Chemical Reactions Notes PDF

UNIT 5: CHEMICAL REACTIONS Table of Contents Balancing Equations/Conservation of Mass Types of Chemical reactions Predicting Reactions Net Ionic Reactions Reaction Rates mass _____ AgF + _____ CaCl2 → _____ AgCl + _____ CaF2 _____ AgF + _____ CaCl2 → _____ AgCl + _____ CaF2 2...

UNIT 5: CHEMICAL REACTIONS Table of Contents Balancing Equations/Conservation of Mass Types of Chemical reactions Predicting Reactions Net Ionic Reactions Reaction Rates mass _____ AgF + _____ CaCl2 → _____ AgCl + _____ CaF2 _____ AgF + _____ CaCl2 → _____ AgCl + _____ CaF2 2 AgF + 1 CaCl2 → 2 AgCl + 1 CaF2 Our sample problem __ PbF2 + __AgNO3 → __AgF + __Pb(NO3)2  Step 1: Draw a box around each formula ____ PbF2 + ____AgNO3 → ____AgF + _____Pb(NO3)2 Never, ever change anything within these boxes. The formulas you start with are valid, so any changes you make to them will break the equation!  Step 2: Make an inventory of the atoms ____ PbF2 + ____AgNO3 → ____AgF + _____Pb(NO3)2 Determine how Element Number on Number on many atoms of reagent side product side each element Pb 1 1 are present on F 2 1 both the left and Ag 1 1 right sides of the N 1 2 equation. O 3 6  Step 3: Change a single number in the equation so the inventory works out evenly ____ PbF2 + ____AgNO3 → ____AgF + _____Pb(NO3)2 2 Since there are two Element Number on Number on F atoms on the reagent side product side reagent side and Pb 1 1 one on the right, F 2 1 let’s write a “2” in Ag 1 1 front of whatever N 1 2 contains F on the O 3 6 right so they’ll even out. Step 4: Redo the inventory with the new number ____ PbF2 + ____AgNO3 → ____AgF + _____Pb(NO3)2 2 Make sure you Element Number on Number on change the reagent side product side inventory for all of Pb 1 1 the atoms in that F 2 2 formula, in this Ag 1 2 case, Ag and F N 1 2 O 3 6  Step 5: If the columns aren’t yet identical, change another coefficient to get it closer 2 ____ PbF2 + ____AgNO3 → ____AgF + _____Pb(NO3)2 2 Since there is one Ag Element Number on Number on on the reagent side reagent side product side and two on the Pb 1 1 product side, let’s put F 2 2 a “2” in front of the Ag 1 2 compound that N 1 2 contains Ag on the O 3 6 reagent side  Step 6: Redo the inventory again 2 2 ____ PbF2 + ____AgNO3 → ____AgF + _____Pb(NO3)2 Element Number on Number on reagent side product side Both columns of Pb 1 1 atoms are the same! F 2 2 This means our Ag 2 2 equation is balanced! N 2 2 O 6 6 Our final, balanced equation: PbF2 + 2 AgNO3 → 2 AgF + Pb(NO3)2 _____ AgNO3 + _____ Ga → _____ Ag + _____ Ga(NO3)3 _____ AgNO3 + _____ Ga → _____ Ag + _____ Ga(NO3)3 3 AgNO3 + 1 Ga → 3 Ag + 1 Ga(NO3)3 _____ Li2SO4 + _____ K3PO4 → _____ Li3PO4 + _____ K2SO4 3 Li2SO4 + 2 K3PO4 → 2 Li3PO4 + 3 K2SO4 _____ ZnBr2 + _____ Pb(NO2)2 → _____ Zn(NO2)2 + _____ PbBr2 1 ZnBr2 + 1 Pb(NO2)2 → 1 Zn(NO2)2 + 1 PbBr2 SUMMARY How to balance equations (the very brief version): Write down a chart of all the elements before and after the arrow Count the number of atoms of each element and put in the chart Change one coefficient in the equation Redo the chart If it's not balanced, change another coefficient and repeat until it is SUMMARY Things to try if the equation doesn't balance: Start over from the very beginning. It's likely that you either messed up the inventory or are stuck in a rut and can't see what you're doing wrong. Start over and get a fresh start. If that doesn't work, start over again, but put a “2” in front of the most complicated looking formula. This often forces you to get a fresh perspective on the problem. If that doesn't work, try putting a “3” and so on. Use your gut instincts. What's the worst that can happen? It's not like you can get more wrong or anything. This isn't a big deal, so take some chances!  