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Table 2. Classification of Chemical Reactions Type of Reaction General Description and Example(s) Combination Two reactants combine to form a single product. The reactants may be elements or compounds. Also calied a synthesis reaction. Zn(s) + L(s) → Znl,(s) CaO(s) + H,O(1) → Ca(OH),(s) Decomposition One reactant, a compound, breaks down to give two or more products. 2H,0,(aq) → 2H,0(1) + 0,(g) Single Replacement An element reacts with a compound and replaces one of the elements in the compound. Metals replace hydrogen or other metals; nonmetals replace nonmetals. Zn(s) + 2HCI(aq) → H,(g) + ZNCI,(ag) Cu(s) + 2A£NO3(aq) → 2Ag(s) + Cu(NO,),(aq) Cl,(aq) + 2Nal(aq) L(aq} + 2NaCl(aq) Double Two ionic compounds (or compounds that break apart to form ions in solution) exchange ions to form new compounds. Examples include precipitation reactions (driving force is formation of a precipitate), acid–base reactions (driving force is formation of water), and gas-forming reactions (driving force is evolution of a gas). NaCl(aq) + A£NO3(aq) H,SO,(aq) + 2NaOH(aq) → Na,SO̟(aq) + 2H,0(1) Na,SO,(aq) + 2HCI(aq) Replacement A£CI(s) + NaNO3(aq) 2NAÇI(aq) + H,0(1) + SO,(g) Combustion A compound burns in the presence of oxygen, producing energy in the form of heat and light. The combustion of organic compounds produces carbon dioxide and water. C,H;(1) + 60,(g) → 4CO,(g) + 4H,0(g) b Questions 1. Write a balanced chemical equation for each reaction #1–8. Classify each reaction using the information provided in the Background section (see Table 2). Reaction #1: Mg (sy 029 Reaction #2: Mg RS Reaction #3: Culy)z COBLS)-) Reaction #4: Ca C0a 1s) Helcae? → Reaction #5: 2nis) + Cucizcae Reaction #6: Cucl caq? Nag Pou Log) > Reaction #7: H Cl cau) +Naotl cae Reaction #8: C 2Ho @lesOzug)> 2. Classifying chemical reactions helps chemists to predict the possible products that will ubetanees ava mived Complete and halance the following equa

Table 2. Classification of Chemical Reactions Type of Reaction General Description and Example(s) Combination Two reactants combine to form a single product. The reactants may be elements or compounds. Also calied a synthesis reaction. Zn(s) + L(s) → Znl,(s) CaO(s) + H,O(1) → Ca(OH),(s) Decomposition One reactant, a compound, breaks down to give two or more products. 2H,0,(aq) → 2H,0(1) + 0,(g) Single Replacement An element reacts with a compound and replaces one of the elements in the compound. Metals replace hydrogen or other metals; nonmetals replace nonmetals. Zn(s) + 2HCI(aq) → H,(g) + ZNCI,(ag) Cu(s) + 2A£NO3(aq) → 2Ag(s) + Cu(NO,),(aq) Cl,(aq) + 2Nal(aq) L(aq} + 2NaCl(aq) Double Two ionic compounds (or compounds that break apart to form ions in solution) exchange ions to form new compounds. Examples include precipitation reactions (driving force is formation of a precipitate), acid–base reactions (driving force is formation of water), and gas-forming reactions (driving force is evolution of a gas). NaCl(aq) + A£NO3(aq) H,SO,(aq) + 2NaOH(aq) → Na,SO̟(aq) + 2H,0(1) Na,SO,(aq) + 2HCI(aq) Replacement A£CI(s) + NaNO3(aq) 2NAÇI(aq) + H,0(1) + SO,(g) Combustion A compound burns in the presence of oxygen, producing energy in the form of heat and light. The combustion of organic compounds produces carbon dioxide and water. C,H;(1) + 60,(g) → 4CO,(g) + 4H,0(g) b Questions 1. Write a balanced chemical equation for each reaction #1–8. Classify each reaction using the information provided in the Background section (see Table 2). Reaction #1: Mg (sy 029 Reaction #2: Mg RS Reaction #3: Culy)z COBLS)-) Reaction #4: Ca C0a 1s) Helcae? → Reaction #5: 2nis) + Cucizcae Reaction #6: Cucl caq? Nag Pou Log) > Reaction #7: H Cl cau) +Naotl cae Reaction #8: C 2Ho @lesOzug)> 2. Classifying chemical reactions helps chemists to predict the possible products that will ubetanees ava mived Complete and halance the following equa

Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter18: Oxidation–reduction Reactions And Electrochemistry
