Stoichiometry of Chemical Reactions: Balancing, Classification, and Calculations

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This educational presentation covers the fundamentals of chemical reaction stoichiometry. Key topics include writing and balancing chemical equations, classifying reactions such as acid-base, precipitation, and redox, mole-mole stoichiometry, limiting reactants and percent yield, and quantitative analysis methods like titration and gravimetric analysis. Designed for chemistry students in the College of Natural and Computational Sciences.

May 11, 202619 slides

Slide 1 of 19

Slide 1 - Stoichiometry of a Chemical Reaction

Stoichiometry of a Chemical Reaction

College of Natural and Computational Sciences Department of Chemistry

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Slide 1 - Stoichiometry of a Chemical Reaction

Slide 2 of 19

Slide 2 - Chapter Outline

Writing and Balancing Chemical Equations
Classification of Chemical Reactions
Reaction Stoichiometry
Reaction Yield
Quantitative Chemical Analysis

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Slide 3 of 19

Slide 3 - Writing and Balancing Chemical Equations

4.1

Writing and Balancing Chemical Equations

From symbolic notation to balanced reactions per law of conservation of mass

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Slide 3 - Writing and Balancing Chemical Equations

Slide 4 of 19

Slide 4 - Writing Chemical Equations

Symbolic representation of a chemical reaction
Concise shorthand for relative amounts of reactants and products
Reactants on left (+ separated), products on right (+ separated), arrow indicates direction
Shows formulas, physical states (s, l, g, aq), relative numbers
Example: Ca(s) + 2H₂O(l) → Ca(OH)₂(aq) + H₂(g)

Slide 5 of 19

Slide 5 - Steps to Balance Equations

Step	Action	Example: N₂H₄(l) + N₂O₄(l) → N₂(g) + H₂O(l)
1	Write unbalanced equation
2	Balance elements with coefficients (except H,O last)	2N₂H₄ + N₂O₄ → 3N₂ + 4H₂O
3	Add states (g,l,s,aq)

Slide 6 of 19

Slide 6 - Equations for Ionic Reactions

Molecular Equation Ba(NO₃)₂(aq) + Na₂SO₄(aq) → BaSO₄(s) + 2NaNO₃(aq)

Net Ionic Equation Ba²⁺(aq) + SO₄²⁻(aq) → BaSO₄(s)

(Spectator ions: Na⁺, NO₃⁻ canceled from complete ionic)

Slide 7 of 19

Slide 7 - Classification of Chemical Reactions

4.2

Classification of Chemical Reactions

Acid-base neutralization, precipitation, and oxidation-reduction reactions

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Slide 7 - Classification of Chemical Reactions

Slide 8 of 19

Slide 8 - Acid-Base Reactions

Transfer of H⁺ from acid to base
Neutralization produces salt and water
Acid donates H⁺, base provides OH⁻ → H₂O; anions/cations form salt
Example: H₂SO₄(aq) + Mg(OH)₂(aq) → MgSO₄(aq) + 2H₂O(l)
SO₂ + 2NaOH → Na₂SO₃ + H₂O

Slide 9 of 19

Slide 9 - Solubility Rules for Ionic Compounds in Water

Category	Examples	Solubility
Nitrates (NO₃⁻)	All	Soluble
Acetates (CH₃COO⁻)	All	Soluble
Halides (Cl⁻, Br⁻, I⁻)	Most, except Ag⁺, Pb²⁺, Hg₂²⁺	Soluble
Sulfates (SO₄²⁻)	Most, except Ba²⁺, Pb²⁺, Sr²⁺, Ca²⁺	Soluble
Carbonates (CO₃²⁻), Phosphates (PO₄³⁻)	Most	Insoluble except Group 1 & NH₄⁺
Hydroxides (OH⁻)	Most	Insoluble except Group 1,2 & NH₄⁺

Slide 10 of 19

Slide 10 - Oxidation-Reduction (Redox) Reactions

Oxidation: substance gains oxygen or loses electrons
Reduction: substance loses oxygen or gains electrons
Always occur together
Examples: Fe → rust (Fe₂O₃), bleaching, H₂O₂ → H₂O + O₂

Slide 11 of 19

Slide 11 - Oxidation Number Rules

Rule	Description
1	Uncombined elements: 0
2	Monatomic ions: = charge
3	O in compounds: -2 (peroxides -1)
4	H in compounds: +1 (hydrides -1)
5	Sum in compound: 0
6	Sum in polyatomic ion: = charge

Slide 12 of 19

Slide 12 - Half-Reaction Method for Redox (Acidic)

Step	Action
1	Split into oxidation and reduction half-reactions
2	Balance elements except H,O
3	Balance O with H₂O
4	Balance H with H⁺
5	Balance charge with e⁻
6	Equalize e⁻, add halves
7	For basic: add OH⁻ to neutralize H⁺, form H₂O
8	Verify atoms & charge