Textbook Notes (280,000)
CA (160,000)
UTSC (20,000)
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CHMA10H3 (100)
Chapter 4

CHMA10H3 Chapter Notes - Chapter 4: Lead


Department
Chemistry
Course Code
CHMA10H3
Professor
Ann Verner
Chapter
4

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Chapter 4 Chemical Quantities and Aqueous Reactions
4.1 Global Warming and the Combustion of Fossil Fuels
N/A
4.2 Reaction Stoichiometry: How Much Carbon Dioxide?
- The coefficients in a chemical reaction specify the relative amounts in moles of each of the
substance involved in the reaction (making mole-to-mole conversions, mass-to-mass
conversions)
4.3 Limiting Reactant, Theoretical Yield and Percent Yield
- Limiting reactant is the reactant that limits the amount of product in a chemical
reaction
- Excess Reactant is any reactant that occurs in greater quantity
- Theoretical yield is the amount of product that can be made in a chemical reaction
BASED on the limiting reactant
- Actual yield is the amount of product actually produced in the chemical reaction
- Percent yield is the % of the theoretical yield that was actually obtained
(actual/theoretical x 100%)
- i.e. 2 Mg(s) + O2(g) 2 MgO(s), 42.5 G Mg and 33.8g O, what is the limiting reactant
(Mg) and theoretical yield (79.3%)
4.4 Solution Concentration and Solution Stoichiometry
- Solution is: solvent is the major component while the solvent is the minor
- Dilute solution is one that contains small solute relative to solvent while concentrated
solutions has relative amounts of solute and solvent
- Molarity (M) = amount of solute (in mol)/ volume of solutions (in L)
I.e. If 25.5g KBr is dissolved in enough water to make 1.75L of solution, what is the
molarity? (Solution: do molar mass, and use the amount of KBr to find mol., then find
molarity = 0.112M)
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