Chapter%203 - Stoichiometry Now it Gets Fun Do all...

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Stoichiometry: Now it Gets Fun! Do all exercises within the chapter as you read. Suggested exercises at the end of the chapter: 3.1, 3.4, 3.6, 3.7, 3.10, 3.11, 3.13, 3.15, 3.19, 3.23, 3.26, 3.27, 3.29, 3.33, 3.37, 3.41, 3.43, 3.47, 3.49, 3.51a, 3.52b, 3.53, 3.55, 3.57, 3.59, 3.63, 3.65, 3.67, 3.69, 3.72, 3.73, 3.79, 3.81, 3.86, 3.98, 3.104. If you get stuck on a particular type of problem try solving others like it until you are comfortable.
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Chemical Reactions are Represented by Chemical Equations 2H 2 (g) + O 2 (g) 2H 2 O(g)
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Components of a Chemical Equation 2 H 2 (g) + O 2 (g) 2 H 2 O (g) Subscript Coefficient Physical State Reactants Product
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Subscript vs. Coefficient Subscripts tell the number of atoms of each element in a molecule (balanced formula) Coefficients tell the number of molecules (balanced equation)
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Analyzing a Chemical Equation CH 4 ( g ) + 2 O 2 ( g ) CO 2 ( g ) + 2 H 2 O ( g )
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Balancing Equations: Sample Problems First try to balance the elements that occur in the fewest chemical formulas on each side of the equation. 1. Li( s ) + N 2 ( s ) Li 3 N( s ) 2. NH 4 NO 3 ( s ) N 2 ( g ) + O 2 ( g ) + H 2 O( g )
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Combination or Decomposition Reactions Combination: Decomposition: 2Mg( s ) + O 2 ( g ) 2MgO( s ) 2NaN 3 ( s ) 2Na( s ) + 3N 2 ( g )
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Combustion Reactions Rapid reactions producing flame. Typically involves the reaction of oxygen in the air and hydro- carbons to produce carbon dioxide and water. Examples: CH 4 ( g ) + 2 O 2 ( g ) → CO 2 ( g ) + 2 H 2 O ( g ) C 3 H 8 ( g ) + 5 O 2 ( g ) → 3 CO 2 ( g ) + 4 H 2 O ( g )
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Predicting Chemical Equations for Chemical Reactions Combination Reaction Mg( s ) + N 2 ( g ) Decomposition MgCO 3 (s) Combustion C 6 H 6 ( l ) +
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Molecular and Formula Weights Sum of the atomic weights for the atoms in a molecule (molecular weight) or an ionic compound’s chemical formula (formula weight).
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