Chemical Reactions Worksheets

Transcription

1 Germanium 32 Ge Nickel 28 Ni Uranium 92 U Sulfur 16 S Worksheets

2 Reactions and Equations Chemical reactions take place when the bonds between atoms are broken and new bonds are formed, creating a new arrangement of atoms and at least one new substance. Evidence of chemical reaction 1) Heat change Heat change is an evidence of chemical reaction. Temperatures may rise during chemical reactions as a wood burning reaction and the temperature may be decrease in other chemical reactions. 2) Color Change The color changing of iron nails is an example for the chemical reactions between iron and oxygen, and the transformation of banana from green to yellow color is another example. 3) Odor and gas bubbles Gas bubbles are an example of chemical reaction. when baking powder is placed on vinegar hydrogen gas bubbles is formed. 4) Formation of a solid A solid precipitate may be formed during the reaction of liquid substances, which is also a evidence of chemical reaction. pg. 1

3 Representing Chemical reactions We use chemical equations to express chemical reactions A + B C + D Reactants Products Symbols used in Chemical Equations Symbol + (s) (l) (g) (aq) Purpose Separate two or more reactants or products Separates reactants from products Separates reactants from products and indicates a reversible reaction Identifies a solid state Identifies a liquid state Identifies a gaseous state Identifies a water solution The substances undergoing reaction are called reactants, and their formulas are placed on the left side of the equation. The substances generated by the reaction are called products, and their formulas are placed on the right side of the equation. Word equation We can describe the reaction between Aluminum and Bromine by a word equation Aluminum(s) + Bromine(l) Aluminum bromide(s) Word equation: Aluminum and Bromine react to produce aluminum Bromide. Skelton equation It uses chemical formulas rather than words to identify the reactants and the products. The Skelton equation for the pervious reaction, Al(s) + Br 2 (l) AlBr 3 (s) pg. 2

4 Covert the following word equations to skeleton equations. Be sure to include to state of matter that each compound as a subscript. Example: Silver nitrate + copper silver + copper nitrate Solution: AgNO 3 (aq) + Cu(s) Ag(s) + Cu(NO 3 ) 2 (aq) 1) Iron + Sulphur Iron(II) sulphide (All solids) 2) Hydrogen + chlorine hydrogen chloride (all gases) 3) Magnesium + oxygen magnesium oxide (last one is a solid) 4) Aluminum oxide aluminum + oxygen (Starts with a solid) 5) Water Hydrogen + oxygen (obvious states) 6) Hydrochloric acid + sodium hydroxide sodium chloride + water (mixing two solutions to make a solid and liquid) 7) Methane + oxygen carbon dioxide + water (obvious states) 8) Potassium hydroxide + hydrogen bromide potassium bromide + water (solid and gas make solid and liquid) 9) Carbon + oxygen carbon dioxide (obvious states) 10) Tin (II) oxide + hydrogen tin + water (starts with a solid) 11) Propane (tricarbon octahydride) + oxygen carbon dioxide + water (obvious states) 12) Sodium hydroxide + phosphoric acid (Hydrogen phosphate) Sodium phosphate + water. (starts with solutions and makes a solution and a liquid) pg. 3

5 13) Calcium bicarbonate calcium carbonate + carbon dioxide + water (solid makes a solid and two gases) 14) potassium + water potassium hydroxide + hydrogen (obvious reactants forming a solution and a gas) 15) Lead(II) nitrate + potassium sulfide potassium nitrate + lead(ii) sulfide (two solutions forming a precipitate and a solution) Law of conservation of mass Unfortunately, it is also an incomplete chemical equation. The law of conservation of matter says that matter cannot be created or destroyed. In chemical equations, the number of atoms of each element in the reactants must be the same as the number of atoms of each element in the products. Chemical equation: statement that uses chemical formulas to show the identities and relative amounts of the substances involved in a chemical reaction. In normal chemical processes, we cannot create or destroy matter (law of conservation of mass). If we start out with ten carbon atoms, we need to end up with ten carbon atoms. pg. 4

