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Types of Chemical Reactions

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  • NaCl(aq) AgNO3(aq) → NaNO3(aq) + AgCl(s)
    Double Replacement
  • 2Na(s)+2H2O(l)→2NaOH(aq)+H2(g)
    Single Replacement
  • C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)
    Combustion
  • CaCO3(s) → CaO(s) + CO2(g)
    Decomposition
  • 2S(s)+3O2(g)→2SO3(g)
    Synthesis
  • Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s)
    Single Replacement
  • Mg(s)+Cu(NO3)2(aq)→Mg(NO3)2(aq)+Cu(s)
    Single Replacement
  • 2H2O(l)→elec2H2(g)+O2(g)
    Decomposition
  • A single reactant breaks down to form 2 or more products.
    Decomposition
  • 2NaOH(s)→Na2O(s)+H2O(g)
    Decomposition
  • A single element replaces a similar element of an adjacent reactant compound.
    Single-Replacement
  • HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
    Double Replacement
  • A single element or compound combines with oxygen gas releasing energy.
    Combustion
  • Two ionic compounds exchange ions, producing 2 new ionic compounds.
    Double Replacement
  • C(s) + O2(g) → CO2(g)
    Synthesis
  • H2CO3(aq) → H2O(l) + CO2(g)
    Decomposition
  • C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(g)
    Combustion
  • Two or more reactants combine to make 1 new product.
    Synthesis
  • H2O(l) + SO3(g) → H2SO4(aq)
    Synthesis
  • 4Fe(s)+3O2(g)→2Fe2O3(s)
    Synthesis
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