Chapter 3 Chemical Reactions and Equations

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1 Chapter 3 Chemical Reactions and Equations

2

3 Chemical Reactions Reactions involve rearrangement and exchange of atoms to produce new pure substances. Reactants Products Chemical Equations Shorthand way of describing a reaction Provides information about the reaction 1. formulas of reactants and products 2. states of reactants and products 3. relative numbers of reactant and product molecules

4 Types of Chemical Reactions

5 Classifying Chemical Reactions by What Atoms Do

6 Synthesis Reactions + 4 Al (s) + 3 O2 (g) 2 Al2O3 (s) 2 H2 (g) + O2 (g) > 2 H2O (g) C2H4 (g) + H2O2 (aq) C2H6O2 (l)

7 Decomposition Reactions + 2 HgO (s) > 2 Hg (l) + O2 (g) CaCO3 (s) > CaO (s) + CO2 (g) 2 NaCl (s) > Cl2 (g) + 2 Na (l)

8 Single Displacement Reactions + + Cu (s) + 2 AgNO3 (aq) > 2 Ag (s) + Cu(NO3)2 (aq) 2 Al (s) + Fe2O3 (s) > Al2O3 (s) + 2 Fe (l) Mg (s) + 2 HCl (aq) > H2 (g) + MgCl2 (aq)

9 2 AgNO3(aq) + Cu(s) 2 Ag (s) + Cu(NO3)2(aq)

10 Fe2O3 (s) + Al (s) 2 Fe (l) + Al2O3(s)

11 Double Displacement Reactions + + Ba(NO3)2 (aq) + Na2SO4 (aq) > BaSO4 (s) + 2 NaNO3 (aq) PCl3 (l) + 3 AgF (s) > PF3 (g) + 3 AgCl (s) HCl (aq) + NaOH (aq) > H2O(l) + NaCl (aq)

12 Chemical Reactions Classified by Reaction Type

13 Chapter 3 Moles and Calculations with Moles

14 Moles What is an amu? 1.66 x g We need a conversion to the macroscopic world. 1. How many hydrogen atoms are in 1.00 g of hydrogen? 1 H atom 1.00 g H x = 6.02 x H atoms 1.66 x g H Avogadro s Number

15 Moles Consider carbon-12 (the most abundant isotope of C) What is the mass of one carbon-12 atom? amu g g 12 x 1.66 x = 1.99 x C atom amu C atom What is the mass of Avogadro s number of C atoms? g 6.02 x C atoms x 1.99 x = g C atom

16 Chemical Packages - Moles Mole = number of particles equal to the number of atoms in 12 g of C-12 The number of particles in 1 mole is called Avogadro s Number = x mole of C atoms weighs g and has x atoms. The average mass of a C atom is amu.

17 1. Calculate the number of atoms in 2.45 mol of copper mol Cu atoms Cu 1 mol = x atoms x Cu atoms 1 mol Cu conversion factors 1 mol Cu x Cu atoms x Cu atoms 2.45 mol Cu x = 1.48 x 10 1 mol Cu 24 Cu atoms

18 Relationship Between Moles and Mass The mass of one mole of atoms is called the molar mass. The molar mass of an element, in grams, is numerically equal to the element s atomic mass, in amu. The lighter the atom, the less a mole weighs. The lighter the atom, the more atoms there are in 1 g.

19 Molar mass of an element The molar mass of an element, in grams, is numerically equal to the element s atomic mass, in amu.

20 2. Calculate the moles of carbon in g of carbon. g C mol C g C 1 mol C 1 mol C = g C conversion factors 1 mol C g C 1 mol C g C x g C = 2.21 x 10-3 mol C

21 3. How many copper atoms are in a 3.10 g of copper? g Cu 1 mol Cu = g Cu g Cu 1 mol Cu 1 mol Cu g Cu mol Cu conversion factors atoms Cu 1 mol Cu = x Cu atoms 1 mol Cu x Cu atoms x Cu atoms 1 mol Cu 1 mol Cu x Cu atoms 3.10 g Cu x x = 2.94 x g Cu 1 mol Cu 22 Cu atoms

22 Formula Mass The mass of an individual molecule or formula unit Also known as molecular mass or molecular weight Sum of the masses of the atoms in a single molecule or formula unit mass of 1 molecule of H2O = 2(1.01 amu H) amu O = amu mass of 1 formula unit of MgCl2 = 2(35.45 amu Cl) amu Mg = amu

23 Molar Mass of Compounds The relative masses of molecules can be calculated from atomic masses. Formula Mass of 1 molecule of H2O = 2(1.01 amu/h) amu/o = amu 1 mole of H2O contains 2 moles of H and 1 mole of O. molar mass = 1 mole H2O = 2(1.01 g H) g O = g so the Molar Mass of H2O is g/mole

24 4. How many moles are in 50.0 g of PbO2? (Pb, g/mol; O,16.00 g/mol) g PbO2 mol PbO2 Pb = 1 x = O = 2 x = g PbO2 1 mol PbO2 PbO2 = g/mol 1 mol PbO g PbO2 1 mol PbO g PbO g PbO2 x = mol PbO2