6 Balancing chemical equations To balance the chemical equations, we have to find the appropriate coefficients. Coefficient: The number that is written before the reactant or products in the chemical equation. Coefficients are always integers. Do not write coefficients if their value is equal to 1 The coefficients describe the simplest numerical ratios of the quantities of the reactants and products. Steps for balancing equations Write and balance the chemical equation for each given chemical reaction Hydrogen and chlorine react to make HCl Steps for balancing equations step process Let us start by simply writing a chemical equation in terms of the formulas of the substances, remembering that both elemental hydrogen and chlorine are diatomic Count the atoms There are two hydrogen atoms and two chlorine atoms in the reactants and one of each atom in the product. Change the coefficient We can fix this by including the coefficient 2 on the product side Now there are two hydrogen atoms and two chlorine atoms on both sides of the chemical equation, so it is balanced Example H 2 + Cl 2 HCl H 2 + Cl 2 HCl H 2 + Cl 2 2HCl pg. 5

7 Fill in the blanks with the most appropriate term: 16) A tells the story of a chemical reaction. are the starting substances in the reaction while are the new substances that are formed. The large numbers in front of some of the formulas are called. These numbers are used to the equation because chemical reactions must obey the Law of of Matter. The number of atoms of each element on both sides of the equation must be because matter cannot be or. When balancing equations, the only numbers that can be changed are ; remember that must never be changed in order to balance an equation. Balance the following equations: 17) Al + O 2 Al 2 O 3 18) C 3 H 8 + O 2 CO 2 + H 2 O 19) Al(NO 3 ) 3 + NaOH Al(OH) 3 + NaNO 3 20) KNO 3 KNO 2 + O 2 21) O 2 + CS 2 CO 2 + SO 2 22) KClO 3 KCl + O 2 23) BaF 2 + K 3 PO 4 Ba 3 (PO 4 ) 2 + KF pg. 6

8 24) H 2 SO 4 + Mg(NO 3 ) 2 MgSO 4 + HNO 3 25) Al + H 2 SO 4 Al 2 (SO 4 ) 3 + H 2 26) WO 3 + H 2 W + H 2 O 27) NaNO 3 + PbO Pb(NO 3 ) 2 + Na 2 O 28) AgI + Fe 2 (CO 3 ) 3 FeI 3 + Ag 2 CO 3 29) C 2 H 4 O 2 + O 2 CO 2 + H 2 O 30) ZnSO 4 + Li 2 CO 3 ZnCO 3 + Li 2 SO 4 31) V 2 O 5 + CaS CaO + V 2 S 5 32) Mn(NO 2 ) 2 + BeCl 2 Be(NO 2 ) 2 + MnCl 2 33) AgBr + GaPO 4 Ag 3 PO 4 + GaBr 3 34) H 2 SO 4 + B(OH) 3 B 2 (SO 4 ) 3 + H 2 O 35) S 8 + O 2 SO 2 36) Fe + AgNO 3 Fe(NO 3 ) 2 + Ag 37) H 3 PO 4 + KOH K 3 PO 4 + H 2 O 38) K + B 2 O 3 K 2 O + B 39) HCl + NaOH NaCl + H 2 O 40) Na + NaNO 3 Na 2 O + N 2 41) C + S 8 CS 2 42) Na + O 2 Na 2 O 43) N 2 + O 2 N 2 O 5 44) H 3 PO 4 + Mg(OH) 2 Mg 3 (PO 4 ) 2 + H 2 O 45) NaOH + H 2 CO 3 Na 2 CO 3 + H 2 O 46) KOH + HBr KBr + H 2 O pg. 7

9 47) Na + O 2 Na 2 O 48) Al + S 8 Al 2 S 3 49) Cs + N 2 Cs 3 N 50) Mg + Cl 2 MgCl 2 51) Rb + RbNO 3 Rb 2 O + N 2 52) C 6 H 6 + O 2 CO 2 + H 2 O 53) N 2 + H 2 NH 3 54) C 10 H 22 + O 2 CO 2 + H 2 O 55) C 3 H 8 + O 2 CO 2 + H 2 O 56) Li + AlCl 3 LiCl + Al 57) C 2 H 6 + O 2 CO 2 + H 2 O 58) Rb + P Rb 3 P 59) CH 4 + O 2 CO 2 + H 2 O 60) Na + Cl 2 NaCl 61) Rb + S 8 Rb 2 S 62) NH 3 + HCl NH 4 Cl 63) Li + H 2 O LiOH + H 2 64) NH 3 + O 2 N 2 + H 2 O 65) FeS 2 + O 2 Fe 2 O 3 + SO 2 66) C + SO 2 CS 2 + CO pg. 8

