Chemical Reactions

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Chemical Reactions

• Predicting Products and Balancing Equations

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I. Synthesis (Composition) Reactions

• A) Liquid hydrogen plus liquid oxygen yields
  gaseous water plus a lot of energy.
• H2(l) O2(l) --gt H2O (g)
• reactants yield products
• 2H2(l) O2(l) --gt 2H2O (g)
• Coefficients are used to balance equations.

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• B. All these type reactions take the general form
• A B --gt AB
• Two or more elements
• yielding a single
• compound.
• C. Fe(s) O2 (g) --gt FeO2 (s)
• Iron plus oxygen yields iron IV oxide
  (rust).

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II. Decomposition Reactions

• All take the general form
• A B ---gt A B
• 2KClO3(s) --gt2KCl(s) O2(g
• This reaction was one of the first reactions
  used to make pure oxygen.
• Salt producing ions in water is another example.
• 2NaCl(s) --gt2Na(aq) Cl2(aq)

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III. Single Replacement Reactions

• B. They may also take the form
• - - - -
• C AD --gt AC D
• F2(g) 2 KI(s) ----gt
• 2KF(s) I2(g)

• A. These take the form of
• - -
• A BC -gt AC B
• Zn(s) 2HCl(aq) ---gt
• ZnCl2S) H2(g)
• This is one of the reactions we used in the
  lab to make hydrogen.

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IV. Double Replacement Reactions

• Take the general form
• - - - -
• AB CD --gt AD CB
• HCl(aq) NaOH(aq) --gt
• acid base
• NaCl(s) HOH(l)
• salt water
• Neutralization rxn (also how soap is made)

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V. Combustion Reaction

• Take the general form of
• CxHy O2 --gt CO2 H2O
• (excess)
• CxHy O2 --gt CO H2O
• (limited)
• Any hydrocarbon when
• burned produces carbon
• dioxide and water
• (gasoline and natural
• gas are other examples)