TYPES OF CHEMICAL REACTION Spoiler alert: There are six THOUGH ALL CHEMICAL REACTIONS ARE SPECIAL IN THEIR OWN WAY, IT’S HANDY TO CLASSIFY THEM INTO GROUPS After all, if chemical compounds can be put into groups where they do similar reactions, we can use this grouping to predict what compounds are likely to be formed in a reaction. This is handy for people who do chemical reactions. Person who does chemical reactions → SO, LET’S TALK ABOUT THE SIX TYPES OF REACTION AND WHAT THEY MAKE.  1. SYNTHESIS REACTIONS In synthesis reactions, simple compounds combine to make relatively complex ones. A+B→C Compound C can be just about anything, but in a practical sense for chemistry students trying to predict a reaction product, it’s likely to be something you’re familiar with already: H2O + CO2 → H2CO3  2. DECOMPOSITION REACTIONS The opposite of a synthesis reaction, these occur when molecules fall apart into relatively less complex ones. C→A+B Typically speaking, the compounds that C break into will be familiar compounds such as CO2, H2O, NH3, or some pure element: CaCO3 → CO2 + CaO 3. SINGLE DISPLACEMENT REACTIONS In a single displacement reaction, an element will trade places with an element from another compound: A + BC → AC + B If you see a pure element present with another compound, it’s probably one of these. Predict the products accordingly: Cu + 2 AgNO3 → Cu(NO3)2 + 2 Ag Note: These reactions will only occur if the pure element on the left side of the equation is more active than the one in the chemical compound it replaces.  Most reactive Least reactive 4. DOUBLE DISPLACEMENT REACTIONS These occur when the cations of two ionic compounds switch place with one another: AB + CD → CB + AD These reactions only occur if both reagents are soluble and one of the products is insoluble. KI(aq) + Pb(NO3)2(aq) → KNO3(aq) + PbI2(s) Otherwise, it’s impossible to isolate your product!  5. ACID-BASE REACTIONS These are double displacement reactions where water is made. The water is formed by the reaction of an acid with a base: HA + BOH → BA + H2O Also called “neutralization reactions”, they can result in the neutralization of acidic and basic solutions: HCl + NaOH → NaCl + H2O We generally assume that these reactions will occur when the reagents are combined, regardless of their formulas.  6. COMBUSTION REACTIONS In combustion reactions, something that contains C and H will react with oxygen – the products formed are always water and carbon dioxide (and lots of heat): CxHy + O2 → CO2 + H2O Bunsen burners use combustion reactions to generate heat: CH4 + 2 O2 → CO2 + 2 H2O  1. Do simple things make a complicated one? SYNTHESIS 2. Does a complicated thing make simple ones? DECOMPOSITION HOW TO 3. Does a lone element switch places with an element in a TELL WHAT compound? SINGLE TYPE OF DISPLACEMENT REACTION 4. Does an element in one IS TAKING compound switch places with another element in a PLACE compound? DOUBLE DISPLACEMENT 5. Does the equation contain oxygen, water, AND carbon dioxide? YES: COMBUSTION NO: ACID-BASE Lab Analysis Open the lab quickwrite. Open the Lab 10 sheet Review your answers from the lab Get ready to share :) Station 1: Copper wire reaction with a silver nitrate solution Station 1: Cu + AgNO3 → Station 2: lead nitrate and potassium iodide  Station 2: lead nitrate and potassium iodide Pb(NO3)2 + KI → Station 3: Ethanol  Station 3: Ethanol C3H8O Station 4: Baking soda + vinegar Baking soda + lemon juice  Station 4: Baking soda + vinegar Baking soda + lemon juice CH3COOH+Na CO3 → 2 Station 5: Elephant toothpaste Station 5: Elephant toothpaste H2O2 → Station 6: Teacher Demo Station 6: Teacher Demo Mg + O2 → MgO PREDICTING REACTION PRODUCTS The whole reason we need to know what the types of reaction are is so that we can predict the products of reactions that will take place when different compounds are combined or predict what reagents will form specific products. This is kind of the whole point of chemistry. This arrow contains the point of chemistry.  