10 Synthesis reaction Classifying chemical reactions A Synthesis reaction is a reaction in which two or more substances combine to form a single new substance. The general form of a Synthesis reaction is: A+B AB One Synthesis reaction is two elements combining to form a compound. Solid sodium metal reacts with chlorine gas to produce solid sodium chloride. 2Na(s)+Cl 2 (g) 2NaCl(s) Synthesis reactions can also take place when an element reacts with a compound to form a new compound composed of a larger number of atoms. Carbon monoxide reacts with oxygen to form carbon dioxide according to the equation: 2CO(g)+O 2 (g) 2CO 2 (g) Two compounds may also react to from a more complex compound. A very common example is the reactions of oxides with water. Calcium oxide reacts readily with water to produce an aqueous solution of calcium hydroxide. CaO(s)+H 2 O(l) Ca(OH) 2 (aq) Complete the following word equations, and write and balance the formula equation. 67) calcium + oxygen 68) copper + sulfur copper(ii) sulfide 69) calcium oxide + water calcium hydroxide 70) hydrogen + nitrogen 71) hydrogen + chlorine 72) silver + sulfur pg. 9

11 73) chromium + oxygen 74) aluminum + bromine 75) sodium + iodine 76) hydrogen + oxygen 77) aluminum + oxygen pg. 10

12 Combustion Reactions A combustion reaction is a reaction in which a substance reacts with oxygen gas, releasing energy in the form of light and heat. Combustion reactions must involve O 2 as one reactant. The combustion of hydrogen gas produces water vapor. 2H 2 (g)+o 2 (g) 2H 2 O(g) Notice that this reaction also qualifies as a Synthesis reaction. CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(l) In each of these cases hydrocarbons (compounds containing only the elements carbon and hydrogen) combine with oxygen in the air to form carbon dioxide gas and water vapor. This is shown in the following equation for the burning of methane (natural gas) in a gas jet. Complete the following word equations, and write and balance the formula equation. 78) methane (CH 4 ) + oxygen 79) ethane (C2H6) + oxygen 80) propane (C 3 H 8 ) + oxygen 81) butane (C 4 H 10 ) + oxygen 82) pentane (C 5 H 12 ) + oxygen 83) hexane (C 6 H 14 ) + oxygen 84) ethene (C 2 H 4 ) + oxygen 85) ethyne (C 2 H 2 ) + oxygen 86) benzene (C 6 H 6 ) + oxygen pg. 11

13 Decomposition Reactions A decomposition reaction is a reaction in which a compound breaks down into two or more simpler substances. The general form of a decomposition reaction is: AB A+B Most decomposition reactions require an input of energy in the form of heat, light, or electricity. Ammonium nitrate on heating decomposes to give nitrous oxide (laughing gas) and water. NH 4 NO 3 N 2 O + 2H 2 O. A famous reaction is the dissociation reaction of sodium azide according to the following equation 2NaN 3 (S) 2Na(S) + 3N 2 (g) This reaction is used to blow up safety bags in cars where an electric spark provides the beginning of the reaction that produces sodium and nitrogen gas. In decomposition reactions, one compound will break down into two or more parts. Complete the following word equations, and write and balance the formula equation. 87) barium carbonate 88) magnesium carbonate 89) potassium carbonate 90) zinc hydroxide 91) sodium chlorate 92) potassium chlorate 93) carbonic acid pg. 12

14 Replacement reactions Single-Replacement Reactions A single-replacement reaction is a reaction in which one element replaces a similar element in a compound. The general form of a single-replacement (also called single-displacement) reaction is: Hydrogen Replacement A + BC AC + B Many metals react easily with acids and when they do so, one of the products of the reaction is hydrogen gas. Zinc reacts with hydrochloric acid to produce aqueous zinc chloride and hydrogen (Figure below). Zn(s)+2HCl(aq) ZnCl 2 (aq)+h 2 (g) In a hydrogen replacement reaction, the hydrogen in the acid is replaced by an active metal. Some metals are so reactive that they are capable of replacing the hydrogen in water. The products of such a reaction are the metal hydroxide and hydrogen gas. All group 1 metals undergo this type of reaction. Sodium reacts vigorously with water to produce aqueous sodium hydroxide and hydrogen 2Na(s)+2H 2 O(l) 2NaOH(aq)+H 2 (g) Sodium metal reacts vigorously with water, giving off hydrogen gas. A large piece of sodium will often generate so much heat that the hydrogen will ignite. Metal Replacement Magnesium is a more reactive metal than copper. When a strip of magnesium metal is placed in an aqueous solution of copper(ii) nitrate, it replaces the copper. The products of the reaction are aqueous magnesium nitrate and solid copper metal. Mg(s)+Cu(NO 3 ) 2 (aq) Mg(NO 3 ) 2 (aq)+cu(s) This subcategory of single-replacement reactions is called a metal replacement reaction because it is a metal that is being replaced (zinc). pg. 13

