Describing Chemical Reactions
On May 6, 1937, the huge airship Hindenburg
erupted into a fireball.
Within a short time, 21...
Basic chemical equation format
Reactants Products
yields
Word Equations use chemical names
bleach + ammonia  poisonous gas
write the formulas of the reactants
to the left of the yields sign (arrow)
and the formulas of the products to
the right.
...
An unbalanced(skeleton) equation
does not indicate the relative
amounts of the reactants and
products.
Here is the unbalan...
Methane + Oxygen  Carbon dioxide + Water
CH4 + O2  CO2 + H2O
A catalyst is a substance that
speeds up the reaction but is not
used up in the reaction.
Without Catalyst With Catalyst
Special conditions, including use
of a catalyst, are written above
the arrow
H2O2 H2O + O2
KI
Writing Chemical Equations
Complete chemical equations
show the state of matter
(in parenthesis) after each
formula.
NaCl (s )
H2O (l )
O2 (g )
iron + oxygen → iron(III) oxide
Fe(s) + O2(g)  Fe2O3(s)
Hydrogen Peroxide  Water and Oxygen
H2O2(aq)  H2O(l) + O2(g)
Chemical equations are not
complete unless they are
BALANCED.
To write a balanced equation add
the coefficients that will show the
reaction obeying the law of
conservation of mass.
PRO...
Coefficients are small whole
numbers that are placed in front
of the formulas in an equation in
order to balance it.
subsc...
subscriptscoefficients
NEVER change subscripts
In a balanced equation each side
of the equation has the same
number of atoms of each element
and mass is conserved.
1. Propane gas reacts with oxygen to
produce water vapor and carbon
dioxide. Choose the correct word
equation for this rea...
2. What coefficient for H2SO4 is required to
balance the following equation?
Ca3(PO4)2 + ____ H2SO4 → 3CaSO4 + 2H3PO4
a. 1...
Lecture 11.1- Balancing Equations
Lecture 11.1- Balancing Equations
Lecture 11.1- Balancing Equations
Lecture 11.1- Balancing Equations
Lecture 11.1- Balancing Equations
Lecture 11.1- Balancing Equations
Lecture 11.1- Balancing Equations
Lecture 11.1- Balancing Equations
Lecture 11.1- Balancing Equations
Lecture 11.1- Balancing Equations
Lecture 11.1- Balancing Equations
Lecture 11.1- Balancing Equations
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Lecture 11.1- Balancing Equations

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Section 11.1 lecture for Honors & Prep Chemistry

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  • Three common chemical reactions are shown. a) When methane gas burns, it combines with oxygen to form carbon dioxide and water. b) Iron turns to red-brown rust (iron(III) oxide) in the presence of oxygen in the air. c) Hydrogen peroxide decomposes to water and oxygen when used as an antiseptic.
  • Hydrogen peroxide decomposes to form water and oxygen gas. a) Bubbles of oxygen appear slowly as decomposition proceeds. b) With the addition of the catalyst manganese(IV) oxide (MnO2), decomposition speeds up. The white “smoke” is condensed water vapor.
  • Three common chemical reactions are shown. a) When methane gas burns, it combines with oxygen to form carbon dioxide and water. b) Iron turns to red-brown rust (iron(III) oxide) in the presence of oxygen in the air. c) Hydrogen peroxide decomposes to water and oxygen when used as an antiseptic.
  • Three common chemical reactions are shown. a) When methane gas burns, it combines with oxygen to form carbon dioxide and water. b) Iron turns to red-brown rust (iron(III) oxide) in the presence of oxygen in the air. c) Hydrogen peroxide decomposes to water and oxygen when used as an antiseptic.
  • Conceptual Problem 11-3
  • Lecture 11.1- Balancing Equations

    1. 1. Describing Chemical Reactions On May 6, 1937, the huge airship Hindenburg erupted into a fireball. Within a short time, 210,000 cubic meters of hydrogen had burned and the airship was destroyed. The chemical reaction that occurred is “hydrogen combines with oxygen to produce water.”
    2. 2. Basic chemical equation format Reactants Products yields
    3. 3. Word Equations use chemical names bleach + ammonia  poisonous gas
    4. 4. write the formulas of the reactants to the left of the yields sign (arrow) and the formulas of the products to the right. To write a chemical equation H2 + O2  H2O Reactants Product
    5. 5. An unbalanced(skeleton) equation does not indicate the relative amounts of the reactants and products. Here is the unbalanced equation for rusting: Fe + O2  Fe2O3 Why is it unbalanced?
    6. 6. Methane + Oxygen  Carbon dioxide + Water CH4 + O2  CO2 + H2O
    7. 7. A catalyst is a substance that speeds up the reaction but is not used up in the reaction. Without Catalyst With Catalyst
    8. 8. Special conditions, including use of a catalyst, are written above the arrow H2O2 H2O + O2 KI
    9. 9. Writing Chemical Equations
    10. 10. Complete chemical equations show the state of matter (in parenthesis) after each formula. NaCl (s ) H2O (l ) O2 (g )
    11. 11. iron + oxygen → iron(III) oxide Fe(s) + O2(g)  Fe2O3(s)
    12. 12. Hydrogen Peroxide  Water and Oxygen H2O2(aq)  H2O(l) + O2(g)
    13. 13. Chemical equations are not complete unless they are BALANCED.
    14. 14. To write a balanced equation add the coefficients that will show the reaction obeying the law of conservation of mass. PRODUCTSREACTANTS
    15. 15. Coefficients are small whole numbers that are placed in front of the formulas in an equation in order to balance it. subscripts coefficient 2H2 + O2  2H2O NEVER change subscripts
    16. 16. subscriptscoefficients NEVER change subscripts
    17. 17. In a balanced equation each side of the equation has the same number of atoms of each element and mass is conserved.
    18. 18. 1. Propane gas reacts with oxygen to produce water vapor and carbon dioxide. Choose the correct word equation for this reaction. a. propane + carbon dioxide → water + oxygen b. propane + oxygen + water → carbon dioxide c. propane + oxygen + water + carbon dioxide d. propane + oxygen → water + carbon dioxide
    19. 19. 2. What coefficient for H2SO4 is required to balance the following equation? Ca3(PO4)2 + ____ H2SO4 → 3CaSO4 + 2H3PO4 a. 1 b. 2 c. 3 d. 4
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