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Do Now: (this problem is in your packet)
Ribose is an important sugar found in DNA and RNA. Ribose has a gram molecular mass of 150 g/mol and an empirical formula of CH2O. What is the molecular formula for ribose?
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Chemical Equations
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What are they?
Def: represents, with symbols and formulas, the reactants and products of a chemical reaction
• Details the ratios of the substances that react.
• Equation must contain the correct formulas of reactants and products
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Law of Conservation of Mass
• matter cannot be created or destroyed• same # of atoms of each element must
be written as products and reactants• coefficients are written to equalize the
number of atoms of each element (coefficients – numbers placed before chemical formulas)
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Balancing chemical equations
1. Identify the names of reactants and products.Ex) Sodium metal reacts with chlorine gas to form sodium
chloride
Sodium + Chlorine sodium chloride 2. Substitute the correct symbols and formulas
Na (s) + Cl2 (g) NaCl (s)
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Keep it going!
3. Balance the number of atoms of each element by changing coefficients only!•subscripts MAY NOT be changed for a chemical, this will change the identity of the substance
___Na (s) + ___Cl2 (g) ___ NaCl (s)4. count the number of atoms of each element to be sure the equation is balanced.
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Helpful Hints
• When polyatomic ions appear the same on both sides of the equation, count them as only one item
When water is formed or decomposed from hydrogen and a hydroxide ion, write the water in as HOH
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ExampleAluminum + hydrogen nitrate Aluminum nitrate + hydrogen
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Example
Na + H2O H2 + NaOH
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Example
MgCl2 + Na2CO3 MgCO3 + NaCl
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Types of Chemical Reactions1. Synthesis Rxns (combination) – two or
more substances combine to form a single new substance
General formula: A + B → AB
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Synthesis Reaction ExamplesMg(s) + O2(g) MgO(s)
Na(s) + S(l)
CaO(s) + H2O(l)
SO3(g) + H2O(l)
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2. DecompositionDef: a single compound is broken down into
two or more products
General formula: AB → A + B
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Decomposition Reaction Examples
[electrolysis] electricity
H2O (l) H2(g) + O2(g) electricity
NaCl (l)
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Decomposition Reaction Examples
Decomposition of carbonates Heat, D
CaCO3(g) CaO(s) + CO2(g)
heat
Sodium carbonate
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Decomposition Reaction Examples
Decomposition of metal hydroxidesheat
Mg(OH)2(s) MgO(s) + H2O(l)
heat
Ba(OH)2
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Decompostion of metal chlorates
heat
NaClO3(s) NaCl(s) + O2(g)
heat
KClO3
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3. Single Replacement RXNSDef: one element replaces a second element in
a compound
• metals replace metals
• nonmetals replace nonmetals
General Formula: A + BC → AC + B
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How does it work?
• check Table J – Activity series• more active metals replace less active metals • (elements can only replace other elements
that are lower on Table J)• more active nonmetals replace less active
nonmetals
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Metals replacing less active metals
Mg(s) + Zn(NO3)2(aq) Mg(NO3)2(aq) + Zn(s)
Zn(s) + AgNO3(aq)
Zn(s) + CaSO4
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Replacement of halogens
Cl2(g) + KI(s) I2(s) + NaF
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Replacement of H in water by a metal
K(s) + H2O
Replacement of hydrogen in an acid by a metal
Zn(s) + HCl(aq)
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4. Double replacement reactions Def: involves the exchange of positive ions
between two reacting aqueous compounds
General Formula: AB + CD → AD + CBproducts typically include:• a precipitate (nearly insoluble compound)• an insoluble gas (bubbles out of solution)• a molecular compound (usually water)
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ExamplesPb(NO3)2(aq) + KI(aq) PbI(s) +
2KNO3(aq) FeS(s) + HCl NaCl + AgNO3 HNO3 + KOH
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Predict the products andBalance this puppy!
Ba(OH)2 + H3PO4 →
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5. Combustion RxnsDef: an element or a compound reacts with
oxygen producing heat and light
hydrocarbons burn completely to form water and carbon dioxide
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ExamplesC2H6(g) + O2(g)
C8H18 + O2
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Mass Relationships in Chemical Reactions
• Stoichiometry is the term used to describe the mass relationships in chemical reactions.
The coefficients in a balanced chemical equation represent the mole to mole ratio of the reactants and products
• the relative amount of reactant needed or product formed in a chemical reaction can be determined by stoichiometry (the equation acts like a recipe for the reaction that takes place)
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N2 + H2 → NH3
After balancing the equation, how many moles of H2 are consumed in the reaction? ____
How many moles of NH3 are produced? _____
Therefore, there is a ______ : _______ ratio of H2 to NH3.
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Calculating the # of moles consumed or produced according to a chem equation:
1. Balance the equation.2. Write the given quantity from the question
above that substance in the equation. Place an X above the substance that you are trying to find.
3. Establish a ratio of the given quantity to the balanced coefficient for each substance in question.
4. Cross multiply to solve for X.
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N2 + H2 → NH3
If 2 moles of N2 react completely:a. How many moles of hydrogen must react?
b. How many moles of ammonia will be produced?
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C2H6 + O2 CO2 + H2O
a. How many moles of CO2 are produced when 1 mole of ethane (C2H6) is consumed?
b. How many moles of O2 are consumed when 5
moles of water are produced?
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The following balanced equation shows the complete combustion of octane. Gasoline is a complex mixture of many chemicals. For the purpose of this calculation, we will assume that gasoline is comprised entirely of a compound called octane.
2 C8H18 + 25 O2 → 16CO2 + 18H2O
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2 C8H18 + 25 O2 → 16CO2 + 18H2O
• How many moles of octane (C8H18) are there in 10.0 gallons (26,714g)?
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2 C8H18 + 25 O2 → 16CO2 + 18H2O
• Use the balanced equation to determine how many moles of CO2 are produced when all of the octane in the previous question is completely consumed?
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When 2.0 mol of octane are burned 10943 kj of heat are
produced. How many grams of water at 100 degrees Celsius can
be boiled?