and oxygen all day relatively safely. As long as you don’t add some heat, the explosion won’t happen. To react, the particles need to collide with sufficient energy and proper orientation. They don’t have that yet.

Potential Energy

kJ/mole


End of reaction

0 kJ


If we begin to warm the reactants up (with some heat) this is what happens…

Dangerous, but not a kaboom yet…

Potential Energy

kJ/mole


End of reaction

0 kJ


Here we are literally at the “point of no return”. One more spot of energy and we won’t be able to hold the reaction back. It’s like being at the very top of the roller coaster as it gets to the top of the first big hill!

Potential Energy

kJ/mole


End of reaction

0 kJ


At this point the kaboom has started, and the reaction has “paid back” the start up energy (AE). We’re back to where we started from an energy point of view. But, we’re not able to stop here.

AE

Potential Energy

kJ/mole


End of reaction

0 kJ


The kaboom keeps happening, the reaction releases all the heat it has to. The products form and they are dull, dull, dull (from an energy point of view).

Potential Energy

kJ/mole


End of reaction

0 kJ


The products, water and CO2 are mostly unreactive. They have a low potential energy. The products have a much greater potential energy. The difference between the potential of the reactants and products is the ΔH.

A –ΔH is needed here, and that indicates EXOTHERMIC.

reactants

products

-ΔH

Potential Energy

kJ/mole


End of reaction

0 kJ


reactants

products

Make sure this diagram has these labels with units, and these definitions below:45. Potential Energy of Reactants: ____________________ 46. Potential Energy of Products: __________________________________ 47. ΔH: __________________________ Here the ΔH is ___________ 48. Activation Energy (AE): _____________________________________________

Using Table I to help us along…Draw the 53. Potential energy diagram for formation of C2H2(G)

Potential energy diagram for formation of C2H2(G)

PEkJ/mole

Time of reaction

PE Reactants

PE Products

AE activation

energy

+ ΔH

Endothermic Potential Energy Diagram has a +ΔH

54. Let’s draw the potential energy diagram for

sodium hydroxide dissolving into water

Time of the reaction…

Potential energy

kJ/mole



Potential energy

kJ/mole

First, write yourself the balanced thermochemical equation, and make note of exo or endothermic…

NaOH(S) Na+1(AQ) + OH-1

(AQ) + energy ΔH = -44.51 kJ (exo)



Potential energy

kJ/mole

Now we draw

NaOH(S) Na+1(AQ) + OH-1

(AQ) + energy ΔH = -44.51 kJ (exo)

-ΔH

AEreactants

products

We don’t know the actual levels, but we know that this difference is 44.51 kJ/mole

Represents the activation complex, the transition between R + P.

Vocab x 555. Potential energy – the energy stored in the bonds of the reactants or the products

56. Activation energy – the energy it takes to start a chemical reaction. It must be sufficient or else.

57. Activation complex – the transitional state of being, where reactants are coming apart but are not yet products

58. ΔH – the difference between the potential energy of the reactants + the potential energy of the products

59. Potential energy diagram – a graph showing the flow of energy of a chemical reaction. Can be exo or endothermic

60. Draw the PE diagram for the synthesis of aluminum oxide. Make the balanced thermochemical equation your title. Label the reactants, products, AE, AC, ΔH (make it + or – as needed), and put labels on the graph too. Go!

Draw the potential energy diagram for the synthesis of aluminum oxide. Label the reactants, products, AE, AC, ΔH (make it + or – as needed), and put labels on the graph, and a title too. Go!

PE diagram for synthesis of aluminum oxide ΔH = -3351 kJ/mole

Al + O2

Al2O3

-ΔH

AEAC

PEkJ/mole

Time of the reaction

In an endothermic reaction, energy is absorbed, the products have more energy in them than the reactants had. Where does this energy come from?

(the environment – which is why these reactions feel cold. They “steal” energy from the immediate surroundings, bringing into the bonds of the reaction.

61.We will attempt to draw the PE diagram for the dissolving of sodium chloride into water

NaCl Na+1 + Cl-1 + energy ΔH = +3.88 kJ/mole

Go!