LET’S SEE HOW TO PREDICT REACTION PRODUCTS: There will always only be ONE compound on the right hand side of the equation. Use your periodic table to find the charges of each element to write the correct compound formula. Refer back to your naming compounds guided notes and resources if you get stuck! Predicting the product of a simple synthesis reaction A synthesis reaction will ALWAYS have the two elements or compounds combining together to form one. There will always only be ONE compound on the right hand side of the equation. You will use your periodic table to find the charges of each element to write the correct compound formula. Refer back to your naming compounds guided notes and resources if you get stuck! Example Na + Cl2 ---------> Example Na + Cl2 ---------> NaCl Let’s Do It Together Al + O2 ----------> Let’s Do It Together Al + O2 ----------> Al2O3 You try Mg + I2 -----------> You try Mg + I2 -----------> MgI2 You try K + Cl2 -----------> Let’s Do It Together K + Cl2 -----------> KCl You try Li + N2 -----------> You try Li + N2 -----------> Li3N Let’s Do It Together [Iron (II)] Fe + S ---------> Let’s Do It Together [Iron (II)] Fe + S ---------> FeS Let’s Do It Together [Copper (II)] Cu + S ---------> Let’s Do It Together [Copper (II)] Cu + S ---------> CuS You try Chromium (III) Cr + O2 ----------> You try Chromium (III) Cr + O2 ----------> Cr2O3  IF YOU SEE A SINGLE COMPOUND WITH AN ARROW AFTER IT, IT’S A DECOMPOSITION REACTION. A decomposition reaction will ALWAYS have one compound on the reactants side. It will always break apart into two or more products. You will look to see what elements are within the compound and split them up. If they are diatomic elements, remember to add a subscript of 2 below it on the product side. H 2CO 3 → H 2O + CO 2 OR H 2 + C + O 2 The left one is the correct answer, but there’s nothing technically wrong with either. Predicting the product of a simple decomposition reaction A decomposition reaction will ALWAYS have one compound on the reactants side. It will always break apart into two or more products. You will look to see what elements are within the compound and split them up. If they are diatomic elements, remember to add a subscript of 2 below it on the product side. Example N2O ----------> Example N2O ----------> N2 + O2 Let’s Do It Together Ni2O3 ------------> Let’s Do It Together Ni2O3 ------------> Ni + O2 You try Ag2O ------------> Let’s Do It Together Ag2O ------------> Ag + O2 You try AlBr3 ------------> Let’s Do It Together AlBr3 ------------> Al + Br2 Let’s Do It Together NaI -------------> You try NaI -------------> Na + I2 Let’s Do It Together AlCl3 -------------> Let’s Do It Together AlCl3 -------------> Al + Cl2  IF YOU SEE A SINGLE ELEMENT AND A CHEMICAL COMPOUND, IT’S A SINGLE DISPLACEMENT REACTION Your product, in this case, will be another element (usually the cation of the initial ionic compound) and an ionic compound in which the cation is the former lone element. Ca + 2 NaOH → Ca(OH) 2 + 2 Na This reaction will only take place if the pure element on the left is higher on the activity series than the one that’s already in the chemical compound. (The activity series is on the back of the periodic table). Example F2 + ZnBr2 ----------> Example F2 + ZnBr2 ----------> ZnF2 + Br2 Let’s Do It Together Sr + CrP ----------> Let’s Do It Together Sr + CrP ----------> Sr3P2 + Cr You try NiO + Li ----------> Let’s Do It Together NiO + Li ----------> Li2O + Ni You try Na + MgCl2 ----------> You try Na + MgCl2 ----------> NaCl + Mg Let’s Do It Together Zn + H2SO4----------> Let’s Do It Together Zn + H2SO4----------> ZnSO4 + H2 Let’s Do It Together Ca3(PO4)2 + K ----------> Let’s Do It Together Ca3(PO4)2 + K ----------> K3PO4 + Ca You try Al + Zn3(PO4)2 ---------->  Let’s Do It Together Al + Zn3(PO4)2 ----------> AlPO4 + Zn You try Al + Pb(NO3)2---------->  