Chemical Reactions. Chapter 17
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1 Chemical Reactions Chapter 17
2 Chemical Equations C+O 2 CO 2 C (s) +O 2 (g) CO 2 (g) Reactants on left, products on right Each are balanced because same number of atoms of reactants as products Some equations show the phase of the substances also: solid, liquid, gas
3 Balancing Chemical Equations Molecules of reactants and products shown Cannot change the molecule Can change how many of them Cannot add or delete reactants or products Balanced equal number of same atoms on each side
4 Water balancing
5 Balancing Tips Never change the molecular formula of reactants or products Count atoms in reactant and products Always add whole molecules, not parts Start by balancing atoms in compounds Save element reactants or products for last to make up any imbalance
6 Rusting of Iron Fe + O 2 Fe 2 O 3 start with oxygen not balanced Fe + 3 O 2 2 Fe 2 O 3 next do iron 4 Fe + 3 O 2 2 Fe 2 O 3
7 Problem 1 in class Balance the following equation, on the worksheet provided. (Put your name on the back of the sheet, please.) N 2 + H 2 NH 3
8 Combustion of propane C 3 H 8 + O 2 CO 2 + H 2 O fix hydrogen first it s in two compounds C 3 H 8 + O 2 CO H 2 O need more carbon product C 3 H 8 + O 2 3 CO H 2 O Do oxygen last, because it is single C 3 H O 2 3 CO H 2 O
9 Problem 2 in class Balance the following chemical equation, the combustion of methane CH 4 + O 2 CO 2 + H 2 O Methane oxygen carbon dioxide water
10 Volume Relationships Equal volumes of gases at the same temperature and pressure have the same number of molecules Gases react in small whole number quantities Avogadro s hypothesis: chemicals react in consistent, small whole number ratios
11 Avogadro s hypothesis
12 Combustion of propane C 3 H O 2 3 CO H 2 O What volume of oxygen is needed to burn 0.5 L of propane? Ratio of Oxygen molecules to propane molecules is 5:1 0.5 L x 5 L O 2 = 2.5 L Oxygen 1 L Propane
13 Problem 3 in class Combustion of propane C 3 H O 2 3 CO H 2 O Calculate how much CO 2 is produced when 2 L of propane is burned
14 Atomic vs. Molecular Weight Atomic weight on periodic table is average of natural abundance of isotopes Atomic mass is the number of nucleons in a particular atom specified by isotope Molecular mass is the mass of one mole of molecules One atomic mass number of grams x10 23 molecules
15 Calculate Molecular Mass O atomic weight (round to 16 for this class) O-16 atomic mass 16 u Molecular oxygen O 2 atomic mass 32 u Molecular O 2 molecular mass 32 g/mole CO 2 molecular mass C=12 g/mole, O 2 =32 g/mole CO 2 =12+32=44 g/mole
16 Problem 4 in class Calculate the molar mass of propane C 3 H 8 Round atomic weight of C to 12 g mole Round atomic weight of H to 1 g mole
17 Grams calculated from Moles Can find the molar mass of substance g 1 mole 4 Na=23 mole of Na Multiply molar mass times moles g 23 mole x moles = 5.75 g
18 Moles calculated from Grams 176 g of CO 2 = Number of moles? Molar mass of CO 2 = 44 If you multiply, g mole 176 g x 44 results in units of you get a unit mess g mole UNITS alert you that you made an error KEEP UNITS WITH NUMBERS!! g 2 mole
19 Moles calculated from Grams 176 g of CO 2 = Number of moles? Molar mass of CO 2 = 44 Divide 176 g by 44 g mole g mole Same as multiply by reciprocal 176 g x ( 1 mole 44 g ) = 4 moles CO 2 Now the grams cancel =)
20 Problem 5 in class 132 g of propane is how many moles?
21 Mass to moles relationship
22 To convert between grams and moles Make sure equation is balanced So you know the molar ratios of them Find molar mass of them Set up proportions for moles and grams
23 Proportions Mathematical device to compare ratios Cross-multiply to solve Correctly organized Be sure you keep same:same in columns and rows
24 Proportions to find grams and moles Correctly organized Example or moles moles moles g of of a of of cross-multiply to solve a a b = = g g of of a b moles g of of b b
25 Proportions Correctly organized It doesn t matter how you write the first ratio, as long as you label the numbers Try to put unknown on the top easier to solve The second ratio needs to match the first
26 Problem NO + O NO grams O 2 How many grams NO 2 produced? First: Balance Equation 2NO + O NO 2 2 2
27 Problem 2NO + O NO grams O 2 How many grams NO 2 produced? Balance Equation Determine molar ratios of them 1:2 Find molar mass of each component NO 2 =46 g, O 2 =32 g, (NO=30 g)
28 Problem 2NO + O NO grams O 2 How many grams NO 2 produced? Molar mass of each: O 2 =32 g, NO 2 =46 g How many moles is 64 grams O 2? One mole
29 Problem 2NO + O NO grams O 2 How many grams NO 2 produced? Molar mass of each O 2 =32 g, NO 2 =46 g Molar ratios O2:NO2 is 1:2 Two mole of O 2 So four moles of NO 2 is produced How many grams is that? 4 mol x 46 g/mol = 184 grams
30 Problem H S + O SO + H O grams SO 2 How many grams O 2 used?
31 Problem 32 grams SO 2 How many grams O 2 used? H S + O SO + H O Balance first 2 H S + 3O 2SO + 2H O Then determine molar ratios 2 SO 2 to 3 O 2
32 Problem 32 grams SO 2 How many grams O 2 used? 2 H S + 3O 2SO + 2H O Find molar masses SO 2 = = 64 g/mol SO 2 O 2 = (2x1) +16 = 32 g/mol O 2 H 2 O= (2x1) +16 = H 2 S = (2x1) +32 = 18 g/mol H 2 O 34 g/mol H 2 S
33 Problem 32 grams SO 2 How many grams O 2 used? 2 H S + 3O 2SO + 2H O g SO 2 needs how many grams O 2? How many moles is 32 g SO 2? 1mole 32 g SO = 0.5 moles 64 g 2 SO 2
34 Problem 32 grams SO 2 How many grams O 2 used? 2 H S + 3O 2SO + 2H O How many moles O 2 is needed? 0.5 moles SO 2 in 2:3 ratio with O moles O 2 1mole 32 g SO = 0.5 moles 64 g 2 SO 2
35 Set up proportion 32 grams SO 2 How many grams O 2 used? with the unknown on top (the O 2 )? g O 2 = [ ] [ ] [ ]
36 Problem 6 C + O CO 2 2 Is it balanced? Molar ratio 1:1:1 4 grams oxygen Grams carbon consumed? Grams carbon dioxide produced?
37 Reaction Speed Collision of molecules required for it to occur Increase concentration Increase temperature Catalyst can facilitate reaction
38 Chlorine catalyst
39 Energy of reactions Release energy EXOTHERMIC Methane combustion Consume energy ENDOTHERMIC Formation of water
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