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Worksheet Predicting Products of Reactions Key, Exercises of Chemistry

Georgia Southern University–Armstrong CampusChemistry

Fill in the blanks with what would be products with given reactants and what is the reaction type

Typology: Exercises

2020/2021

Uploaded on 04/20/2021

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Predicting Products of Chemical Reactions
This worksheet is designed to help you predict products of simple reactions of the four basic reaction types (synthesis,
decomposition, single replacement, and double replacement) and combustion reactions.
For the first few reactions, the type of reaction is listed, you should predict the products, then balance. Further questions just have
the reactants listed and you should decide on the type of reaction, as well as the correct products. Many of these reactions fall into
the category of redox reactions, though do not let that confuse you...each can be described in terms of the four basic reaction types
(except the combustion reactions).
Although states (s, l, g, aq) of the reactants and products are very important in a chemical reaction, don’t worry about determining
those for these problems. Rather, focus on what products might result from the reactants given. Pay particular attention to the ionic
charge of species that you know form ions with only one possible charge (e.g., alkali metals, alkaline earth metals, halogens, etc.)
a. Combustion: C6H12 + O2
b. Combustion: C4H6 + O2
c. Combustion: C6H10O3 + O2
1. Synthesis: Mg + I2
2. Double displacement: CuCl2 + H2S
3. Double displacement: NaOH + HClO4
4. Decomposition: ZnCO3 + heat
5. Single replacement: HCl + Zn
6. ________________ Na + MgCl2
7. ________________ CaCl2 + K2CO3
8. ________________ K + Cl2
9. ________________ BaCl2 + K3PO4
10. ________________ H2SO4 + KOH
11. ________________ Al2(CO3)3 + heat
12. ________________ Al + O2
13. ________________ Pb(NO3)2 + KOH
14. ________________ H2SO4 + BaCl2
15. ________________ Ca + AgCl
16. ________________ H3PO4 + FeBr3
17. ________________ Li + N2
18. ________________ HCl + Mg(OH)2
19. ________________ Mg(OH)2 + heat
20. ________________ Fe(OH)3 + heat
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Predicting Products of Chemical Reactions

This worksheet is designed to help you predict products of simple reactions of the four basic reaction types (synthesis, decomposition, single replacement, and double replacement) and combustion reactions.

For the first few reactions, the type of reaction is listed, you should predict the products, then balance. Further questions just have the reactants listed and you should decide on the type of reaction, as well as the correct products. Many of these reactions fall into the category of redox reactions, though do not let that confuse you...each can be described in terms of the four basic reaction types (except the combustion reactions).

Although states (s, l, g, aq) of the reactants and products are very important in a chemical reaction, don’t worry about determining those for these problems. Rather, focus on what products might result from the reactants given. Pay particular attention to the ionic charge of species that you know form ions with only one possible charge ( e.g. , alkali metals, alkaline earth metals, halogens, etc.)

a. Combustion: C 6 H 12 + O 2 

b. Combustion: C 4 H 6 + O 2 

c. Combustion: C 6 H 10 O 3 + O 2 

  1. Synthesis: Mg + I 2 
  2. Double displacement: CuCl 2 + H 2 S 
  3. Double displacement: NaOH + HClO 4 
  4. Decomposition: ZnCO 3 + heat 
  5. Single replacement: HCl + Zn 
  6. ________________ Na + MgCl 2 
  7. ________________ CaCl 2 + K 2 CO 3 
  8. ________________ K + Cl 2 
  9. ________________ BaCl 2 + K 3 PO 4 

10. ________________ H 2 SO 4 + KOH 

  1. ________________ Al 2 (CO 3 ) 3 + heat 
  2. ________________ Al + O 2 
  3. ________________ Pb(NO 3 ) 2 + KOH 
  4. ________________ H 2 SO 4 + BaCl 2 
  5. ________________ Ca + AgCl 
  6. ________________ H 3 PO 4 + FeBr 3 
  7. ________________ Li + N 2 
  8. ________________ HCl + Mg(OH) 2 
  9. ________________ Mg(OH) 2 + heat 
  10. ________________ Fe(OH) 3 + heat 

Answers for Predicting Products of Chemical Reactions

For all combustion reactions of hydrocarbons or hydrogen-carbon-oxygen molecules, the products will always be CO 2 and H 2 O (assuming a complete reaction).

a. Combustion: C 6 H 12 + 9O 2  6CO 2 + 6H 2 O

b. Combustion: 2C 4 H 6 + 11O 2  8CO 2 + 6H 2 O

c. Combustion: C 6 H 10 O 3 + 7O 2  6CO 2 + 5H 2 O

  1. Synthesis: Mg + I 2  MgI 2 Note that Mg can only form Mg2+^ and I can only form I-, so the product will must have a 1:2 cation:anion ratio.
  2. Double displacement: CuCl 2 + H 2 S  CuS + 2HCl Note that the product is not H 2 Cl 2. It is important to recognize that CuCl 2 is made of three ions, Cu2+^ and two Cl-.
  3. Double displacement: NaOH + HClO 4  NaClO 4 + H 2 O In this question, you must recognize that perchlorate, ClO 4 - , and hydroxide, OH-, are polyatomic ions and will not break apart. Also, this is an acid-base reaction, so the products should be salt and water.
  4. Decomposition: ZnCO 3 + heat  ZnO + CO 2 When reactions have heat as a reactant, it is very likely that they will involve decompositions. Carbonate compounds usually decompose to CO 2 and a metal oxide.
  5. Single replacement: 2HCl + Zn  ZnCl 2 + H 2 Note that one reactant is in its elemental form; if a single replacement reaction is going to occur, the species NOT in its elemental form in the reactants (H+^ in this case), will end up in its elemental form in the products (H 2 ) and the species that IS in its elemental form (Zn) will end up ionized (Zn2+). Note that zinc can only form a Zn2+^ ion, so it will have two chloride ions. Note also that hydrogen in its elemental form is H 2 , not H.
  6. Single replacement 2Na + MgCl 2  2NaCl + Mg Again notice that one species is in its elemental form (Na). The magnesium in MgCl 2 is an ion (Mg2+), but is transformed into its elemental state (Mg), while the Na is converted into an ion (Na+, sodium only forms a +1 ion).
  7. Double replacement CaCl 2 + K 2 CO 3  CaCO 3 + 2KCl Recognize that carbonate is a polyatomic ion (CO 3 2-) and that the cations are already stable ions (Ca2+^ and K+).
  8. Synthesis 2K + Cl 2  2KCl Note that both materials are elemental species, so the only result could be a synthesis reaction. In the product, K+ and Cl-^ are formed. Note that we would NOT write the product as K 2 Cl 2. Ionic compounds are written in their simplest forms.
  9. Double replacement 3BaCl 2 + 2K 3 PO 4  Ba 3 (PO 4 ) 2 + 6KCl Note that phosphate (PO 4 3-) is a polyatomic ion and will not break apart. Since barium is a +2 ion, the barium phosphate will have a 3:2 ratio of Ba:PO 4 in order to balance the charge.
  10. Double replacement H 2 SO 4 + 2KOH  2H 2 O + K 2 SO 4 Notice that sulfate (SO 4 2-) is a polyatomic ion and that potassium exists as a +1 ion (K+). Also, this is an acid-base reaction, so the products should be salt and water.
  11. Decomposition Al 2 (CO 3 ) 3 + heat  Al 2 O 3 + 3CO 2 Another decomposition that will generate CO 2 and a metal oxide (note that Al forms a +3 ion, Al3+, and monatomic oxygen will have a – 2 charge, O2-).