You try Al + Pb(NO3)2----------> Al(NO3)3 + Pb  IF YOU SEE TWO IONIC COMPOUNDS, SWITCH THE CATIONS TO MAKE TWO NEW IONIC COMPOUNDS IN A DOUBLE DISPLACEMENT REACTION Important notes: Both compounds need to be valid Only one of the three compounds can be soluble in water or the reaction either won’t proceed or it will make a big mess. 3 ZnCl 2(aq) + 2 H 3PO 4(aq) → Zn 3(PO 4) 2(s) + 6 HCl (aq) Note: Seriously, only one of these compounds can be soluble in water, or things won’t work out in an acceptable way! Example KI (aq) + AgNO3 (aq) ----------> Example KI (aq) + AgNO3 (aq) ----------> KNO3 + AgI Let’s Do It Together Na2S (aq) + NiSO4 (aq) ----------> Let’s Do It Together Na2S (aq) + NiSO4 (aq) ----------> Na2SO4 + NiS You try Al(NO3)3 (aq) + Na3PO4 (aq) ----------> Let’s Do It Together Al(NO3)3 (aq) + Na3PO4 (aq) ----------> AlPO4 + NaNO3 You try AlCl3 (aq) + Ca(NO3)2 (aq) ----------> You try AlCl3 (aq) + Ca(NO3)2 (aq) ----------> Al(NO3)3 + CaCl2 You try (NH4)3PO4 (aq) + Na2SO4 (aq) ----------> Let’s Do It Together (NH4)3PO4 (aq) + Na2SO4 (aq) ----------> Na3PO4 + (NH4)2SO4 IF AN ACID AND A BASE REACT, IT’S AN ACID-BASE REACTION AND THE Note: The formula of the salt must be valid! PRODUCTS WILL BE WATER AND HNO 3(aq) + KOH (aq) → KNO 3(aq) + H 2O (l) A SALT Extra note: This reaction can always be assumed to occur. You try NaOH + HClO4 ----------> You try NaOH + HClO4 ----------> NaClO4 + H2O You try ----------> HCl + Mg(OH)2 You try ----------> MgCl2 + H2O HCl + Mg(OH)2  IF THE REAGENTS CONTAIN SOMETHING WITH CARBON AND HYDROGEN, AS WELL AS OXYGEN, IT’S A C 2H 2 + O 2 → CO 2 + H 2O COMBUSTI The products are ALWAYS carbon dioxide and water in a combustion ON reaction, and this reaction always REACTION proceeds with the addition of energy! Write the product of the combustion reaction: CH4 + O2 -------> Write the product of the combustion reaction: C2H6 + O2 -----------> Write the product of the combustion reaction: C6H12O6 + O2 ------------> Write the product of the combustion reaction: C2 H5 OH + O2 -----------> AND THAT’S THAT. Let’s do some practice stuff. Nitrogen + hydrogen —> Balanced equation: Reaction type: Nitrogen + hydrogen —> N2 + H2 —> NH3 Synthesis Calcium + Silver Chloride —> Balanced equation: Reaction type: Calcium + Silver Chloride —> Ca + 2AgCl —> CaCl2 + 2Ag Single replacement/displacement Copper (II) Oxide —> Balanced equation: Reaction type: Copper (II) Oxide —> 2 CuO —> 2Cu + O2 Decomposition Butane (C4H1o) + oxygen —> Balanced equation: Reaction type: Butane + oxygen —> C4H10 + O2 —> 8 CO2 + 10 H2O Combustion Calcium chloride + potassium carbonate —> Balanced equation: Reaction type: Calcium chloride + potassium carbonate —> CaCl2 + K2CO3 —> CaCO3 + 2KCl Double displacement/replacement Net Ionic Equations Chemical Equations Chemical equations represent chemical changes. These changes are the result of a rearrangement of atoms into new combinations. Any representation of a chemical change must contain equal numbers of atoms of every element before and after the change occurred. Equations demonstrate that mass is conserved in chemical reactions. Law of Conservation of Mass A balanced equations follow the law of conservation of matter/mass that states that in any chemical or physical reaction no matter can be created or destroyed. (Everything on the left side of the equation has to equal the right) Coefficients are used to change the number of each particle in the reaction. The subscripts are NEVER changed to balance a chemical equation. States of Matter We can include the states of matter in the equation to provide more information. In a physical reaction, only the states of matter change. aq = aqueous, g = gas, l = liquid, s = solid definitions 3 different ways to write a balanced equation for a precipitation reaction: molecular equation – each reactant and product is written as a neutral compound total