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Table 2. Classification of Chemical Reactions Type of Reaction General Description and Example(s) Combination Two reactants combine to form a single product. The reactants may be elements or compounds. Also calied a synthesis reaction. Zn(s) + L(s) → Znl,(s) CaO(s) + H,O(1) → Ca(OH),(s) Decomposition One reactant, a compound, breaks down to give two or more products. 2H,0,(aq) → 2H,0(1) + 0,(g) Single Replacement An element reacts with a compound and replaces one of the elements in the compound. Metals replace hydrogen or other metals; nonmetals replace nonmetals. Zn(s) + 2HCI(aq) → H,(g) + ZNCI,(ag) Cu(s) + 2A£NO3(aq) → 2Ag(s) + Cu(NO,),(aq) Cl,(aq) + 2Nal(aq) L(aq} + 2NaCl(aq) Double Two ionic compounds (or compounds that break apart to form ions in solution) exchange ions to form new compounds. Examples include precipitation reactions (driving force is formation of a precipitate), acid–base reactions (driving force is formation of water), and gas-forming reactions (driving force is evolution of a gas). NaCl(aq) + A£NO3(aq) H,SO,(aq) + 2NaOH(aq) → Na,SO̟(aq) + 2H,0(1) Na,SO,(aq) + 2HCI(aq) Replacement A£CI(s) + NaNO3(aq) 2NAÇI(aq) + H,0(1) + SO,(g) Combustion A compound burns in the presence of oxygen, producing energy in the form of heat and light. The combustion of organic compounds produces carbon dioxide and water. C,H;(1) + 60,(g) → 4CO,(g) + 4H,0(g)
Transcribed Image Text:Table 2. Classification of Chemical Reactions Type of Reaction General Description and Example(s) Combination Two reactants combine to form a single product. The reactants may be elements or compounds. Also calied a synthesis reaction. Zn(s) + L(s) → Znl,(s) CaO(s) + H,O(1) → Ca(OH),(s) Decomposition One reactant, a compound, breaks down to give two or more products. 2H,0,(aq) → 2H,0(1) + 0,(g) Single Replacement An element reacts with a compound and replaces one of the elements in the compound. Metals replace hydrogen or other metals; nonmetals replace nonmetals. Zn(s) + 2HCI(aq) → H,(g) + ZNCI,(ag) Cu(s) + 2A£NO3(aq) → 2Ag(s) + Cu(NO,),(aq) Cl,(aq) + 2Nal(aq) L(aq} + 2NaCl(aq) Double Two ionic compounds (or compounds that break apart to form ions in solution) exchange ions to form new compounds. Examples include precipitation reactions (driving force is formation of a precipitate), acid–base reactions (driving force is formation of water), and gas-forming reactions (driving force is evolution of a gas). NaCl(aq) + A£NO3(aq) H,SO,(aq) + 2NaOH(aq) → Na,SO̟(aq) + 2H,0(1) Na,SO,(aq) + 2HCI(aq) Replacement A£CI(s) + NaNO3(aq) 2NAÇI(aq) + H,0(1) + SO,(g) Combustion A compound burns in the presence of oxygen, producing energy in the form of heat and light. The combustion of organic compounds produces carbon dioxide and water. C,H;(1) + 60,(g) → 4CO,(g) + 4H,0(g)
b Questions 1. Write a balanced chemical equation for each reaction #1–8. Classify each reaction using the information provided in the Background section (see Table 2). Reaction #1: Mg (sy 029 Reaction #2: Mg RS Reaction #3: Culy)z COBLS)-) Reaction #4: Ca C0a 1s) Helcae? → Reaction #5: 2nis) + Cucizcae Reaction #6: Cucl caq? Nag Pou Log) > Reaction #7: H Cl cau) +Naotl cae Reaction #8: C 2Ho @lesOzug)> 2. Classifying chemical reactions helps chemists to predict the possible products that will ubetanees ava mived Complete and halance the following equa
Transcribed Image Text:b Questions 1. Write a balanced chemical equation for each reaction #1–8. Classify each reaction using the information provided in the Background section (see Table 2). Reaction #1: Mg (sy 029 Reaction #2: Mg RS Reaction #3: Culy)z COBLS)-) Reaction #4: Ca C0a 1s) Helcae? → Reaction #5: 2nis) + Cucizcae Reaction #6: Cucl caq? Nag Pou Log) > Reaction #7: H Cl cau) +Naotl cae Reaction #8: C 2Ho @lesOzug)> 2. Classifying chemical reactions helps chemists to predict the possible products that will ubetanees ava mived Complete and halance the following equa
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