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Daily Inquiry : Monday, January 28

Daily Inquiry : Monday, January 28. Convert the following word equations into formula equations and balance. Be sure to include state labels and reaction conditions in the equation. When heated, solid aluminum carbonate decomposes to form solid aluminum oxide and carbon dioxide gas. 

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Daily Inquiry : Monday, January 28

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  1. Daily Inquiry:Monday, January 28 Convert the following word equations into formula equations and balance. Be sure to include state labels and reaction conditions in the equation. • When heated, solid aluminum carbonate decomposes to form solid aluminum oxide and carbon dioxide gas.  • Hydrogen gas and iron (III) oxide powder react to form liquid water and solid iron powder. • Pellets of sodium hydroxide are dropped into an aqueous solution of iron(III) chloride, iron(III) hydroxide precipitates and sodium chloride stays dissolved in the water.

  2. Extended Science Vocabulary of the Week1-28-2013 • Inert – • not chemically reactive. • Since noble gases have a completely filled valence shell, they are considered inert.  • Deflagrate – • to burn, especially suddenly and violently. • Explosive materials will deflagrate when ignited.

  3. Synthesis Reactions • In a synthesis reaction, also known as a composition or combination reaction, two or more reactants combine to form a single product. • This type of reaction is represented by the following general equation. A + X  AX • Formation of binary compound from its elements 2 Cu(s) + O2(g)  2 CuO(s) S8 (s) + 8 O2(g)  8 SO2(g) 2 Na(s) + Cl2(g)  2 NaCl(s)

  4. Reactants can also be compounds. CaO(s) + H2O(l)  Ca(OH)2(s) SO2(g) + H2O(l)  H2SO3(aq) CaO(s) + SO2(g)  CaSO3(s)

  5. Decomposition Reactions In a decomposition reaction, a single reactant undergoes a reaction that produces two or more simpler substances. Decomposition reactions are the opposite of synthesis reactions. They are represented by the following general equation. AX  A + X Decomposition reactions take place only when energy is added.

  6. Types of Decomposition Reactions • Decomposition of Binary Compounds • compound breaks up into its elements 2 H2O (l)  2 H2 (g) + O2 (g) 2 HgO (s)  2 Hg (l) + O2 (g) • Decomposition of Metal Carbonates • when heated, metal carbonates decompose into a metal oxide and carbon dioxide CuCO3 (s)  CuO (s) + CO2 (g)

  7. c) Decomposition of Metal Chlorates • when heated, metal chlorates decompose into a metal chloride and oxygen 2 KClO3 (s)  2 KCl (s) + 3 O2 (g)

  8. Final Countdown What are the three most important things you learned today? What are two questions you would still liked answered? What is the one way what you learned connects with what you know before?

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