ionic equation or complete ionic equation– any substance that ionizes completely is broken up into separate ions; any substance that does not ionize (or is only partially ionized) is written as a neutral compound spectator ions – ions that appear in identical forms on both sides of a complete ionic equation. They don’t participate in the reaction net ionic equation – the balanced equation that describes the actual reaction that occurs in aqueous solution; it is obtained after the spectator ions are eliminated from the complete ionic equation Different Types of Balanced Equations ELECTROLYTES VS NONELECTROLYTES What are Electrolytes? An electrolyte is a substance that dissociates in water into charged particles called ions. ELECTROLYTES VS NONELECTROLYTES Distilled water, H2O, is an example of a nonelectrolyte. It is a covalent molecular substance that consists of neutral molecules. The absence of charged particles explains why a sample of pure H2O does not conduct electricity.  ELECTROLYTES VS NONELECTROLYTES Saltwater, NaCl(aq), is an example of an electrolyte. NaCl is an ionic substance. When NaCl dissolves in water, the Na+ and Cl– ions break away from the solid crystal lattice. A solution of NaCl(aq) contains positive and negative ions that can move freely throughout the solution. The movement of ions allows electricity to flow through the solution. Practice problems (b) A sample of solid crystals of sodium chloride, NaCl(s), does not conduct electricity. Practice problems (c) A sample of molten (i.e., melted) sodium chloride, NaCl(l), does conduct electricity. Practice problems (d) A sample of aqueous sucrose, C12H22O11(aq), does not conduct electricity. Practice problems (e) A sample of aqueous methanol, CH3OH(aq), does not conduct electricity. Practice problems (f) A sample of aqueous potassium hydroxide, KOH(aq), does conduct electricity. Monatomic iONS Polyatomic Ions Don’t Forget “Have no fear of ice cold beer” When a word problem says oxygen it means O2! The atoms that are diatomic in their natural state are: Bromine, Br2 Iodine, I2 Nitrogen, N2 Chlorine, Cl2 Hydrogen, H2 Oxygen, O2 Fluorine, F2 Each of the following solutes can be dissolved in water to form an aqueous solution. Write a balanced chemical equation that represents what happens to the solute particles when the solute is dissolved in water. Each of the following solutes can be dissolved in water to form an aqueous solution. Write a balanced chemical equation that represents what happens to the solute particles when the solute is dissolved in water. Students were asked to write an equation that represents what happens to the solute particles when solid calcium nitrate, Ca(NO3)2, is dissolved in water. Give a reason to explain why each of the following responses is incorrect. Students were asked to write an equation that represents what happens to the solute particles when solid calcium nitrate, Ca(NO3)2, is dissolved in water. Give a reason to explain why each of the following responses is incorrect. Precipitation (double replacement) REACTION A precipitation reaction occurs when two different aqueous solutions containing ions are combined, resulting in the formation of an insoluble (or slightly soluble) solid ionic compound. The solid product is called the precipitate. Solubility Rules…”SNAP” RULE Precipitation reactions frequently involve mixing ions in aqueous solution to produce an insoluble or sparingly soluble ionic compound. All sodium (Na+), nitrate (NO3–), ammonium (NH4+), and potassium (K+) salts are soluble in water. One way to remember these four soluble ions is to think of them as the “SNAP” ions. (S = sodium, N = nitrate, A = ammonium, and P = potassium) Group 1 metals* (Li+, Na+, etc) Balancing Equations Example: C3H8 + O2 → CO2 + H2O Example: C3H8 + 5 O2 → 3 CO2 + 4 H2O Total Ionic EQUATIONS Total ionic equations show how ionic compounds