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Spontaneous Decompositions

Spontaneous Decompositions. H 2 CO 3 ( aq ) -> H 2 0 (l) + CO 2 (g) NH 4 OH ( aq ) -> H 2 O (l) + NH 3. Net Ionic Reactions : 3 steps. 1. Complete balanced equation 2. Complete Ionic Equation -break “ aq ” states into ions -Cross out identical reactants and products

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Spontaneous Decompositions

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  1. Spontaneous Decompositions • H2CO3(aq) -> H20(l) + CO2(g) • NH4OH(aq) -> H2O(l) + NH3

  2. Net Ionic Reactions : 3 steps • 1. Complete balanced equation • 2. Complete Ionic Equation • -break “aq” states into ions • -Cross out identical reactants and products • 3. Net ionic equation • If a No reaction, then no net ionic equation.

  3. Spectator Ion = an ion that appears on both sides of an equation and is not directly involved in the reaction

  4. Single Replacement 1Cu(s) + 2AgNO3(aq) -> 1Cu(NO3)2(aq) + 2Ag(s) 1Cu(s) + 2Ag1+(aq) +2NO31-(aq) -> 1Cu2+ + 2NO31- (aq) + 2Ag(s) 1Cu(s) + 2Ag1+(aq) -> 1Cu2+ + 2Ag(s) Balanced: Complete: Net

  5. Double Replacement Balanced: AgNO3(aq) + KCl(aq) AgCl(s) + KNO3(aq) Compelte: Ag+(aq) + NO3–(aq)+ K+(aq) + Cl–(aq)AgCl(s) + K+(aq) +NO3–(aq) Ag+(aq) + Cl–(aq)AgCl(s) Net

  6. Net Ionic Reactions! - DR Balanced: Pb(NO3) 2(aq) +2LiCl(aq) PbCl2 (s) + 2LiNO3(aq) C: Pb+2(aq)+2NO3–(aq)+2 Li+(aq)+2Cl–(aq)PbCl2(s)+2Li+(aq)+2NO3–(aq) Pb+2(aq) + 2Cl–(aq)PbCl2 (s) Net:

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