15 The Activity Series Single-replacement reactions only occur when the element that is doing the replacing is more reactive than the element that is being replaced. Therefore, it is useful to have a list of elements in order of their relative reactivities. The activity series is a list of elements in decreasing order of their reactivity. Since metals replace other metals, while nonmetals replace other nonmetals, they each have a separate activity series. Table beside is an activity series of most common metals and of the halogens. For a single-replacement reaction, a given element is capable of replacing an element that is below it in the activity series. This can be used to predict if a reaction will occur. Suppose that small pieces of the metal nickel were placed into two separate aqueous solutions: one of iron(iii) nitrate and one of lead(ii) nitrate. Looking at the activity series, we see that nickel is below iron, but above lead. Therefore, the nickel metal will be capable of replacing the lead in a reaction, but will not be capable of replacing iron. Ni(s)+Pb(NO 3 ) 2 (aq) Ni(NO 3 ) 2 (aq)+pb(s) Ni(s)+Fe(NO 3 ) 3 (aq) NR (no reaction) In the descriptions that accompany the activity series of metals, a given metal is also capable of undergoing the reactions described below that section. For example, lithium will react with cold water, replacing hydrogen. It will also react with steam and with acids, since that requires a lower degree of reactivity. Halogen Replacement The element chlorine reacts with an aqueous solution of sodium bromide to produce aqueous sodium chloride and elemental bromine. Cl 2 (g)+2nabr(aq) 2NaCl(aq)+Br 2 (l) The reactivity of the halogen group (group 17) decreases from top to bottom within the group. Fluorine is the most reactive halogen, while iodine is the least. Since chlorine is above bromine, it is more reactive than bromine and can replace it in a halogen replacement reaction. pg. 14

16 Write the skeleton equation, determine whether reaction will take place. If reaction takes place, balance it and write mole relations between reactants and products. 94) Silver metal immersed in potassium nitrate aqueous solution. 95) Zinc metal immersed in silver nitrate aqueous solution. 96) Aluminum metal in sulfuric acid. 97) Chlorine gas is pumped through potassium iodide aqueous solution. 98) Lithium metal is put into water. 99) Copper metal is immersed in iron(ii) sulfate aqueous solution. 100) Sodium metal is put into water. 101) Iron metal is immersed in lead(ii) nitrate aqueous solution. 102) Copper metal is put into water. 103) Copper metal is immersed in aluminum sulfate aqueous solution. 104) Aluminum metal is immersed in lead(ii) nitrate aqueous solution. 105) Chlorine gas is pumped through sodium iodide aqueous solution. 106) Iron metal is immersed in silver acetate aqueous solution. 107) Aluminum metal is immersed in copper(ii) chloride aqueous solution. 108) Liquid bromine is added to aqueous calcium iodide solution. pg. 15

17 109) Aluminum metal is added to hydrochloric acid solution (HCI). 110) Magnesium metal is added to hydrochloric acid solution (HCI). 111) Zinc metal is added to sulfuric acid solution (H 2 SO 4 ). 112) Iron metal is immersed in copper(ii) sulfate aqueous solution. 113) Chlorine gas is pumped through magnesium iodide aqueous solution. 114) A piece of aluminum metal is added to a solution of silver nitrate. 115) Aluminum metal is added to a solution of copper(ii) chloride. 116) Chlorine gas is bubbled into a solution of sodium bromide 117) Hydrogen gas is passed over hot copper(ii) oxide. 118) Magnesium turnings are added to a solution of iron(iii) chloride. 119) Chlorine gas is pumped into a solution of sodium iodide. 120) Fluorine gas is bubbled through a solution of potassium chloride. pg. 16