dissociate into their ions when they dissolve in water. If you have solutions (look for (aq)) of an ionic compound (particularly any sodium, potassium, ammonium, and nitrate salts) they should be written as their ions. Total (or Overall) Ionic Net Ionic Equations The net ionic equation only shows the particles that change in the reaction. It cancels out the spectator ions. A spectator ion is one that isn’t involved in the reaction and stays the same phase throughout. In the example below, the sodium ions and the nitrate ions are the same phase throughout the reaction and are unchanged, they should be cancelled out to create a net ionic equation. Net Ionic Equations Together Together (NH4)2CO3(aq) +2 AgNO3(aq) → Ag2CO3 (s) + 2 NH4NO3(aq) 2NH4+(aq) + CO32-(aq) +2 Ag+(aq) +2NO3-(aq)→ Ag2CO3(s) + 2NH4+(aq) +2NO3-(aq) 2 NH4+(aq) +2 NO3-(aq) CO32-(aq) +2 Ag+(aq) → Ag CO3(s) 2 You Do, We Review You Do, We Review The reaction of potassium chloride and lead II nitrate Balanced Equation: Total Ionic Equation: Spectator Ions: Net Ionic Equation: The reaction of potassium chloride and lead II nitrate Molecular Equation: 2KCl (aq) + Pb(NO3)2 (aq) -> 2KNO3 (aq) + PbCl2 (s) Complete Ionic Equation: 2K+ (aq) + 2Cl- (aq) + Pb2+ (aq) + 2NO3– (aq) -> 2K+ (aq) + 2NO3– (aq) + PbCl2 (s) Net Ionic Equation: 2Cl- (aq) + Pb2+ (aq) -> PbCl2 (s) The reaction of Potassium chromate and calcium chloride Balanced Equation: Total Ionic Equation: Spectator Ions: Net Ionic Equation: The reaction of Potassium chromate and calcium chloride Balanced Equation: K2(CrO4)(aq) + CaCl2(aq) → 2KCl(aq) + Ca(CrO4)(aq) Total Ionic Equation: 2K+ (aq) + C2O4 2- (aq) + Ca2+(aq)+ 2Cl- (aq) → 2K+ (aq) + 2Cl- (aq) + Ca2+ + C2O4 2- Spectator Ions: All Net Ionic Equation: NA The reaction of Sodium phosphate & nickel II perchlorate Balanced Equation: Total Ionic Equation: Spectator Ions: Net Ionic Equation: The reaction of Sodium phosphate & nickel II perchlorate Balanced Equation: 2Na3PO4(aq) + 3Ni(ClO4)2(aq) → 6NaClO4(aq) + Ni3(PO4)2(s) Total Ionic Equation: Ionic Equation: 6Na+ (aq) 2PO4 3- (aq) + 3Ni2+(aq) + 6ClO4 - (aq) → 6Na+ (aq) + 6ClO4 - (aq) + Ni3(PO4)2(s) Spectator Ions: Net Ionic Equation: 2PO4 3- (aq) + 3Ni2+(aq) → Ni3(PO4)2(s) The reaction of Potassium fluoride and magnesium nitrate Balanced Equation: Total Ionic Equation: Spectator Ions: Net Ionic Equation: The reaction of Potassium fluoride and magnesium nitrate Balanced Equation: 2KF(aq) + Mg(NO3)2(aq) → 2KNO3(aq) + MgF2(s) Total Ionic Equation: 2K+ (aq) + 2F- (aq) + Mg2+(aq) + 2NO3 - (aq) → 2K+ (aq) + 2NO3 - (aq) + MgF2(s) Spectator Ions: Net Ionic Equation: 2F- (aq) + Mg2+(aq) → MgF2(s) The reaction of Ammonium chromate and aluminum perchlorate Balanced Equation: Total Ionic Equation: Spectator Ions: Net Ionic Equation: The reaction of Ammonium chromate and aluminum perchlorate Balanced Equation: 3(NH4)2CrO4(aq) + 2Al(ClO4)3(aq) → Al2(CrO4)3(s) + 6NH4ClO4(aq) Total Ionic Equation: 6NH4 + (aq) + 3CrO4 2- (aq) + 2Al3+(aq) + 6ClO4 - (aq) → 6NH4 + (aq) + 6ClO4 - (aq) + Al2(CrO4)3(s) Spectator Ions: Net Ionic Equation: 3C2O4 2- (aq) + 2Al3+(aq) → Al2(CrO4)3(s) Reaction Rates  Collision THEORY Collision theory states that in order for a reaction to take place the following things must occur: 1. Particles must collide. 2. They must have sufficient energy. 3. The particles must be in the correct orientation. (Certain parts on one molecule and certain parts on another molecule must meet in order for the reaction to occur) Orientation Even when molecules collide with sufficient energy, activation energy or above, a successful collision is not guaranteed. In most reactions, molecules must be oriented in a certain way during collision for a reaction to occur. Collision Theory Surface Area  Reactant Concentrations Pressure Temperature Catalysts Together  Together Small chips, 0.0050M, and ice bath Powdered, 0.50M, warm water bath