25 5. Find the number of CO2 molecules in 10.8 g of CO2. 1 mol CO2 = x molecules g CO2 mol CO2 molec CO2 C = 1 x = O = 2 x = CO2 = 44.01g/mol g CO2 1 mol CO2 1 mol CO g CO g CO2 x 1 mol CO2 x x molecules = g CO2 1 mol CO x 10 x molecules CO2

26 6. What is the mass of 4.78 x NO2 molecules? 1 mol = x 10 23,1 mol NO2 = g molec NO2 mol NO2 g NO x molec NO2 1 mol NO2 1 mol NO x molec NO g NO2 1 mol NO2 1 mol NO g NO2 1 mol NO x molec NO x molec NO2 x x g NO2 1 mol NO2 = g NO2 365 g NO2

27 Writing Balanced Chemical Equations

28 Combustion of Methane Methane gas reacts with oxygen gas to produce carbon dioxide gas and gaseous water. CH4(g) + O2(g) CO2(g) + H2O(g) This equation reads 1 molecule of CH4 gas combines with 1 molecule of O2 gas to make 1 molecule of CO2 gas and 1 molecule of H2O gas. + +

29 What about conservation of mass?? + + X 1 C + 4 H + 2 O 1 C + 2 O + 2 H + O

30 Combustion of Methane, Balanced To show the reaction obeys the Law of Conservation of Mass, the equation must be balanced. CH4(g) + O2(g) CO2(g) + H2O(g) CH4(g) + O2(g) CO2(g) + 2 H2O(g) CH4(g) + 2 O2(g) CO2(g) + 2 H2O(g) molecule of CH4 gas combines with 2 molecules of O2 gas to make 1 molecule of CO2 gas and 2 molecules of H2O gas.

31 Symbols Used in Equations Symbols used to indicate state after chemical: (g) = gas; (l) = liquid; (s) = solid (aq) = aqueous = dissolved in water Energy symbols used above the arrow for conditions for reactions: Δ = heat hν = light shock = mechanical elec = electrical

32 Steps in Balancing Equations 1. In compounds balance elements other than H and O. a. Balance elements which occur only once on each side of the equation. b. Start with the elements which occur the most. c. Balance polyatomic ions which do not change in the reaction. 2. Be prepared to rebalance if something changes!!! 3. Balance H. 4. Balance O. 5. Balance elements which appear in their elemental forms.

33 1. When aluminum metal reacts with air, it produces a white, powdery compound, aluminum oxide. aluminum(s) + oxygen(g) aluminum oxide(s) Al(s) + O2(g) Al2O3(s) 2 Al(s) + O2(g) Al2O3(s) 2 Al(s) + 3 O2(g) 2 Al2O3(s) 4 Al(s) + 3 O2(g) 2 Al2O3(s)

34 2. Solid phosphorous (P4) reacts with hydrogen gas to produce phosphorous trihydride. P4 (s) + H2 (g) > PH3 (g) P4 (s) + H2 (g) > 4 PH3 (g) P4 (s) + 6 H2 (g) > 4 PH3 (g)

35 3. Solid potassium chlorate decomposes to produce oxygen gas and potassium chloride. KClO3 (s) > O2 (g) + KCl (s) 2 KClO3 (s) > 3 O2 (g) + KCl (s) 2 KClO3 (s) > 3 O2 (g) + 2 KCl (s)

36 4. Aqueous sulfuric acid reacts with solid sodium cyanide to produce aqueous sodium sulfate and hydrogen cyanide gas. H2SO4 (aq) + NaCN (s) > Na2SO4 (aq) + HCN(g) H2SO4 (aq) + 2 NaCN (s) > Na2SO4 (aq) + HCN(g) H2SO4 (aq) + 2 NaCN (s) > Na2SO4 (aq) + 2 HCN(g)

37 5. Aqueous potassium phosphate reacts with aqueous calcium nitrate to produce solid calcium phosphate and aqueous potassium nitrate. K3PO4 (aq) + Ca(NO3)2 (aq) > Ca3(PO4)2 (s) + KNO3 (aq) K3PO4 (aq) + 3 Ca(NO3)2 (aq) > Ca3(PO4)2 (s) + KNO3 (aq) K3PO4 (aq) + 3 Ca(NO3)2 (aq) > Ca3(PO4)2 (s) + 6 KNO3 (aq) 2 K3PO4 (aq) + 3 Ca(NO3)2 (aq) > Ca3(PO4)2 (s) + 6 KNO3 (aq)

38 Acetic acid reacts with the metal aluminum to make aqueous aluminum acetate and gaseous hydrogen Al(s) + HC2H3O2(aq) Al(C2H3O2)3(aq) + H2(g) Al(s) + 3 HC2H3O2(aq) Al(C2H3O2)3(aq) + H2(g) Al(s) + 6 HC2H3O2(aq) Al(C2H3O2)3(aq) + 3 H2(g) Al(s) + 6 HC2H3O2(aq) 2 Al(C2H3O2)3(aq) + 3 H2(g) 2 Al(s) + 6 HC2H3O2(aq) 2 Al(C2H3O2)3(aq) + 3 H2(g)

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