Table salt dissolves in water, ΔH = +3.88 kJ/mole

PEkJ/mole

Time of reaction

salt

Ions in solution

+ΔHAE

Endothermic +ΔH

62. Draw the PE diagram for the combustion of propane.

Indicate the PE of reactants, products, AE, AC, ΔH, and a title. Title:

Y axis label

X axis label

Draw the PE diagram for the combustion of propane.Indicate the PE of reactants, products, AE, AC, ΔH, and a title.

The combustion of propane ΔH = -2219.2 kJ/mole

P E

kJ/mole

Reaction time

C3H8 + O2

CO2 + H2O

-ΔH

AE

NOTE: the PE of the products is less than the PE of the reactants.

63. Where is the missing energy? Matter, nor energy, can be created ordestroyed in any chemical reaction, or physical change.

Kinetics Class #3

The affect of catalysts on chemical reactions

64 + 65 Draw the PE diagram for both lithium bromide dissolving into water, and for ammonium chloride dissolving into water. Make 2 graphs big, so we can label PE of reactants and products, AE, AC, and ΔH (+ or -), and titles with axis labels.

This should only take 4 minutes! Click ahead now

time

PPEkJ/molePE

kJ/mole

Lithium bromide becomes aqueous ΔH = -48.83 kJ/mole

Ammonium chloride gets aqueous ΔH = +14.78kJ/mole

RR

P-ΔH

AEAE +ΔH

AC AC

time

Exothermic on left Endothermic on right

66. Define Catalyst

66. Define Catalyst A substance that speeds up a chemical reaction without changing it in any other way. It doesn’t get used up, it doesn’t alter the amount of energy absorbed or released. It lowers the activation energy required to start a reaction, or it offers a different chemical pathway that makes it happen faster.

time

PPEkJ/molePE

kJ/mole



RR

P-ΔH

AEAE +ΔH

AC AC

time

WHAT HAPPENS IF YOU ADD A CATALYST TO THESE REACTIONS?

Exothermic on left Endothermic on right

time

PPEkJ/molePE

kJ/mole



RR

P-ΔH

AEAE +ΔH

AC AC

time

With a catalyst, the PE of reactants and products can’t change, nor can the ΔH. What does change

is the AE, which is lowered.

67. Show the catalyst effect on the last 2 PE DIAGRAMS now.

How does a catalyst work?

It does NOT change the number of collisions of particles.

Catalysts are said to work in 2 different ways….

68. Catalysts lower the activation energy of a reaction. This lets the reaction start in a less energetic way, so it can happen quicker than normal. Once it starts, it moves right along.

69. Catalysts are said to provide “an alternate pathway” for the reaction to proceed, which lets this reaction happen quicker. (it’s like it provides a shortcut)

Demo: Catalysts speed up the rate of a chemical reaction.

We’ll watch the decomposition of hydrogen peroxide once more, but with a different eye, now we’re much more educated and we’ll understand at a deeper level.

H2O2 solution

+ KI

Catalyst

Demo #2 Catalysts are written above the reaction arrow.

2H2O2 2H2O + O2 + ENERGY (exothermic)

H2O2 solution + KI

Catalyst

WOW!BORING

KI

The same reaction will happen at left, just MUCH SLOWER!

70. Does the amount of energy given off change between the uncatalyzed or catalyzed reactions? ______

71. Does it “seem so”? ______

72. How would we explain that the reaction with the catalyst “seems to give off so much more energy”?

Kinetics Class #4

OB: reactions that are in dynamic equilibrium and how to “push” them forward, or reverse using LeChatelier's Principle.

Most chemical reactions are “one way”, meaning that once they happen, they are done. Spontaneous reversals in chemistry are not common, because most reactions are without enough energy to go the other way.

The Potential Energy diagrams show us the huge energy demand it would take to go backwards. Usually the energy required is “lost” to the environment.

73. Some reactions are reversible because the energy requirements are much less, for a variety of reasons.

One of the most important reactions that is reversible, is the simultaneous synthesis of ammonia from nitrogen and hydrogen, and the decomposition of ammonia into nitrogen and hydrogen, shown below…

N2 + 3H2 2NH3

When a reaction is reversible (easily) and you let it happen, you will end up with both synthesis and decomposition. Both a forward and a reverse reaction will both happen, and the “system” will reach a dynamic equilibrium.

