2 Chemical Reaction Another name for a chemical change New properties when you are doneNo new atoms are madeAtoms are rearrangedNew compounds can be madeOld bonds are brokenNew bonds are formed
3 Indications of Chemical Reactions New propertiesColor changeOdor changeNew phase is madePrecipitates- solids in a liquidGases- bubbles in a liquidTwo parts of reactionReactants- the stuff you start withProducts- the stuff you make
4 Starting a Reaction Always takes a little energy Energy goes into breaking bonds in the reactantsCan use different forms of energyHeatElectricityLight
5 Forming Bonds Makes Energy Releases energyEnergy is conservedChemical Energy- energy stored in the bonds of the chemicals.Reactions have an energy change
6 Exothermic ReactionsIf breaking bonds takes less energy than making them- it releases energyExo- outsidetherm- heatExothermic reactions release energyGet hotGive off lightOr release electricity
7 Change is downChemical EnergyEnergy ReleasedReactantsProducts
8 Endothermic Reactions If breaking bonds takes more energy than making them- it absorbs energyEndo- insidetherm- heatEndothermic reactions absorb energyGet coldRequire heat or energy or they stop
9 Change is upHeat is releasedChemical EnergyReactantsProducts
10 Chemical EquationsCopper reacts with chlorine to form copper (II) chloride.In a word equationMethane + oxygen ® water +carbon dioxideArrow means “yields” or “makes”The plus sign means “and”Can use formulasCH4 +O2 ® CO2 +H2O
11 Balanced Equation Atoms can’t be created or destroyed All the atoms we start with we must end up withA balanced equation has the same number of each element on both sides of the equation.
12 ® O + C O C O O C + O2 ® CO2 This equation is already balanced What if it isn’t already?
13 ® O + C C O O C + O2 ® CO We need one more oxygen in the products. Can’t change the formula, because it describes what is
14 CCOO+OCCOMust have started with two C2 C + O2 ® 2 CO
15 Rules for balancingWrite the correct formulas for all the reactants and productsCount the number of atoms of each type appearing on both sidesBalance the elements one at a time by adding coefficients (the numbers in front)Check to make sure it is balanced.
16 Never Change a subscript to balance an equation. If you change the formula you are describing a different reaction.H2O is a different compound than H2O2Never put a coefficient in the middle of a formula2 NaCl is okay, Na2Cl is not.
17 ExampleH2 +O2H2OMake a table to keep track of where youare at
18 ExampleH2 +O2H2ORP2H22O1Need twice as much O in the product
27 Moles and Reactions 2H2 + O2 ® 2H2O 2 dozen molecules of hydrogen and 1 dozen molecules of oxygen form 2 dozen molecules of water.2 x (6.02 x 1023) molecules of hydrogen and 1 x (6.02 x 1023) molecules of oxygen form 2 x (6.02 x 1023) molecules of water.2 moles of hydrogen and 1 mole of oxygen form 2 moles of water.
28 Moles and ReactionsThe coefficients of balanced equations tell how many particles reactAnd how many moles of particlesWe can make ratios with those moles2 Mg + O2 2 MgOIf 2 moles of Mg react, 1 mole of O2 will be required2 mol Mg or 1 mol O2 1 mol O mol Mg
29 Mole ratiosCan be used to figure out how many moles of products and reactants were used or made2H2 + O2 ® 2H2OIf 6 mole of H2 react, how many moles of water will form?How many moles of hydrogen are needed to react with 3.6 mole of oxygen?
30 Mole to mole conversions 2 Al2O3 ® 4Al + 3O2every time we use 2 moles of Al2O3 we make 3 moles of O22 moles Al2O33 mole O2or3 mole O22 moles Al2O3
31 Mole to Mole conversions How many moles of O2 are produced when 3.34 moles of Al2O3 decompose?2 Al2O3 ® 4Al + 3O23.34 moles Al2O33 mole O2=5.01 moles O22 moles Al2O3
32 Your Turn2C2H2 + 5 O2 ® 4CO2 + 2 H2OIf 3.84 moles of C2H2 are burned, how many moles of O2 are needed?How many moles of C2H2 are needed to produce 8.95 mole of H2O?If 2.47 moles of C2H2 are burned, how many moles of CO2 are formed?
33 Collision TheoryIn order to react molecules and atoms must touch each other.They must hit each other hard enough to react.Anything that increase these things will make the reaction faster.
34 Things that Affect Rate TemperatureHigher temperature faster particles.More and harder collisions.Faster Reactions.ConcentrationMore concentrated closer together the molecules.Collide more often.Faster reaction.
35 Things that Affect Rate Particle sizeMolecules can only collide at the surface.Smaller particles bigger surface area.Smaller particles faster reaction.Smallest possible is molecules or ions.Dissolving speeds up reactions.Getting two solids to react with each other is slow.
36 Things that Affect Rate Catalysts- substances that speed up a reaction without being used up.Inhibitor- a substance that blocks a catalyst, slowing the reaction downEnzymes are biological catalysts- made by plants and animals to control reactionsHeat destroys most catalysts
37 Reactions Some go to completion All the reactants get turned into productsNo reactants leftSome reactions go both directionsThey are called reversible reactions
38 Reversible Reactions 2H2(g) + O2(g) ® 2H2O(g) + energy 2H2O(g) + energy ® 2H2(g) + O2(g)2H2(g) + O2(g) H2O(g) + energy
39 EquilibriumWhen I first put reactants together the forward reaction starts.Since there are no products there is no reverse reaction.As the forward reaction proceeds the reactants are used up so the forward reaction slows.The products build up, and the reverse reaction speeds up.
40 EquilibriumEventually you reach a point where the reverse reaction is going as fast as the forward reaction.This is dynamic equilibrium.The rate of the forward reaction is equal to the rate of the reverse reaction.The concentration of products and reactants stays the same, but the reactions are still running.
41 EquilibriumEquilibrium position- how much product and reactant there are at equilibrium.Shown with the double arrow.Reactants are favoredProducts are favoredCatalysts speed up both the forward and reverse reactions so don’t affect equilibrium position.
43 LeChâtelier’s Principle If something is changed in a system at equilibrium, the system will respond to undo that change.Three types of changes are described.
44 Changing Concentration If you add reactants (or increase their concentration).The forward reaction will speed up.More product will form.Equilibrium “Shifts to the right”Reactants ® products
45 Changing Concentration If you add products (or increase their concentration).The reverse reaction will speed up.More reactant will form.Equilibrium “Shifts to the left”Reactants ¬ products
46 Changing Concentration If you remove products (or decrease their concentration).The reverse reaction will slow downMore product will form.Equilibrium reverse“Shifts to the right”Reactants ® products
47 Changing Concentration If you remove reactants (or decrease their concentration).The forward reaction will slow down.More reactant will form.Equilibrium “Shifts to the left”.Reactants ¬ productsUsed to control how much yield you get from a chemical reaction.
48 Changing Temperature Reactions either require or release heat. Endothermic reactions go faster at higher temperature.Exothermic go faster at lower temperatures.All reversible reactions will be exothermic one way and endothermic the other.
49 Changing TemperatureAs you raise the temperature the reaction proceeds in the endothermic direction.As you lower the temperature the reaction proceeds in the exothermic direction.Reactants + heat ® Products at high TReactants + heat ¬ Products at low T
50 Changes in PressureAs the pressure increases the reaction will shift in the direction of the least gases.At high pressure H2(g) + O2(g) ® 2 H2O(g)At low pressure H2(g) + O2(g) ¬ 2 H2O(g)