18 Double-Replacement Reactions A double-replacement reaction is a reaction in which the positive and negative ions of two ionic compounds exchange places to form two new compounds. The general form of a doublereplacement (also called double-displacement) reaction is: AB + CD AD + CB In this reaction, A and C are positively-charged cations, while B and D are negatively-charged anions. Double-replacement reactions generally occur between substances in aqueous solution. Calcium hydroxide and hydrochloric acid react like in the next equation Ca(OH) 2 (aq) + HCl(aq) CaCl 2 (aq) + 2H 2 O(l) In order for a reaction to occur, one of the products is usually a solid precipitate, a gas, or a molecular compound such as water. Formation of a Precipitate A precipitate forms in a double-replacement reaction when the cations from one of the reactants combine with the anions from the other reactant to form an insoluble ionic compound. When aqueous solutions of potassium iodide and lead(ii) nitrate are mixed, the following reaction occurs. Formation of a Gas 2KI(aq)+Pb(NO 3 ) 2 (aq) 2KNO 3 (aq)+pbi 2 (s) Some double-replacement reactions produce a gaseous product which then bubbles out of the solution and escapes into the air. When solutions of sodium sulfide and hydrochloric acid are mixed, the products of the reaction are aqueous sodium chloride and hydrogen sulfide gas. Na 2 S(aq)+2HCl(aq) 2NaCl(aq)+H 2 S(g) Formation of a Molecular Compound Another kind of double-replacement reaction is one that produces a molecular compound as one of its products. Many examples in this category are reactions that produce water. When aqueous hydrochloric acid is reacted with aqueous sodium hydroxide, the products are aqueous sodium chloride and water. HCl(aq) + NaOH(aq) NaCl(aq) + H 2 O(l) pg. 17

19 guidelines for writing double replacement reactions Steps for balancing equations step process Write chemical formulas for reactants Type positive and negative ions in each compound Connect the positive ion in the composite and the negative ion in the other compound Write chemical formulas for products Type the chemical equation of the reaction Balance the reaction Example Al(NO 3 ) 3 (aq) + H 2 SO 4 (aq) Al(NO 3 ) 3 has Al 3+ and (NO 3 ) - H 2 SO 4 has H + 2- and SO 4 Al pairs with SO 4 H + pairs with (NO 3 ) - Al 2 (SO 4 ) 3 HNO 3 Al(NO 3 ) 3 (aq) + H 2 SO 4 (aq) Al 2 (SO 4 ) 3 (aq) + HNO 3 (aq) 2Al(NO 3 ) 3 (aq) + 3H 2 SO 4 (aq) Al 2 (SO 4 ) 3 (aq) + 6HNO 3 (aq) Complete the following word equations, and write and balance the formula equation. 121) aluminum iodide + mercury(ii) chloride 122) silver nitrate + potassium phosphate 123) calcium acetate + sodium carbonate 124) ammonium chloride + mercury(i) acetate 125) iron(ii) sulfide + hydrochloric acid 126) copper(ii) hydroxide + acetic acid 127) calcium hydroxide + phosphoric acid pg. 18

20 Reactions in aqueous solutions Solution: A homogeneous mixture of two or more pure substances. Solvent: substance present in the greatest quantity. Solute: substance dissolved in the solvent. How do compounds dissolve in water? Molecular compounds, divided into two types, 1) Molecules dissolve in water into their original components, without forming ions such as sugar and ethanol. 2) Molecular substances separate in water into ions such as hydrochloric acid. HCl (aq) H + (aq) + CL - (aq) Ionic compounds Ionic compounds consist of positive ions and negative ions that are separated from each other when dissolved in water. This process is called Ionization. This occurs when sodium chloride is dissolved in water. NaCl (aq) Na + (aq) + CL - (aq) pg. 19

21 Types of reactions in aqueous solutions Solvent molecules (water) do not usually enter the reactions that occur in solutions, and the separated ions in the solution react and often double-replacement reactions occur. These reactions produce one of these products, (Precipitate formation, Gas production, or Water composition. 1) Reactions that produce a precipitate Two soluble substances in water may react and produce a non-dissolving substance, Reactants are present in ions form, The dissolves products are also present in the form of ions, But the product that does not dissolve form a precipitate and does not exist in the form of ions Ionic Equations In ionic equations we not only write formulas and symbols of compounds and elements involved in the reaction, but we write the equation in the form of ions, Complete ionic equation: an ionic equation that shows all the particles in the solution. spectator ions: The ions that appear on both sides of the equation, they appear with reactants and products. Net ionic equation: the equation that includes only the particles involved in the reaction pg. 20