If enough synthesis occurs, and enough ammonia forms, then it will start to decompose faster. That would create excess nitrogen and hydrogen, setting off a push to synthesize. Over time, the rate of the forward reaction is equal to the rate of the reverse.

This is dynamic equilibrium.

NOTE: In a dynamic equilibrium situation, you do NOT necessarily have equal masses, or equal moles on both sides of the reaction, but you do have equal rates of forward and reverse reactions.

nitrogen and

hydrogen

ammonia and

energy

the RATE of the forward reaction = the rate of the reverse reaction.

75. Is a reversible chemical reaction where…

76. Anytime you disrupt a dynamic equilibrium by adding (or subtracting, or changing temperature or pressure) the system has to adjust to accommodate this chemical stress, and a NEW different dynamic equilibrium forms.

nitrogen and

hydrogen

ammonia and

energy

76. What happens if we pump in a bunch of ammonia gas to this closed system?

ammonia, ammonia, ammonia,

ammonia, + energy

nitrogen and hydrogen

If this situation happens, a lot more decomposition will happen because there is so much ammonia, the reverse reaction will push backwards until a new balance is reached.

77. LeChatelier's Principle:

A chemical system in dynamic equilibrium will stay at equilibrium, and if a chemical stress is applied, the system will shift to counter act this stress, until a new equilibrium is reached.

The chemical stresses that could be applied are limited to these:

Change in pressure

Change in temperature

Add reactants

Remove reactants

Since the reactions are reversible the word “reactants” refers to reactants or products.

N2 + 3H2 2NH3 + energyThis closed system is in dynamic equilibrium. Let’s apply some stresses, and see which way the system will “push” to create a new dynamic equilibrium.

79. Add nitrogen

80. Add hydrogen

81. Add ammonia

82. Add energy (heat)

83. Add pressure


Add nitrogen

Add hydrogen

Add ammonia

Add energy (heat)

Add pressure


84. Remove nitrogen

85. Remove hydrogen

86. Remove ammonia

87. Remove energy (cool system)

88. Lower pressure

4Al + 3O2 2Al2O3 + Energy

Here, the forward reaction is exothermic, the reverse is endothermic.

The forward reaction is synthesis, the reverse is decomposition. This reaction is at dynamic equilibrium.

We cannot know how much aluminum, oxygen, or aluminum oxide is on hand, but we do see that the rate of synthesis (forward) is equal to the rate of the reverse (decomposition). The reactions continue, but the amounts remain constant.

Let’s stress this out now…

89. Add aluminum oxide

90. Remove oxygen

91. Remove heat (cool system)

92. Add aluminum

93. Add Heat

94. Increase pressure

4Al + 3O2 2Al2O3 + Energy

Let’s stress this out now…

Add aluminum oxide

Remove oxygen

Remove heat (cool system)

Add aluminum

Heat system

Increase pressure

A couple of things to pay attention to…

95. Pressure only has an effect on gases, it has NO effect on solids, liquids, or aqueous solutions.

If a stress “stops” a forward reaction, the reverse keeps happening.

If a stress “stops” a reverse reaction, the forward keeps happening.

At least for a while, until a new balance is reached.

Sometimes we “play” in chemistry, and use a reaction that is not so easily reversed with LeChatelier. If the double arrows are there, the reaction does go both ways.

CH4(G) + 2O2(G) CO2(G) + 2H2O(G) + energy

96. Add methane

97. Add water

98. Add heat

99. Remove carbon dioxide

100. Remove heat

101. Remove methane

102. Add carbon dioxide

103. Increase pressure

104. Decrease pressure

CH4(G) + 2O2(G) CO2(G) + 2H2O(G) + energy

96. Add methane

97. Add water

98. Add heat

99. Remove carbon dioxide

100. Remove heat

101. Remove methane

102. Add carbon dioxide

103. X Increase pressure X

104. X Decrease pressure X

Both sides have equal moles of gases, pressure is steady

Review for Kinetics

Copy, write, think, do.

Questions

105. Is this an exo or endothermic reaction?106. What is the potential energy of the activated complex?

107. What is the PE of the products?108. What is the ΔH?

109. What would be a possible activation energy with a catalyst?

Questions

105. Is this an exo or endothermic reaction? exo106. What is the potential energy of the activated complex? 175 kJ/mole

107. What is the PE of the products? 50 kJ/mole108. What is the ΔH? -50 kJ/mole

109. What would be a possible activation energy with a catalyst? Less than 75 kJ/mole

Examine this closely!

Now answer these questions!

110. What is the PE of the reactants?

111. What is the activation energy for this reaction?

112. Is this reaction exo or endothermic?

114. What are possible AE values for this reaction with a catalyst?

115. What is the ΔH for this reaction?

116. Would the ΔH for this reaction change with a catalyst?

Now answer these questions!

110. What is the PE of the reactants? 50 kJ/mole

111. What is the activation energy for this reaction? 175 kJ/mole

112. Is this reaction exo or endothermic? endo

114. What are possible AE values for this reaction with a catalyst? Less than 175, more than 50 kJ/mole

115. What is the ΔH for this reaction? +50 kJ/mole

115. Would the ΔH for this reaction change with a catalyst?

No, only the AE

There are four different dynamic equilibrium reactions in the drills section of the website, four that I’d try later tonight. You think that this is a good idea???

In this dynamic equilibrium…

3A(G) + B(S) 3C(G) + D(G) + energy

118. Add heat119. Add B120. Inc. pressure121. Remove D122. Add C

There are four different dynamic equilibrium reactions in the drills section of the website, four that I’d try later tonight. You think that this is a good idea???

In this dynamic equilibrium…

3A(G) + B(S) 3C(G) + D(G) + energy

Add heatAdd B

Inc. pressureRemove D

Add C

123. State in plain language, and in complete sentences, LeChatelier’s Principle

124. State the 4 stresses that can be applied to a dynamic equilibrium reaction.

LeChatelier’s Principle

Chemical systems at equilibrium tend to stay at equilibrium. When a chemical stress is put upon a chemical system in equilibrium, it will shift to relieve that stress, and a new dynamic equilibrium forms.

124. Stresses include changes in pressure, temperature, and adding/removing reactants.

125. There are 4 factors that would cause a chemical reaction to speed up. 3 of them work one way, the 4th factor works a different way.

What are they, explain the ways they work.

There are 4 factors that would cause a chemical reaction to speed up. 3 of them work one way, the fourth factor works a different way.

What are they, explain the ways they work.

1. Increase temp = more Kinetic energy = more collisions = faster reaction

2. Increase surface area of reactants = more collisions = faster reactions

3. Increase concentration of reactants = more collisions = faster reactions

4. Use a catalyst = lowers the Activation Energy required or provides an alternate pathway = faster reaction (no change in collisions)

Entropy is the Measure of disorder in a chemical system. In AP Chem it has units and numbers, in our course it is just a definition, and a comparison.

Much disorder = HIGH ENTROPY

No disorder = LOW ENTROPY

126. Compare or Rank these phases of matter for entropy:

Water Steam

Ice

Compare or Rank these phases of matter for entropy:

Water Medium entropy Steam Highest entropy (most disorder)

Ice Lowest entropy (most order)

127. If all of these particles are at the same temperature (305 K) and the same pressure (105 kPa), which has the most and which has the least entropy?

Carbon monoxide octane

Sucrose (table sugar)

If all of these particles are at the same temperature (305 K) and the same pressure (105 kPa), which has the most and which has the least entropy?

Carbon monoxide octane

Sucrose (table sugar)

Most/smallest particles

Least entropy/biggest particlesmedium

Which arrow directions is more likelylefty or righty?

If mountains crumble to the sea, there will still be you & me. 128. From the NYS Curriculum:

Systems in nature tend to undergo changes toward lower energy and higher entropy. (boulders break up)

Note, entropy is one thing, but energy is included as well.

Energy is spent, is spreads out, it does not come back.

Heat radiates away, it does not accumulate in one place.

kinetics class #1 ob: intro to kinetics and equilibrium chemistry. factors that affect the rate of...

Documents

energy of chemical reactions

heat of reaction

forward reaction

simplest reactions

co2g cs o2g

kjmoleexo21n2g o2g

chemical reactant

reactionactual hexo