22 Write the net ionic equation for each of the following reactions. List all spectator ions. If all species are spectator ions, please indicate that no reaction takes place. 128) A solution of aluminum bromide, AlBr 3 reacts with a solution of sodium hydroxide, NaOH to form the precipitate aluminum hydroxide, Al(OH) ) Aqueous copper (II) nitrate, Cu(NO 3 ) 2 reacts with aqueous potassium carbonate, K 2 CO 3 forming solid copper (II) carbonate, Cu(CO 3 ). 130) A solution of barium chloride, BaCl 2 reacts with a solution of magnesium sulfate, MgSO 4 to form the precipitate barium sulfate, BaSO ) Aqueous potassium sulfide, K 2 S reacts with a solution of cadmium chloride, CdCl 2 to form solid cadmium sulfide, CdS 132) AgNO 3(aq ) + KCl (aq) AgCl (s) + KNO 3(aq) 133) Mg(NO 3 ) 2(aq) + Na 2 CO 3(aq) MgCO 3(s) + NaNO 3(aq) 134) strontium bromide (aq) + potassium sulfate (aq) strontium sulfate (s) + potassium bromide (aq) 135) manganese(ii)chloride (aq) + ammonium carbonate (aq) manganese(ii)carbonate (s) + ammonium chloride (aq) 136) chromium(iii)nitrate (aq ) + iron(ii)sulfate (aq) chromium(iii)sulfate (aq) + iron(ii)nitrate (aq) pg. 21

23 2) Reactions that form water In some double-substitution reactions water is a product but we cannot distinguish the formation of water because it is essentially the solvent that is the reactants dissolved in Chemical equation Sodium hydroxide with hydrobromic acid HBr (aq) + NaOH (aq) H 2 O (l) + NaBr (aq) Complete ionic equation Spectator ions removing Net ionic equation H + (aq) + Br - (aq) + Na + (aq) + OH - (aq) H 2 O (l) + Na + (aq) + Br - (aq) H + (aq) + Br - (aq) + Na + (aq) + OH - (aq) H 2 O (l) + Na + (aq) + Br - (aq) H + (aq) + OH - (aq) H 2 O (l) 3) Reactions that form gases Some double-replacement reactions result in gases such as carbon dioxide, hydrogen cyanide or hydrogen sulfide Lithium sulfide with hydroiodic acid Chemical equation Complete ionic equation Spectator ions removing Net ionic equation 2HI (aq) + Li 2 S (aq) H 2 S (g) + 2LiI (aq) 2H + (aq) + 2I - (aq) + 2Li + (aq) + S 2- (aq) H 2 S (g) + 2Li + (aq) + 2I - (aq) 2H + (aq) + 2I - (aq) + 2Li + (aq) + S 2- (aq) H 2 S (g) + 2Li + (aq) + 2I - (aq) 2H + (aq) + S 2- (aq) H 2 S (g) Write the net ionic equation for each of the following reactions CaCO3 (s) + 2HCl (aq) CaCl2 (aq) + CO2 (g) + H2O (l) NaHCO3 (aq) + HBr (aq) NaBr (aq) + CO2 (g) + H2O (l) SrSO3 (s) + 2 HI (aq) SrI2 (aq) + SO2 (g) + H2O (l) Na2S (aq) + H2SO4 (aq) Na2SO4 (aq) + H2S (g) pg. 22

24 Overall equations Some chemical reactions occur in more than one step. For example, the reaction of hydrochloric acid with sodium bicarbonate is as follows Hydrochloric acid with Sodium bicarbonate Equation 1 Equation 2 Combined equation Overall equation Complete ionic equation Spectator ions removing Net ionic equation HCl (aq) + NaHCO 3(aq) H 2 CO 3(aq) + NaCl (aq) H 2 CO 3(l) H 2 O (l) + CO 2(g) HCl (aq) + NaHCO 3(aq) + H 2 CO 3(aq) H 2 CO 3(aq) + NaCl (aq) + H 2 O (l) + CO 2(g) HCl (aq) + NaHCO 3(aq) NaCl (aq) + H 2 O (l) + CO 2(g) H + (aq) + Cl - (aq) + Na + (aq) + HCO 3 - (aq) H 2 O (l) + CO 2(g) + Na + (aq) + Cl - (aq) H + (aq) + Cl - (aq) + Na + (aq) + HCO 3 - (aq) H 2 O (l) + CO 2(g) + Na + (aq) + Cl - (aq) H + (aq) + HCO 3 - (aq) H 2 O (l) + CO 2(g) Overall equation: An equation that combines two reactions. the reaction between hydrogen ions and bicarbonates occurs within the lung cells, where carbon dioxide travels with the blood in the form of carbonate ions that soon combine with the hydrogen ions producing carbon dioxide which is released during exhalation. The same reaction takes place in the products that depend on baking soda which is the responsible for the baked goods rises, it is also used in the manufacture of toothpaste, detergents as well as in the manufacture of fire extinguishers pg. 23